Following are the different types of solutions with examples:

 

Concentration is an important factor that determines the strength of a solution. There are two ways to explain the concentration of a solution. One is a qualitative method, and the other is a quantitative method. 

The qualitative way to describe the concentration of a solution is either you can call it concentrated or diluted. However, in order to determine how concentrated exactly is the concentrated solution, we need a quantitative definition. 

When we talk about the strength of a solution, we look at the amount of dissolved solute per unit of solvent. There are various methods for determining the strength of a solution. These include: 

1. Mass Percentage 

The mass percentage refers to the mass of a component in a solution of 100g. To determine mass percentage, use the following formula:

The mass percent of a component = Mass of component in the solution/Total Mass of the solution ×100

 

2. Volume Percentage

Volume percentage refers to the volume of a component in 100 ml of a solution. To determine volume percentage, use the following formula:

The volume percent of a component = Volume of component/Total Volume of the solution ×100

 

3. Mass by Volume Percentage 

Mass by volume percentage refers to the mass of the solute in grams in a solution of 100 ml. To determine mass by volume percentage, use the following formula:

Mass by volume percent = mass of solute in grams/volume of solution in mL×100

 

4. Parts Per Million (ppm)

Formula: 

Parts per million = number of parts of the component/Total Number of components of the solution ×106

In parts per million, volume to volume, mass to volume, and mass to mass are the three ways to express concentration.

 

5. Mole Fraction 

Mole fraction refers to the number of moles of a solute in a solution of one mole. To determine mole fraction, use the following formula:

Mole fraction = number of moles of the component/Total number of moles of all the components 

 

6. Molarity, M

Molarity M refers to the number of moles of solute in a solution of 1 litre. The representation for molarity is molar or MM, as its unit is in milligrams per litre. To determine molarity M, use the following formula:

Molarity, M= Moles of solute/volume of the solution in a litre

 

7. Molality, m

Molality, m refers to the number of moles of solute in a solvent of one kilogram. The representation for molality is molal or m, as its unit is mol per kg. To determine molality m, use the following formula:

Molality, m= Moles of solute/Mass of solvent in kg

We use a solution's colligative properties to find the molecular weight of compounds. It is important to note that this method is helpful to find molar masses of complex polymers, proteins, and molecules. Colligative properties include:

 

Boiling Point Elevation

Boiling point elevation is a phenomenon that indicates that with the mixture of another compound, the boiling point of a liquid can elevate. 

This change in breaking point correlates with molal centralization in a solute. Thus, the formula is:

ΔTb=Kbm

Where,

Kb = Boiling Point Elevation Constant

ΔTb = elevation in boiling point

m = molal concentration of the solution 

 

Depression Of Freezing Point

Depression of freezing point helps determine the molar masses, like the ennobling of boiling point. So, the expression becomes:

ΔTf=Kbm

Where,

Kb = Freezing Point Constant

ΔTf = depression of freezing point

m = molal concentration of the solution

 

Osmotic Pressure

Osmotic pressure refers to the minimal effort needed to forestall internal progression. It is concerned with pure solvent instead of a semipermeable layer. The formula is:

π=CRT

Where,

C= Molar concentration of the solution

π =osmotic pressure

T= Temperature

R= Universal gas constant

 

Van T Hoff Factor 

Van T Hoff factor quantifies osmotic pressure, the boiling point elevation, depression of freezing point. These are cardinal colligative properties. Therefore, the Van T Hoff factor formula is:

i=alpha n+(1- alpha)

Where –

alpha- degree of dissociation

i- Van T Hoff Factor

n- the number of ions formed from one formula

Here are the NCERT solutions for class 12 chemistry, chapter 2:

 

 

 

 

 

1. Which topics are essential from an exam point of view in chapter solutions for class 12 Chemistry?

The essential topics from exam point of view in chapter solutions for class 12 Chemistry include the following:

• • Ideal and Nonideal Solutions
  • Abnormal Molar Masses
  • Vapour Pressure of Solutions of Solids in Liquids
  • Elevation of Boiling Point
  • Depression of Freezing Point
  • Vapour Pressure of Liquid Solutions
  • Raoult's Law as a case of Henry's Law
  • Solubility
  • Relative Lowering of Vapour Pressure
  • The solubility of a Solid in a Liquid
  • Expressing Concentration of Solutions
  • The solubility of a Gas in a Liquid
  • Types of Solutions
  • Vapour Pressure of Liquid-Liquid Solutions
  • Colligative Properties and Determination of Molar Mass
  • Osmosis and Osmotic Pressure

 

2. How beneficial are chapter solutions for class 12 Chemistry in the first semester?

Chapter solutions for class 12 chemistry play a crucial role in the first term of your schooling. This chapter called ‘solutions’ gives an in-depth understanding of physical chemistry. Thus, it acts as the base for your competitive examinations. 

3. What is a solution?

A solution is made after mixing a solute into a solvent. So it means that any combination of a homogeneous substance with two or more segments is a solution. The term solution can refer to solid, liquid or gaseous forms.