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A solution is a homogenous mixture that contains a solvent and a solute. A solvent is that substance which is present in the larger amount in solution and solute is a substance which is present in a smaller amount. There are some various common examples of solutions that you see in your daily life.
Other than these, there are several other examples as well which are very common for household purposes:

Saltwater is formed when we mix salt in water.
Vinegar is obtained when we mix acetic acid in water.
Tincture of iodine is formed when we dissolve crystals of iodine in alcohol.
Mouthwash consists of a number of chemicals dissolved in water.

Important Topics of Chapter Solution

Types of solutions
Solubility
Vapour pressure of liquid solutions
Raoult's law
Ideal and non-ideal solutions
Colligative properties
Abnormal molar mass

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Overview of Chapter

There are various kinds of binary solutions exist in nature as given in the table below:

Types of Solutions	Solvent	Solute	Examples
Gaseous	Gas	Gas	Mixture of Oxygen and Nitrogen
	Gas	Liquid	Humidity
	Gas	Solid	Camphor in Nitrogen gas
Liquid	Liquid	Gas	Carbon dioxide in Water
	Liquid	Liquid	Milk dissolved in water
	Liquid	Solid	Sugar dissolved in water
Solid	Solid	Gas	Hydrogen in Palladium
	Solid	Liquid	An amalgam of mercury with sodium
	Solid	Solid	Brass (an alloy of copper and zinc)

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In this chapter, there are various important topics that you must understand completely:

(i) Solubility: The maximum ability of a substance to get completely dissolved in a solvent. When the solute is solid and the solvent is liquid, then the only temperature affects the solubility. With the increase in temperature, the solubility increases. But pressure has no effect in this case as both solids and liquids are incompressible. But is the solute is gas, then pressure also is an important factor that plays major role insolubility. For this case, Henry's law is given which states that - "At constant temperature, the solubility of a gas is directly proportional to the partial pressure of a gas present above the solution".

(ii) Vapour pressure of liquid solutions: In this concept, you learn that the vapour pressure of volatile liquids in solution when taken in a closed vessel. This phenomenon is explained by Raoult's law, which states that - "The vapour pressure of each volatile liquid present in the solution is directly proportional to the mole fraction of that liquid present in solution".
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Mathematically, Raoult's law can be expressed as follows:

$p_{total}\: =\: p_{1}^{0}\: +\: (p_2^{0}\: +\: p_{1}^{0})x_{2}$
where, vapour pressure of pure component 1
$p_{2}^{0}$ = vapour pressure of pure component 2
$x_{2}$ = mole fraction of component 2
(iii) Ideal and non-ideal solutions: Ideal solutions are those solutions which obey Raoult's law at all ranges of concentrations. Whereas the non-ideal solutions are those which do not obey Raoult's law at all range of concentrations. The vapour pressure of non-ideal solutions are always higher or lower than as predicted by Raoult's law and thus we say that the solution is exhibiting the positive or negative deviation, respectively.
non%20ideal%20solution
(iv) Colligative properties: The properties of solutions which depend only on the number of solute particles present in the solution are known as colligative properties.
colligative%20properties

Relative lowering of vapour pressure: The actual vapour pressure of a solvent in a solution is less than that of the pure solvent. Raoult explained this behaviour and established that this lowering of vapour pressure depends only on the concentration of the solute particles. Mathematically, it can be expressed as follows:
$\frac{\Delta p_{1}}{p_{1}^{0}}\, =\, \frac{p_{1}^{0}-p_{1}}{p_{1}^{0}}\, =\, x_{2}$
Elevation of the boiling point: The boiling point is the point of temperature when the vapour pressure of a substance is equal to the atmospheric pressure. This also depends upon the number of solute particles present in the solution.

Mathematically, it can be expressed as follows: $\Delta T_{b}\, =\, K_{b}m$
K_b= Boiling point elevation constant

Depression of freezing point:

Abnormal Mass: This concept says, that when a solute is dissolved in a liquid then the solute does not dissociate completely as expected instead it dimerizes and thus the molar mass of solute become double. Such deviation of molar mass from the actual value is known as abnormal molar mass.

To deal with the case of an abnormal mass, a Vant Hoff factor was introduced in 1880, which mathematically is described as follows:

$i\: =\: \frac{Normal\: Molar \: Mass}{ Abnormal \: Molar \: Mass}$

How to prepare for Solutions

This chapter is a part of the physical chemistry and it is very important from the numerical point of view. The theory part is less but you simply need to work with the formulas and questions of this chapter.
There are some common terms are used in this chapter like vapour pressure and mole fraction, so before coming to this chapter, first, you must finish the two basic chapters - "Mole concept" and "Gaseous state".
You must have completely memorized all the formulas and must have the very good hold in solving the numericals.
Usually, this chapter is liked by most of the students as it is very easy and straightforward. This chapter holds a good weight ok marks in Boards exams as well as in competitive exams like JEE and NEET.

NCERT Solutions Subject wise link:

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Prescribed Books for Solutions

For this chapter, first, you need to finish the theory thoroughly from class 12th NCERT book and then simultaneously solve the examples and questions given in the book. Apart from this, if you want to prepare for the advanced level for competitive exams like JEE and NEET, you must prepare from the books - O.P. Tandon and R.C Mukherjee. Meanwhile, in the preparation, you must continuously write the mock tests for the depth of knowledge. Our platform will help you to provide with the variety of questions for deeper knowledge with the help of videos, articles and mock tests.

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