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8.3: Concentrations of Solutions (Problems)

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PROBLEM \(\PageIndex{1}\)

What mass of a concentrated solution of nitric acid (68.0% HNO 3 by mass) is needed to prepare 400.0 g of a 10.0% solution of HNO 3 by mass?

PROBLEM \(\PageIndex{2}\)

What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?

PROBLEM \(\PageIndex{3}\)

What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.

\(\mathrm{114 \;g}\)

PROBLEM \(\PageIndex{4}\)

The hardness of water (hardness count) is usually expressed in parts per million (by mass) of \(\ce{CaCO_3}\), which is equivalent to milligrams of \(\ce{CaCO_3}\) per liter of water. What is the molar concentration of Ca 2+ ions in a water sample with a hardness count of 175 mg CaCO 3 /L?

\(1.75 \times 10^{−3} M\)

PROBLEM \(\PageIndex{5}\)

A throat spray is 1.40% by mass phenol, \(\ce{C_6H_5OH}\), in water. If the solution has a density of 0.9956 g/mL, calculate the molarity of the solution.

PROBLEM \(\PageIndex{6}\)

Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?

\(\mathrm{2.38 \times 10^{−4}\: mol}\)

PROBLEM \(\PageIndex{7}\)

What are the mole fractions of H 3 PO 4 and water in a solution of 14.5 g of H 3 PO 4 in 125 g of water?

\(X_\mathrm{H_3PO_4}=0.021\)

\(X_\mathrm{H_2O}=0.979\)

PROBLEM \(\PageIndex{8}\)

What are the mole fractions of HNO 3 and water in a concentrated solution of nitric acid (68.0% HNO 3 by mass)?

\(X_\mathrm{HNO_3}=0.378\)

\(X_\mathrm{H_2O}=0.622\)

PROBLEM \(\PageIndex{9}\)

Calculate the mole fraction of each solute and solvent:

• 583 g of H 2 SO 4 in 1.50 kg of water—the acid solution used in an automobile battery
• 0.86 g of NaCl in 1.00 × 10 2 g of water—a solution of sodium chloride for intravenous injection
• 46.85 g of codeine, C 18 H 21 NO 3 , in 125.5 g of ethanol, C 2 H 5 OH
• 25 g of I 2 in 125 g of ethanol, C 2 H 5 OH

\(X_\mathrm{H_2SO_4}=0.067\)

\(X_\mathrm{H_2O}=0.933\)

\(X_\mathrm{HCl}=0.0026\)

\(X_\mathrm{H_2O}=0.9974\)

\(X_\mathrm{codiene}=0.054\)

\(X_\mathrm{EtOH}=0.946\)

\(X_\mathrm{I_2}=0.035\)

\(X_\mathrm{EtOH}=0.965\)

PROBLEM \(\PageIndex{10}\)

• 0.710 kg of sodium carbonate (washing soda), Na 2 CO 3 , in 10.0 kg of water—a saturated solution at 0 °C
• 125 g of NH 4 NO 3 in 275 g of water—a mixture used to make an instant ice pack
• 25 g of Cl 2 in 125 g of dichloromethane, CH 2 Cl 2
• 0.372 g of histamine, C 5 H 9 N, in 125 g of chloroform, CHCl 3

\(X_\mathrm{Na_2CO_3}=0.0119\)

\(X_\mathrm{H_2O}=0.988\)

\(X_\mathrm{NH_4NO_3}=0.09927\)

\(X_\mathrm{H_2O}=0.907\)

\(X_\mathrm{Cl_2}=0.192\)

\(X_\mathrm{CH_2CI_2}=0.808\)

\(X_\mathrm{C_5H_9N}=0.00426\)

\(X_\mathrm{CHCl_3}=0.997\)

PROBLEM \(\PageIndex{11}\)

What is the difference between a 1 M solution and a 1 m solution?

In a 1 M solution, the mole is contained in exactly 1 L of solution. In a 1 m solution, the mole is contained in exactly 1 kg of solvent.

PROBLEM \(\PageIndex{12}\)

What is the molality of phosphoric acid, H 3 PO 4 , in a solution of 14.5 g of H 3 PO 4 in 125 g of water?

PROBLEM \(\PageIndex{13}\)

What is the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO 3 by mass)?

PROBLEM \(\PageIndex{14}\)

Calculate the molality of each of the following solutions:

• 0.710 kg of sodium carbonate (washing soda), Na 2 CO 3 , in 10.0 kg of water—a saturated solution at 0°C

6.70 × 10 −1 m

PROBLEM \(\PageIndex{15}\)

A 13.0% solution of K 2 CO 3 by mass has a density of 1.09 g/cm 3 . Calculate the molality of the solution.

Contributors

Paul Flowers (University of North Carolina - Pembroke), Klaus Theopold (University of Delaware) and Richard Langley (Stephen F. Austin State University) with contributing authors.  Textbook content produced by OpenStax College is licensed under a Creative Commons Attribution License 4.0 license. Download for free at http://cnx.org/contents/[email protected] ).

• Adelaide Clark, Oregon Institute of Technology

Think one of the answers above is wrong? Let us know here .

M 1 V 1 = M 2 V 2 (1.6 mol/L) (175 mL) = (x) (1000 mL) x = 0.28 M

M 1 V 1 = M 2 V 2 (x) (2.5 L) = (1.2 mol/L) (10.0 L) x = 4.8 M

M 1 V 1 = M 2 V 2 (5.00 mol/L) (x) = (0.3 mol/L) (160 + x) 5x = 48 + 0.3x 4.7x = 48 x = 10. mL (to two sig figs)

M 1 V 1 + M 2 V 2 = M 3 V 3 (3.55) (0.250) + (5.65) (x) = (4.50) (0.250 + x) Where x is volume of 5.65 M HCl that is added (0.250 + x) is total resultant volume 0.8875 + 5.65x = 1.125 + 4.50 x 1.15x = 0.2375 x= 0.2065 L Total amount of 4.50 M HCl is then (0.250 + 0.2065) = 0.4565 L Total amount = 456.5 mL

Since the amount of 5.65 M added is not asked for, there is no need to solve for it. M 1 V 1 + M 2 V 2 = M 3 V 3 (3.55) (250) + (5.65) (x − 250) = (4.50) (x) That way, x is the answer you want, the final volume of the solution, rather than x being the amount of 5.65 M solution that is added.

M 1 V 1 + M 2 V 2 = M 3 V 3

(1.80) (40.0) + (0.808) (21.5) = (M 3 ) (40.0 + 21.5) M 3 = 1.45 M

M 1 V 1 + M 2 V 2 = M 3 V 3 (0.445) (2.00) + (x) (3.88) = (0.974) (2.00 + 3.88) 0.890 + 3.88x = 5.72712 3.88x = 4.83712 x = 1.25 M (to three sig figs)

(0.445 mol/L) (2.00 L) = 0.890 moles

(x) (3.88 L) = moles HCl in unknown solution

(0.974 mol/L) (5.88 L) = 5.73 moles

0.890 moles + [(x) (3.88 L)] = 5.73 moles x = 1.25 M (to three sig figs)

(4.49g CuCl 2 ) (1 mole CuCl 2 / 134.45 grams) = 0.033395 moles CuCl 2

(0.033395 moles CuCl 2 ) / (0.0515 liters) = 0.648 M

M 1 V 1 = M 2 V 2 (7.90 M) (133 mL) = (0.648 M) (V 2 ) V 2 = 1620 mL

moles of Br¯ from KBr: (0.55 mol/L) (0.095 L) = 0.05225 mol moles of Br¯ in final solution: (0.65 mol/L) (0.260 L) = 0.169 mol moles Br¯ provided by the BaBr 2 solution: 0.169 − 0.05225 = 0.11675 mol BaBr 2 provides two Br¯ per formula unit so (0.11675 divided by 2) moles of BaBr 2 are required for 0.11675 moles of Br¯ in the solution. molarity of BaBr 2 solution: 0.058375 mol / 0.165 L = 0.35 M

125.6 g / 41.9 g/mol = 3.00 mol

3.00 mol in 1000 mL so 3 x (180/1000) = 0.54 mol in 180 mL

0.54 mol / 0.50 L = 1.08 mol/L = 1.08 M

KCl ⇒ (2.00 mol/L) (0.100 L) = 0.200 mol of chloride ion CaCl 2 ⇒ (1.50 mol/L) (0.0500 L) (2 ions / 1 formula unit) = 0.150 mol of chloride ion. The '2 ions / 1 formula unit' is the problem child. The solution is 1.50 M in calcium chloride, but 3.00 M in just chloride ion. total moles = 0.200 mol + 0.150 mol = 0.350 mol

0.350 mol / 0.150 L = 2.33 M

(2.00 mol/L) (0.100 L) + (3.00 mol/L) (0.0500 L) = (M 3 ) (0.150 L) Note that the CaCl 2 molarity is 3.00 because that is the molarity of the solution from the point-of-view of the chloride ion.

6 g   x –––––––  =  ––––––– 100 mL   425 mL x = 25.5 g We must use sufficient 30.% (w/v) solution to provide 25.5 g of H 2 O 2 .

30 g   25.5 g –––––––  =  ––––––– 100 mL   x x = 85 mL

(85 mL) (1.10 g/mL) = 93.5 mL The density of the solution is required, which necessitates some Internet searching. Here is an example of a site which gives a value for the density.

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Concentration of a Solution

Concentration of Solution is a measure of the amount of solute that has been dissolved in the given amount of solvent. In simple words, it means determining how much of one substance is mixed with another substance. As Concentration is a frequently used term in chemistry and other relevant fields, although it is most commonly used in the context of solutions, where it refers to the quantity of solute dissolved in a solvent. Concentration can be expressed in both qualitative or quantitative (numerically) terms.

Concentration of a Solution Definition

Concentration of a solution is defined as the amount of solute dissolved in the solution. It is given by the ratio of the amount of solute to the amount of solution or solvent sometimes. However, we can express it in percentages, Parts per Million, and several other ways. The concentration of a solution can be expressed both qualitatively and quantitatively which we will see in the below topics. Before learning more about concentration let’s understand some of the general types of solution

Solution of Solid and Liquid

Solutions of solids and liquids involve the dissolution of a solid solute in a liquid solvent or a liquid solute in a liquid solvent. Examples include:

a. Solid in Liquid: Dissolving table salt (NaCl) in water.

b. Liquid in Liquid: Mixing ethanol and water to form a homogeneous solution.

Solution of Gas

Solutions of gases involve the dissolution of a gas in a liquid solvent or another gas. Examples include:

a. Gas in Liquid: Dissolving carbon dioxide (CO 2 ) in water to form carbonated water.

b. Gas in Gas: Mixing different gases, such as oxygen and nitrogen, in the atmosphere to form a homogeneous mixture.

Qualitative Expressions of Concentration

To qualitatively express concentration, a solution can be classified as a dilute solution or a concentrated solution, which are explained as follows:

Dilute Solution

Dilute Solution contains a smaller proportion of solute than the proportion of solvent. For example, if 2 grams of salicylic acid is dissolved in 100 ml of water and in another container, 8 grams of salicylic acid is dissolved in the same amount of water then a 2-gram solution of salicylic acid is a dilute solution compared to 8 grams solution of salicylic acid.

Concentrated Solution

Concentrated Solution contains a much greater proportion of solute than the proportion of solvent. For example, if 2 grams of salicylic acid is dissolved in 100 ml of water and in another container, 8 grams of salicylic acid is dissolved in the same amount of water then 8 grams solution of salicylic acid is a concentrated solution compared to 2 grams solution of salicylic acid.

Figure 1. Dilute (left) and Concentrated (right) solutions

Semi-Qualitative Expressions of Concentration

To semi-qualitatively express concentration, a solution can be classified as a saturated solution or an unsaturated solution , which are explained as follows:

Saturated Solution  

A saturated solution is one in which the greatest quantity of solute is dissolved in a solvent at a given temperature. When a solution reaches saturation, it can no longer dissolve any more solute at that temperature. Undissolved chemicals settle to the bottom. The saturation point is determined as the point at which no more solute can be dissolved in the solvent.

Unsaturated Solution

An unsaturated solution is one that contains less solute than the maximum possible solute it can dissolve before the solution reaches the saturation level. When more solute is dissolved in this solution, there are no residual substances at the bottom, indicating that all of the solutes have been dissolved in the solvent. An unsaturated solution is a chemical solution in which the solute concentration is less than the corresponding equilibrium solubility.

Figure 2. Unsaturated (left) and Saturated (right) solutions

Solubility is defined as the greatest amount of solute that may dissolve in a certain quantity of solvent at a given temperature.

A solution is a liquid that is a homogeneous combination of one or more solutes and a solvent. A typical example of a solution is, sugar cubes added to a cup of tea or coffee. Here, solubility is the characteristic that allows sugar molecules to dissolve.

As a result, the term solubility may be defined as a substance’s (solute’s) ability to dissolve in a particular solvent.

Quantitative Expressions of Concentration

Qualitative expressions of concentration are relative terms, which do not provide the exact concentration of the solution. To characterize the concentrations of various solutions around us in an accurate and precise manner, we require quantitative expressions of concentration.

Generally, concentration is represented in both ways: Concentration = Quantity of Solute / Quantity of Solution or Concentration = Quantity of Solute / Quantity of Solvent

To quantitatively express concentration, we use the following terms:

• Mass Percentage
• Volume Percentage
• Mass by Volume Percentage
• Parts per Million and Parts per Billion

Mole Fraction 

Mass percentage (w/w%).

Mass percentage which is also called weight by weight concentration of solute and is defined as the amount of solute (in grams) present in 100 gm of the solution.

Mass Percentage = (Mass of Solute / Mass of Solution) × 100

Mass percentage has no unit as it is the ratio of the mass of solute and solution.

Volume Percentage (v/v%)

Volume Percentage which is also called volume by volume concentration of solute and is defined as the amount of solute (in ml) present in 100 ml of the solution.

Volume Percentage  = (Volume of Solute / Volume of Solution) × 100

Volume percentage has no unit as it is the ratio of the volume of solute and solution.

Mass by Volume Percentage(w/v %)

It is defined as the amount of solute (in grams) present in the 100ml of the solution.

Mass by Volume Percentage = (Mass of Solute(in gm) / Volume of Solution(in ml) × 100

Unit of mass by volume percentage is gram per milliliter as it is the ratio of the mass of the solute and volume of the solution.

Parts per Million (PPM)

Parts Per Million or PPM is used to measure the very small amount of solute dissolved in the Solvent. Drinking water, air, soils, etc. are the solvents that have very fewer amounts of solutes in them, which can’t be measured in percentage as a percentage only calculates the concentration out of 100. If we represent concentrations of these solvents in percentage it looks like 0.00002 %, which is not an effective way. That’s why parts per million were introduced to make a representation of these concentrations.

PPM of solute = Mass of solute (in milligrams)/Mass of solution(In Kg)

Parts per Billion

Like, Parts per million, Parts Per Billion are also used to represent solute available in trace quantities. Parts Per Billion represents the amount of solute in 1 billion parts of the solution. 

PPB of solute = Mass of solute (in micrograms)/Mass of solution(In Kg)

Molarity of a given solution is defined as the number of moles present in the 1 liter of solution. For example, if 2 moles of NaCl are dissolved in 1 liter of water, the molarity of the resulting solution would be 2M, and the Formula for Molarity is given as follows:

Molarity (M) = Moles of solute /Volume of solution(in Liter)

Molality of a given solution is defined as the number of moles present in 1 kg of solution. For example, if 3 moles of KOH are dissolved in 3 Liters of water (density of water 1 kg/L), the molality of the resulting solution would be 1 m, as there is 1 mole of KOH present in each Kg of water. The formula for molality is given as follows:

Molality (m) = Moles of solute / Mass of solvent(in Kg)

Mole fraction i.e., X is defined as the ratio of the number of moles of one component to the total number of moles present in the solution. It is a dimensionless quantity. The mole fraction of solute A in a solution containing n components such as A, B, C, . . ., N can be calculated using the following formula:

Mole fraction of A (X A ) = Moles of A / (Moles of A + Moles of B + . . . + Moles of N)

The mole fraction of other solvents (B, C, D, . . .N) in a solution can be calculated using a similar formula.

Normality is a measure of concentration equivalent to the number of equivalents per liter of solution. It is often used for reactions that involve acid-base neutralization, precipitation reactions, or redox reactions, and it takes into account the stoichiometry of the reaction.

Normality (N) = Equivalents of solute / Volume of solution in liters

For example, for an acid-base reaction, normality can be calculated using:

Normality = Molarity × Basicity or Acidity of the compound

Where basicity or acidity is the number of hydrogen ions (H⁺) or hydroxide ions (OH⁻) that can be released per molecule of the compound.

Formality is similar to molarity in that it measures the number of moles of solute per liter of solution. However, formality is used when the solute undergoes a reaction or dissociation in solution. Formality measures the concentration based on the initial composition of the solution, not the final dissolved state.

Formality (F) = Moles of solute / Volume of solution in liters

Temperature Dependence of Quantitative Expressions of Concentration

The following table shows the temperature dependence of the Quantitative Expressions of Concentration.

Mole Concept Heterogeneous and Homogeneous Mixtures Ideal and Non-Ideal Solutions

Sample Problems on Concentration of Solution

Problem 1: 15 g of common salt is dissolved in 400 g of water. Calculate the concentration of the solution by expressing it in Mass by Mass percentage (w/w%).

Given that, Mass of solute (common salt) = 15 g    …(1) Mass of Solvent (water) = 400 g    …(2) It is known that,  Mass of Solution = Mass of Solute + Mass of Solvent    …(3) So,  Substituting (1) and (2) in (3), we obtain the following, Mass of Solution = 15 g + 400 g = 415 g    …(4) From Figure 4, we know Mass by Mass Percentage = ( Mass of Solute / Mass of Solution ) × 100    …(5) Substituting (1) and (4) in (5), we obtain the following, Mass by Mass Percentage = ( 15 g / 415 g ) × 100 = ( 0.0361 ) × 100 = 3.61 Answer is: ( w / w % ) = 3.61

Problem 2: 15 g of common salt is dissolved in a solution of 300 mL, calculate the Mass by Volume percentage (w/v%).

Given that, Mass of solute (common salt) = 15 g     . . . (1) Mass of Solution (salt solution) = 300 mL    . . . (2) From Figure 5, we know Mass by Volume Percentage = ( Mass of Solute / Volume of Solution ) × 100   . . . (3) Substituting (1) and (2) in (3), we obtain the following, Mass by Volume Percentage = ( 15 g / 300 mL ) × 100 = ( 0.05 ) × 100 = 5 g/mL Answer is: ( w / v % ) = 5 g/mL

Problem 3: Richard dissolved 70 g of sugar in 750 mL of sugar solution. Calculate the Mass by Volume percentage (w/v%).

Given that, Mass of solute (common salt) = 70 g    . . . (1) Mass of Solution (salt solution) = 750 mL     . . . (2) From Figure 5, we know Mass by Volume Percentage = ( Mass of Solute / Volume of Solution ) × 100     . . . (3) Substituting (1) and (2) in (3), we obtain the following, Mass by Volume Percentage = ( 70 g / 750 mL ) * 100 = ( 0.933 ) × 100 = 93.3 g/mL Answer is: ( w / v % ) = 93.3 g/mL

Problem 4: What is the molarity of a solution containing 0.5 moles of NaCl dissolved in 500 mL of water?

Given, Moles of NaCl = 0.5, Volume of Solution = 500 mL = 0.5 Liter As, Molarity (M) = moles of solute / liters of solution ⇒ M = 0.5 moles / 0.5 liters = 1 M So the molarity of the solution is 1 M.

Problem 5: What is the molality of a solution containing 20 g of glucose dissolved in 500 g of water?

Given: Mass of Glucose = 20 g, Mass of water = 500 g = 0.5 kg,  Molar mass of glucose (C 6 H 12 O 6 ) = 180 g/mol Number of Moles = Mass/Molar Mass ⇒ Moles of Glucose = 20 / 180 = 1/9 ≈ 0.111 moles of glucose As, Molality (m) = moles of solute / kilograms of solvent ⇒ m = 0.111 / 0.5 = 0.222 mol/kg So the molality of the solution is 0.222 mol/kg.

Problem 6:How many moles of HCl are present in 250 mL of a 0.2 M HCl solution?

Given: Molarity of solution = 0.2 M, Volume of solution = 250 mL = 0.25 liters Molarity (M) = moles of solute / liters of solution ⇒ Moles of solute = Molarity x liters of solution ⇒ Moles of HCl = 0.2 M x 0.25 L = 0.05 moles So there are 0.05 moles of HCl present in 250 mL of the solution.

Problem 7:What is the ppm of lead in a sample that contains 20 mg of lead in 10 L of water?

Given : mass of solute(in mg) = 20 mg and Volution of solvent = 10 L Mass of solution = Mass of water = 10 L x 1 Kg/L = 10 Kg (density of water is 1Kg/L or 1g/mL) ppm (parts per million) = Mass of solute(in mg)/Mass of solution (in Kg) ⇒ ppm = 20 / 10 = 2 So the ppm of lead in the sample is 2ppm.

Problem 8: What is the ppb of mercury in a sample that contains 0.01 g of mercury in 1000 L of air?

Given : mass of solute(in mg) = 0.01 g = 10,000 μg and Volution of solvent = 1000 L Mass of solution = Mass of water = 1000 L x 1 Kg/L = 1000 Kg (density of water is 1Kg/L or 1g/mL) ppb (parts per million) = Mass of solute(in μg)/Mass of solution (in Kg) ⇒ ppm = 10000 / 1000 = 10 So the ppm of lead in the sample is 10 ppb.

FAQs on Concentration of Solution

What is solubility, what is a dilute solution.

A dilute solution is solution which contains a smaller proportion of solute as compared to the proportion of solvent.

What is the difference between PPM and PPB?

PPM and PPB are both represents the concentration of very small scale and only difference between them is that PPM is 1000 times greater scale then PPB or PPB is 1000 times smaller scale then PPM i.e., 1 PPM = 1000 PPB

What is the difference between Molarity and Molality?

Molarity is the number of moles of solute per liter of solution, whereas molality is the number of moles of solute per kilogram of solvent.

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• Difference between Rigidity and Fluidity of Matter We know that matter may change form since it is made up of microscopic particles. But what are the properties of these matter particles? What exactly is the science behind it? Let's learn more about them down below. The matter is defined as everything that has mass and takes up space. Different type 5 min read
• Prove That Liquids have No fixed Shape but have a Fixed Volume The liquid state of matter has a fixed size, in terms of the occupied volume. The state of matter occupies constant space or volume. A liquid contains a fixed number of molecules, irrespective of the container it is placed in, in case there is no addition or deletion of the liquid in the container. 3 min read
• Diffusion in Solids, Liquids, and Gases While the meal is being cooked in the kitchen, people may smell the food while sitting in the drawing-room. Because of diffusion in the air, the vapour from the food reaches us and gives us the fragrance of food. People can smell a burning incense stick from a distance. When they burn an incense sti 7 min read
• What is the Unit of Temperature? Temperature is a measure of how hot or cold something is. It is a physical quantity. Temperature can be measured in terms of the kinetic energy of the particles. It defines the rate of movement of particles moving inside a material. It is considered to be an average measure. The higher the temperatu 5 min read
• What is the Relationship Between Celsius and Kelvin Scale of Temperature? Although you may be familiar with the notion of temperature, many people confuse it with heat. Temperature is a measure of how hot or cold one thing is in comparison to another (its thermal energy content), whereas heat is the movement of thermal energy between objects of various temperatures. Tempe 6 min read
• Liquification of Gases Matter is defined as anything that occupies space and has mass. Modern scientists divide matter into two categories: physical properties and chemical properties. The matter is classified as solids, liquids, or gases based on its physical properties. Solids include things like sugar, sand, iron, and 7 min read
• How to demonstrate the Presence of Water Vapour in Air? Water vapour is the most potent of the greenhouse gases in Earth’s atmosphere. The maximum capacity of water vapour that can be contained in the air depends on the temperature of the air. Warm air can contain more water vapour. Water continually keeps on cycling through the atmosphere. It evaporates 5 min read
• What is Plasma and Bose-Einstein Condensate? We are very familiar with the term matter. Everything around us can be considered as a matter. Generally, it's misconceived that the study of matter only involves three states of it which are solid, liquid, and gaseous. But, matter does exist in other forms of states in nature besides these three. T 9 min read

Chapter 2: Is Matter Around Us Pure?

• Mixtures A mixture is a compound that is made up of two more chemical compounds or substances that do not combine together chemically. It is the physical combination of two or more substances that can retain their individual identities while they are mixed to form solutions, suspensions, or colloids. In this 6 min read
• Solution: Properties of Solution A solution is a homogeneous mixture of two or more substances. A solution is formed of two components: the solute and the solvent. The substance dissolved in the solution is called the solute, whereas the component in which the solute is dissolved is known as a solvent. In this article, we will lear 10 min read
• Saturated and Unsaturated Solutions Saturated and Unsaturated Solutions are the types of solutions based on the concentration of solute in the solvent for any given solution. A saturated solution is one that contains the maximum amount of solute capable of being dissolved at a given temperature, whereas unsaturated solutions contain l 7 min read
• Concentration of a Solution Concentration of Solution is a measure of the amount of solute that has been dissolved in the given amount of solvent. In simple words, it means determining how much of one substance is mixed with another substance. As Concentration is a frequently used term in chemistry and other relevant fields, a 14 min read
• Suspensions Suspension is a heterogeneous mixture of a fluid that contains solute particles that are considerably large for the process of sedimentation. Suspensions are considered to be heterogeneous in nature because they contain at least two different substances. The particles in a suspension are easily visi 6 min read
• Colloids Colloids or Colloidal Solution is a type of mixture in which insoluble components are suspended on a microscopic scale in some another component. Colloids are essential components in the daily lives of the common man, as we use or consume colloids and we even don't know. From Jellys to Mayonese to t 11 min read
• How will you distinguish a Colloid from a Solution? A colloid is a mixture in which one material is suspended throughout another substance and contains scattered insoluble particles. The whole mixture is referred to as a colloidal solution. A colloid has a dispersed phase (suspended particles) and a continuous phase, unlike a solution, which has only 7 min read
• Classification of Colloids Before we get into the specifics of how we classify colloids, it's important to first define what a colloid is. A colloid is a material made up of big molecules mixed with another substance in chemistry. This encompasses a wide range of items, many of which you may already have in your house, which 8 min read
• Tyndall Effect Tyndall effect is the scattering of light by a colloid or an extremely tiny solution of particles. It is also known as the Tyndall phenomenon and is similar to Rayleigh scattering, in that the intensity of the scattered light is inversely proportional to the wavelength's fourth power, with blue ligh 6 min read
• Separation of Mixtures Separation of Mixtures or method of separation is the process of separating or extracting different components of a mixture using some physical methods. The type of mixture and variations in the chemical characteristics of the mixture's components determine the separation method to be used. Separati 14 min read
• How to separate a Mixture of Two Solids? As we look at our surroundings, we see many things with different shapes, sizes and textures. Everything in this universe is made up of material which scientists call matter. The air we breathe, the food we eat, stones, clouds, stars, plants and animals, even a small drop of water or a particle of s 8 min read
• Separation by a suitable solvent Many of the substances we come into contact with mix. Two or more chemicals are combined together in these combinations. In other cases, such a blend may not be possible to employ in both households and businesses. For our purposes, we may just need one (or two) distinct elements of a combination. T 5 min read
• Separation of Mixtures using Sublimation and Magnets Sublimation is the separation technique where a substance makes a transition from the solid to the gas state directly. The substance does not undergo the liquid stage. Therefore, it is used to illustrate a solid-to-gas transition between the states of a substance. This process is endothermic in natu 11 min read
• How to Separate a Mixture of a Solid and a Liquid? In our daily life, we use different products. And, always keep in search of pure products as mostly also found written on the packaging of items. But scientifically the term pure is used for those matters which are made up of particles that have the same chemical nature or formation. Hence, the majo 10 min read
• Filtration: Definition, Process, Diagram and Examples Filtration is a method to separate the components of a mixture where the solvent part is liquid and the solute is an insoluble solid. Let's know more about Filtration Definition, Process, Application and examples in detail below. In simple words, Filtration is the process in which solid particles in 5 min read
• Water Purification Water is carried through canals or lengthy pipelines in a water purification system, which contains various pollutants and suspended particles from rivers and lakes. River water is commonly used to supply cities with drinking and dining water. This water is unsafe for drinking or dining because it c 6 min read
• Centrifugation Centrifugation is a technique used to separate components of a mixture based on their size, shape, viscosity and density. It works by spinning the mixture at high speed in a machine called a centrifuge, which creates a force called centrifugal force. This force pushes denser components outward, away 12 min read
• How to Separate Cream from milk? As we look at our surroundings, we see many things with different shapes, sizes and textures. Everything in this universe is made up of material which scientists call matter. The air we breathe, the food we eat, stones, clouds, stars, plants and animals, even a small drop of water or a particle of s 5 min read
• Difference Between Homogeneous and Heterogeneous Mixture Mixture is a combination of two or more substances that are not chemically bonded together. These substances can be elements, compounds, or both. There are two types of mixtures: Homogeneous and Heterogenous Mixture. In homogeneous mixture, components are uniformly distributed and not easily disting 4 min read
• Difference Between Compound and Mixture The matter is divided into three main types Compounds, Mixtures, and Elements. Pure substances are compounds. Impure substances are Mixtures. The key difference between compounds and mixtures is that a compound is made up of molecules, each of which is composed of two or more different types of chem 7 min read
• Factors affecting Solubility A solution is a liquid that is a homogeneous combination of one or more solutes and a solvent. A frequent example of a solution is sugar cubes added to a cup of tea or coffee. Solubility is the characteristic that allows sugar molecules to dissolve. As a result, the term solubility may be defined as 6 min read
• Separation by Evaporation Evaporation is the process of the separation of a solid substance that is dissolved in water. The application is based on the fact that solids do not vaporize easily, whereas liquids do. On performing evaporation, the solid substance is left behind as a residue. It is a vaporization technique where 7 min read
• Crystallization Crystallization is a technique for purification of the substances. It is a technique that separates a solid from its solution. The process in which the solid dissolve in the liquid arranges itself in well-defined 3-D structures called the crystal is called crystallization. When any substance undergo 9 min read
• Chromatography Chromatography is the separation of mixtures by distribution between two or more immiscible phases. In chemical laboratories, where it is used for analysis, isolation, and purification, chromatography is the most used separation technique. It is also frequently used in the chemical process industry 15 min read
• Distillation Distillation is the method of separating mixtures, in which the conversion of a liquid into vapour is afterwards condensed back to liquid form. distillation method is used for the purification of metals. Distillation is preferable where both solid and liquid have to be extracted from the solution. A 9 min read
• Separation of Mixtures of Two or More Liquids Most of the time, the substances we encounter are not in their purest form. They are essentially a chemical synthesis of two or more substances. Surprisingly, mixtures can take on a number of forms. As a result, many types of separation processes are used to separate a mixture of substances. When it 8 min read
• Fractional Distillation Fractional Distillation is a technique used in the separation of miscible liquids. The process requires repeated distillations and condensations of the mixture. The separation of the mixture happens when the mixture is heated at a certain temperature where fractions of the mixture start to vaporize 7 min read
• Pure and Impure Substances Substance is a matter which is associated with a set of definite properties and composition. Every pure compound and element is a substance. Substances are the materials composed of atoms and molecules. Every substance is recognized by a specific weight and volume. It cannot be segregated into other 4 min read
• What is an Element? Element in chemistry are substances that cannot be broken down into simpler substances by any chemical method by the application of heat or light. For instance, melting a piece of gold still remains the gold element. These substances are composed of a singular type of atoms i.e., they are monoatomic 12 min read
• Metals, Non-Metals and Metalloids Matter is defined as any substance that has mass and occupies space by having a volume in classical physics and general chemistry. Daily objects that can be touched are ultimately made up of atoms, which are made up of interacting subatomic particles, and matter refers to atoms and everything made u 8 min read
• Properties of Metals and Non-Metals Metals and Non-metals have different properties and reactivity with other elements. This difference between the physical and chemical properties of elements depends on their position in the periodic table. The physical properties of substances (or elements) include tendencies like conductivity, dens 7 min read

Chapter 3: Atoms and Molecules

• Laws of Chemical Combination Laws of Chemical Combination are one of the most fundamental building blocks of the subject of chemistry. As in our surrounding different matter reacts with each other and form various kind of different substances. Laws of Chemical Combination are the collection of laws that explains how these subst 7 min read
• Law of Conservation of Mass Law of Conservation of Mass: The law of conservation of mass states that the mass can neither be created nor destroyed in a chemical reaction. This implies, in a closed system the mass of the elements involved initially in a chemical reaction is equal to the mass of the product obtained by the react 9 min read
• Verification of the Law of Conservation of Mass in a Chemical Reaction Law of conservation of mass states that "The mass can neither be created nor destroyed in a chemical reaction" French chemist Antoine Lavoisier was the first to state the law of conservation of mass in his book. There is just a rearrangement in the atoms of substances for the formation of compounds. 7 min read
• Law of Constant Proportions We are all aware that matter is made up of atoms. Surprisingly, Greek philosophers proposed the concept of atom in the fifth century BC (BCE). Their notion, however, was philosophical rather than scientific. John Dalton proposed the first scientific theory of the atom. Few of Dalton's atomic postula 10 min read
• What is Atom? Atoms are tiny particles that comprise all the things in the known universe. Atoms of an element are responsible for all chemical reactions occurring in nature. We know that atoms are made up of three fundamental particles namely, ElectronsProtonsNeutronsThese particles are also called subatomic par 8 min read
• Atomic Mass Atomic mass is the total mass of all subatomic particles of an atom, including protons, neutrons, and electrons. However, the mass of electrons is incredibly small, so it's typically neglected when determining an atom's overall mass. The unit commonly used to express atomic mass is the Atomic Mass U 9 min read
• How Do Atoms Exist? If you are going to build a house, you will undoubtedly need to manage a big number of bricks. This is due to the fact that it may be classified as a building component for your well-planned shelter. Similarly, atoms are the basic building units of stuff that surrounds us. Think of anything, and it 8 min read
• Cations vs Anions Ions are charged species that are formed by the transfer of electrons from the outermost shell. Ions are either positive or negative in nature depending on the overall charge of the ion. If an atom loses an electron it has excess proton forming positive ions whereas if an atom gains an electron it h 9 min read
• What are Ionic Compounds? In chemistry we usually come across terms called ions, anions, cations, ionic compounds study of such compounds is a must to understand various concepts. Let us understand why ions are formed generally, atoms are made up of particles called electrons, protons and neutrons. The number of electrons an 7 min read
• What are Monovalent Ions? Ions are a type of ion that is studied in science. Chemistry is made up of atoms and electrons that have gained or lost weight due to the removal or addition of one or more valence electrons, which results in either a positive or a negative charge. Ions with a negative charge are known as anions, wh 5 min read
• What are Divalent Ions? The study and research on the periodic table have come with various conclusions like the discovery of elements, atomic model, the structure of the atom, subatomic particles, etc. By the time there have been notable discoveries by scientists and researchers which made the study much relevant. The the 5 min read
• Trivalent Ions - Cations and Anions The theories proposed till now explains the physical and chemical properties of different elements found.The studies by different scientists have contributed to the expansion of the periodic table and described various other participants of atomic chemistry. Such as molecules, isotopes, ions, radica 5 min read
• Polyatomic Ions An ion is a chemical entity that has a positive or negative charge of a certain magnitude. The term 'ion' can refer to atoms or molecules that have non-zero net charges attached to them. As a result, all ions contain either more protons than electrons in their overall atomic or molecule structure or 6 min read
• Formulas of Ionic Compounds The study of the modern periodic table shows all the elements dhows their own kind of nature. Among them, most of the atoms of the elements cannot exist freely in a stable state. Hence, for the purpose of obtaining stability, they share their valence electron with the atoms of other elements. This s 6 min read
• Chemical Formula Chemical formula is a way to describe chemical ratios of atoms that make up a specific chemical compound or molecule in chemistry. Chemical element symbols, numbers, and sometimes other symbols, such as parentheses, dashes, brackets, commas, plus (+), and minus (-) signs, are used to represent the c 6 min read
• Chemical Formula of Common Compounds Chemical Formulas of compounds are symbolic representations of their chemical composition. They tell us about which elements the chemical compound is made of and in what ratio. In this article, we will learn about the chemical formulae of some common compounds in detail. Table of Content What is Che 6 min read
• Molecular Mass Molecular Mass is the mass of all the atoms present in a molecule. In ancient India and Greece, philosophers have first given the idea of atoms and deeply studied them. Around 500 BC. Everything around is made up of very small units these units are atoms in the language of science, very small in the 10 min read
• Mole Concept Mole concept is the method used to express the amount of substance. This has been experimentally proving that one gram atom of any element, as well as one gram molecule of any substance, contains the same amount of entities. The experimentally decided number is found to be 6.022137 × 1023. After the 10 min read
• Problems Based on Mole Concepts Indian philosopher Maharishi kanad postulated that if a matter is divided into further smaller pieces, it will have smaller parts. However, there shall come a point when the matter no longer can be divided further and that smallest part is called Parmanu. By the end of the 18th century, scientists r 7 min read
• Dalton's Atomic Theory In the year 1808, the English scientist and chemist John Dalton proposed Dalton's atomic hypothesis, a scientific theory on the nature of matter. It asserted that all matter is made up of atoms, which are tiny, indivisible units. According to Dalton's atomic theory, all substances are made up of ato 9 min read
• Drawbacks of Dalton's Atomic Theory The idea of atoms dates back two millennia, long before John Dalton introduced the concept of atoms in 1803. Kanada, an ancient Indian philosopher, discussed the existence of indivisible particles, which he referred to as "anu." The rule of conservation of matter was introduced by French scientist L 6 min read
• Significance of the Symbol of Elements An element in chemistry refers to the purest form of a substance containing only atoms and cannot be broken down further by any means. These elements are classified according to their properties (both chemical and physical) and arranged according to their atomic number (Z) in the modern periodic tab 6 min read
• Difference Between Molecules and Compounds Molecules are the smallest building blocks that form the matter around us. They are the simplest particles that carry the properties of matter. Molecules are joined together to form the Compound. A molecule is the smallest unit of matter formed by joining various atoms together whereas the compounds 6 min read
• How to Calculate Valency of Radicals? To construct the formulas of ionic compounds, we must first understand the valencies of the positive and negative ions that combine to produce the ionic compounds. As a result, we'll start with ion valencies. The valency of an ion is equal to its charge. If an ion has one unit charge, its valency is 5 min read
• What is the Significance of the Formula of a Substance? Everyone may think that if the atom is very tiny in size, what is its importance of it? So, this is because the entire world is made up of atoms and molecules. As known that one cannot see them with the naked eyes but they are always present around. They may be in the surrounding, substances that ev 5 min read
• Gram Atomic and Gram Molecular Mass Avogadro's number is critical to understanding the structure of molecules as well as their interactions and combinations. e.g. because one atom of oxygen will combine with two atoms of hydrogen to form one molecule of water (H2O), one mole of oxygen (6.022 × 1023 of O atoms) will mix with two moles 7 min read

Chapter 4: Structure of the Atom

• Charged Particles in Matter Can we deduce from these actions that rubbing two items together causes them to become electrically charged? The presence of charged particles in an atom was discovered thanks to the efforts of many scientists. By 1900, it was established that the atom was an indivisible particle that contained at l 8 min read
• Thomson's Atomic Model Thomson's Atomic Model is one of the fundamental models of the atom that tries to explain the working and structure of the atom. this model was proposed by famous Scientist JJ Thomson in 1904. Thomson during his cathode ray experiment proved the existence of a negatively charged particle called elec 6 min read
• Rutherford Atomic Model Rutherford Atomic Model was proposed by Ernest Rutherford in 1911. It is also called the Planetary Model of the Atom. It introduced the concept of a dense, positively charged nucleus at the center of an atom, with electrons orbiting around it, forming the basis for modern atomic theory. In this arti 6 min read
• Drawbacks of Rutherford's Atomic Model In Rutherford's Model of the Atom, Rutherford performed an experiment based on that experiment some of the hypotheses are given. At that time those hypotheses are considered revolutionary as there was an experiment to back that hypothesis. But as the experiment performed by Rutherford is rudimentary 10 min read
• Bohr's Model of an Atom Neil Bohr proposed the Bohr model and was based on the modification of Rutherford’s model of an atom. Rutherford's model introduced a nuclear model of an atom in which it was explained that the nucleus which is positively charged is surrounded by negatively charged particles called electrons. Bohr m 7 min read
• Neutrons Neutrons are fundamental subatomic particles of the atom. An atom is made up of electrons, protons and neutrons. James Chadwick, an English physicist, discovered the neutron in 1932. Neutrons are particles with no charge and higher mass. They are represented by n. They reside inside the nucleus of t 8 min read
• Valency Valency of an element is a measure of an atom's ability to combine with other atoms to create molecules or chemical compounds. The characteristics of an element that indicate how many more atoms can join one of its atoms in a covalent bond are known as valence, or valency, in chemistry. The term, wh 9 min read
• Valence Electrons Any of the fundamental negatively charged particles in the outermost area of atoms that participate in the creation of chemical bonds are referred to as valence electrons. Changes in the atomic structure are confined to the outermost, or valence, electrons regardless of the kind of chemical connecti 10 min read
• Mass Number Mass Number of an atom is the total number of protons and neutrons present in an atom. We know that an atom consists of electrons, protons, and neutrons but the mass of the atom is contributed by protons and neutrons as the mass of electrons is very low hence it doesn't contribute to the mass of an 11 min read
• Relation Between Mass Number and Atomic Number Atoms are the fundamental building blocks of matter, and they may combine in a variety of ways to produce various substances. You must be aware that all atoms are made up of electrons, protons, and neutrons. But did you know that the presence of these subatomic particles may explain an element's pro 8 min read
• Isobars Isobars are a group of elements that have the same mass number but different atomic numbers. In an isobar, we have different numbers of protons but the same number of nucleons, i.e. the sum of the number of protons and neutrons in the nucleus of isobars of the elements are the same. An example of is 5 min read
• Why do all the Isotopes of an Element have similar Chemical Properties? The fundamental building units of matter are atoms and molecules. The existence of many types of matter is due to the various atoms that contain them. The atom was no longer seen as a simple, indivisible unit by 1900. It did, however, contain at least one subatomic particle, the electron. J.J. Thoms 6 min read
• Why Isotopes have different Physical Properties? The atom is divided into two parts: the atomic structure and the extra nucleus. Positively charged protons and neutral neutrons make up the atomic structure. Electrons in the extra nucleus are negatively charged. Atoms, like all elements and compounds, have mass. Because of protons, the mass of an a 5 min read
• What is Fractional Atomic Mass? The smallest possible amount of matter which still retains its identity as a chemical element, consisting of a nucleus surrounded by electrons is called an atom. These are the atoms that make up an element. An element is a material with the same number of protons in all of its atoms. Protons, electr 9 min read
• Radioactive Isotopes Radioactive Isotopes or Radioisotopes are the isotopes of the elements that are not stable, i.e. they emit some radiation and change the composition of their nucleus. Radioactive isotopes are defined as the isotopes of any chemical element that have different masses and unstable nuclei and release e 8 min read
• Discovery of Electrons The basic idea of the discovery of the elementary particles was generated by Dalton's Atomic Theory. John Dalton in 1808 gave the first scientific theory about atoms, in which, he stated that atoms are the smallest particle of any matter. They are indivisible and indestructible. According to Dalton 7 min read
• What is a Proton? Protons are the fundamental particles that reside inside the nucleus of any atom. They are the positive charge particle and are responsible for balancing the negative charge of the electron to make the atom electrically neutral. Proton was discovered by the famous scientist Ernest Rutherford. Atoms 6 min read
• Rutherford's Alpha Scattering Experiment Rutherford's Alpha Scattering Experiment is the fundamental experiment done by Earnest Rutherford's Alpha Scattering Experiment that gives the fundamental about the structure of the atom. Rutherford in his experiment directed high-energy streams of α-particles from a radioactive source at a thin she 6 min read
• Atomic Nucleus The nucleus of an atom is a small, dense, round region located in the centre of an atom. It has two subatomic particles, protons and neutrons. Protons are electrically positively charged ions having a mass of approximately one atomic mass unit (amu). Neutrons are electrically neutral. The atomic nuc 11 min read
• How did Neil Bohr explained the Stability of Atom? Bohr model of the atom was explained by Neil Bohr in 1915. It came into existence with the modification of Rutherford’s model of the atom. Rutherford’s model introduces the nuclear model of the atom, in which he explained that a nucleus (positively charged) is surrounded by negatively charged electr 7 min read
• Electron Configuration Electron Configuration of an element tells us how electrons are filled inside various orbitals of the atom. The distribution of electrons inside various orbital of atoms is very useful in explaining various properties of the atoms and their combination with other atoms. The electron configuration of 8 min read
• Potassium and Calcium - Atomic Structure, Chemical Properties, Uses An atom is the smallest part of an element or compound that takes part in a chemical reaction. They are made of tiny particles known as protons, neutrons, and electrons. The Greek philosopher Democritus was the first person to use the term atom. The structure of the atom was discovered by John Dalto 8 min read
• Noble Gas Inert gases are chemically unreactive. Noble gases, also termed inert gases are group 0 elements. There are six types of noble gases, helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radioactive radon (Rn). The noble gases are the type of elements belonging to group 18. Under standa 4 min read
• What is meant by Chemical Combination? The composition of an element's nucleus and the arrangement of electrons around it are referred to as its atomic structure. Protons, electrons, and neutrons are the building blocks of matter's atomic structure. The nucleus of the atom is made up of protons and neutrons, which is surrounded by the at 6 min read
• Difference between Electrovalency and Covalency We're all familiar with how electrons in an atom are organised into orbitals or shells. Valence electrons are the electrons that exist in the atom's outermost orbit. According to the Bohr-bury theory, the outermost shell may hold a maximum of 8 electrons. When the outermost shell is entirely filled, 8 min read
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• Concentration of Solution

An introduction to Concentration of Solution

Everyone talks about the concentration of solutions. They may also talk about the concentration of coffee or tea. Everyone has a particular view of what is meant by the concentration of a solution. You must have noticed that whenever you make coffee, if you add a lot of powder, you will end up with a concentrated drink, whereas if you add little, it will result in a dilute solution. Therefore, it is essential that you understand what the concentration of the solution is. In this chapter, we will learn about what is meant by the concentration of a solution; we will also see how to find the concentration of a solution and the different methods of expressing the concentration of the solution.

What is Concentration of a Solution?

In an aqueous solution, two parts exist, namely solute and solvent. They are the two basic solution concentration terms that you need to know. We always need to keep an account of the amount of solute in the solution. In chemistry, we define the concentration of solution as the amount of solute in a solvent. When a solution has more solute in it, we call it a concentrated solution. Whereas when the solution has more solvent in it, we call it a dilute solution.

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Now that you understand the concept of what is the concentration of solution let's move on to the different methods of expressing concentration.

Methods of Expressing the concentration of Solution

There are various methods of expressing the concentration of a solution. You will usually see Chemists working with the number of moles. Pharmacists will use percentage concentrations instead of the number of moles. Hence it is important to understand all the methods of expressing the concentration of solutions.

The concentration of the solution formula is given as follows.

Concentration of solution = \[\frac{\text{Weight of the solute in gram}}{\text{volume in Litres}}\]

We will also see other methods on how to calculate the concentration of a solution based on the different methods of expressing concentrations.

Concentration in Parts per Million

It is expressed in terms of weight. The formula for parts per million is given as follows:

ppm(A)= \[\frac{\textrm{Mass of A}}{\textrm{Total mass of the solution}}\]x10\[^{6}\]

Mass Percentage (w/w)

It is expressed in terms of mass percentage of solute to the solution. The formula for mass percentage is given as follows.

Mass percentage of A =  \[\frac{\text{Mass of component A}}{\text{Total mass of the soution}}\]x100

e.g. CH 3 COOH 33% w/w, and H 2 SO 4 98.0% w/w.

Volume Percentage (V/V)

It is expressed in terms of the volume percentage of solute to the solvent. The formula for volume percentage is given as follows.

Volume percentage of A = \[\frac{\text{Volume of component A}}{\text{Total volume of the solution}}\]x100

Mass by Volume Percentage (w/V)

Percentage weight in volume expresses the number of grams of solute in 100 ml of product.

e.g. BaCl 2 solution 10% w/v, and H 2 O 2 solution 5-7% w/v.

Molarity (M)

It is the number of moles of solute contained in 1000 ml of solution. It is a commonly used method for expressing concentrations.

Molarity = \[\frac{\text{Mass of solute}}{\text{volume of solution in litres}}\]

Molality (m)

The molality is expressed as the number of moles of a solute contained in 1000 gm of a solvent. The formula for molality is given as follows.

Molality (m) = \[\frac{\text{Mass of solute}}{\text{Mass of solvent in Kg}}\]

Normality (N)

We can define it as the number of equivalents of the solute present in the solution, and it is also called equivalent concentration. The formula for normality is given as follows.

Normality (N) = \[\frac{\text{Weight of solute in grams}}{\text{Equivalent mass} \times \text{Volume in litre}}\]

Mole Fraction:

The mole fraction (X) of a component in a solution is defined as the ratio of the number of moles of that component to the total number of moles of all components in the solution. The mole fraction of A is expressed as X A with the help of the following equation in a solution consisting of A, B, C, … we can calculate X A .

X\[_{A}\] = \[\frac{\text{moles of A}}{\text{mole of A + mole of B + momle of C +.... }}\]

Similarly, we can calculate the mole fraction of B, X B with the help of the following formula.

X\[_{B}\] = \[\frac{\text{moles of B}}{\text{mole of A + mole of B + momle of C +.... }}\]

Now that you know how to find the concentration of a solution using various concentrations of solution formulas, we will try to solve some concentrations of solution questions.

Solved Problems

Question 1) 2 ml of water is added to 4 g of a powdered drug. The final volume is 3ml. Find the mass by volume percentage of the solution?

Answer 1) Given, Mass of solute = 4g

Volume of solution = 3ml

Mass by volume percentage = \[\frac{\text{Mass of solute}}{\text{Volume of solution}}\]x100 = \[\frac{4g}{3ml}\] = 133%

Therefore, the mass by volume percentage is 133 %.

Question 2) Many people use a solution of Na 3 PO 4 to clean walls before putting up wallpaper. The recommended concentration is 1.7 % (m/v). Find the mass of Na 3 PO 4 needed to make 2.0 L of the solution?

Answer 2) Given, 

Mass/Volume percentage = 1.7 %

Volume of Solution = 2000 ml

Mass by volume percentage = \[\frac{\text{Mass of solute}}{\text{Volume of solution}}\] × 100 

1.7 % = \[\frac{\text{Mass of solute}}{2000ml}\] ×100

Mass of solute = 34 g

Therefore, the mass required is 34 g.

In chemistry, we are often required to calculate the concentration of the solution. The above-mentioned methods of expressing the concentration of a solution are important. The solved examples are helpful for a better understanding of the concept of concentration of a solution.

FAQs on Concentration of Solution

1. Does solution concentration change when solution volume changes?

The answer to this question depends on how we define concentration. If we talk about molarity, then yes it does change. If we take concentration by mass into consideration, it will still change, unless the substance is with an undefined density. That's because the mass of a substance will change with its volume, and so the concentration changes. But, if both the solute and solvent are either increasing or decreasing in volume/mass/moles in an equal ratio, the concentration and molarity will remain the same.

2. How do I convert from molarity to a weight percentage?

The first step is to multiply the molarity by the molar mass of the solute to get grams of solute per litre. The second step is to divide the concentration expressed as grams of solute per litre by the density of the solution in grams per litre. Finally, multiply it by 100% to convert it to percentage.