Match the laws given in Column I with expressions given in Column II.
| Column I | Column II | ||
|---|---|---|---|
| A. | Raoult's law | 1. | $\Delta T_f=K_f m$ |
| B. | Henry's law | 2. | $\pi=CRT$ |
| C. | Elevation of boiling point | 3. | $p=x_i p^\circ_1+x_2p^\circ_2$ |
| D. | Depression in freezing point | 4. | $\Delta T_b=K_b m$ |
| E. | Osmotic pressure | 5. | $p=K_H . x$ |
A. $\rightarrow$ (3) B. $\rightarrow$ (5) C. $\rightarrow$ (1) D. $\rightarrow$ (1) E. $\rightarrow(2)$
A. Raoult's law Mathematical representation of Raoult's law
$$p=x_1 p_1^{\circ}+x_2 p_2^{\circ}$$
B. Henry's law $p=K_H \cdot x$
C. Elevation of boiling point Mathematical representation, $\Delta T_b=K_b \cdot m$
D. Depression in freezing point Mathematical representation, $\Delta T_f=K_f \cdot m$
E. Osmotic pressure Mathematical representation, $\pi=C R T$.
Match the terms given in Column I with expressions given in Column II.
| Column I | Column II | ||
|---|---|---|---|
| A. | Mass percentage | 1. | $\frac{\text{Number of moles of the solute component}}{\text{Volume of solution in litres}}$ |
| B. | Volume percentage | 2. | $\frac{\text{Number of moles of a component}}{\text{Total number of moles of all the components}}$ |
| C. | Mole fraction | 3. | $\frac{\text{Volume of the solute component in solution}}{\text{Total volume of solution}}\times100$ |
| D. | Molality | 4. | $\frac{\text{Mass of the solute component in solution}}{\text{Total mass of the solution}}\times100$ |
| E. | Molarity | 5. | $\frac{\text{Number of moles of the solute components}}{\text{Mass of solvent in kilograms}}$ |
$\begin{array}{llll}\text { A. } \rightarrow(4) & \text { B. } \rightarrow(3) & \text { C. } \rightarrow(2) & \text { D. } \rightarrow(5) \\ \text { E. } \rightarrow(1)\end{array}$
| Column I (Concentration terms) |
Column II (Mathematical formula) |
||
|---|---|---|---|
| A. | Mass percentage | 1. | $\frac{\text{Mass of the solute component in solution}}{\text{Total mass of the solution}}\times100$ |
| B. | Volume percentage | 2. | $\frac{\text{Volume of the solute component in solution}}{\text{Total volume of solution}}\times100$ |
| C. | Mole fraction | 3. | $\frac{\text{Number of moles of a component}}{\text{Total number of moles of all the components}}$ |
| D. | Molality | 4. | $\frac{\text{Number of moles of the solute components}}{\text{Mass of solvent in kilograms}}$ |
| E. | Molarity | 5. | $\frac{\text{Number of moles of the solute component}}{\text{Volume of solution in litres}}$ |
Assertion (A) Molarity of a solution in liquid state changes with temperature.
Reason (R) The volume of a solution changes with change in temperature.
Assertion (A) When methyl alcohol is added to water, boiling point of water increases.
Reason (R) When a volatile solute is added to a volatile solvent elevation in boiling point is observed.
Assertion (A) When NaCl is added to water a depression in freezing point is observed.
Reason (R) The lowering of vapour pressure of a solution causes depression in the freezing point.