Solutions – Chemistry Smart Booklet

2. SOLUTIONS




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, SOLUTIONS
Introduction:
In this chapter, we will discuss about liquid solutions and their formation. This will be
followed by studying the properties of solutions, like vapour pressure and colligative
properties. We will begin with types of solutions and expressions for concentration of
solutions in different units.

Thereafter, we will state and explain Henry’s law and Raoult’s law, distinguish between
ideal and non-ideal solution and deviation of real solutions from Raoult’s law. We will
also discuss abnormal colligative properties alongwith association and dissociation of
solute.

Types of Solutions




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All the three states of matter (solid, liquid and gas) may behave either as solvent or solute.
When a solution is composed of only two chemical substances, it is termed as binary
solution. Depending upon the state of solute or solvent, binary solutions can be classified
as
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Some Important Definitions

 Mixture - When two or more chemically non-reacting substances are mixed, they
form mixture.

 Heterogeneous Mixture - It consists of distinct phases, and the observed properties
are just the sum of the properties of individual phases.

 Homogeneous Mixture - It consists of a single phase which has properties that
may differ from one of the individual components.

 Solution - The homogeneous mixture of two or more components such that at least
one component is a liquid is called solution.

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,  Solvent - It is the constituent of solution which has same physical state as that of
solution and generally present in greater amount than all the other components.

 Solute - The component of a solution other than solvent is called solute, may or
may not have same physical state as that of solution. Generally it is in smaller
amount.
Example - In a sugar syrup (liquid solution) containing 60% sugar (solid) and 40%
water (liquid), water is termed as solvent, due to same physical state as that of
solution.

Expressing the Strength of Solution
For a given solution the amount of solute dissolved per unit volume of solution is called
concentration of solute. Strength of solution is the amount of solute in grams dissolved in
one litre of solution. It is generally expressed in g/litre.

Other methods of expressing the strength of solution are:




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1. Mass percentage –
Mass of solute
Mass % of solute = × 100
Total mass of solution
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Mass of solvent
Mass % of solvent = × 100
Total mass of solution


2. Volume percentage –
Volume of solute
Volume % of solute = × 100
Total volume of solution
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Volume of solvent
Volume % of solvent = × 100
Total volume of solution



3. Molality (m) - It is no. of moles of solute dissolved in 1 kg of the solvent.
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(Number of moles of solute)
m =
(Mass of solvent *in kg+)



4. Molarity (M) - It is no. of moles of solute dissolved in 1 litre of solution.

(Number of moles of solute)
M =
(Mass of soution *in litre+)

5. Normality (N) - It is no. of gram-equivalents of solute dissolved in 1 litre of solution



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