The correct answer is option 3. 3.
The correct match is 3: A-III, B-V, C-IV, D-I, E-II.
| Column I |
Column II |
| (A) Raoult's law |
(iii) \(p = \chi _1P_1^o + \chi _2P_2^o\) |
| (B) Henry's law |
(v) \(P = K_H \chi\) |
| (C) Elevation of boiling point |
(iv) \(\Delta T_b = K_bm\) |
| (D) Depression in freezing point |
(i) \(\Delta T_f = K_fm\) |
| (E) Osmotic pressure |
(ii) \(\pi = CRT\) |
(A) Raoult's law: Raoult's law relates the vapor pressure of a component in an ideal solution to its mole fraction in the solution. According to Raoult's law, the partial vapor pressure of a component is equal to the product of its mole fraction in the solution and the vapor pressure of the pure component at that temperature. Mathematically, it can be represented as \(p = \chi _1P_1^o + \chi _2P_2^o\), where \(p\) is the total vapor pressure of the solution, \(\chi _1\) and \(\chi_2\) are the mole fractions of the components, and \(P_1^o\) and \(P_2^o\) are the vapor pressures of the pure components (iii).
(B) Henry's law: Henry's law describes the relationship between the concentration of a gas dissolved in a liquid and its partial pressure above the liquid. It states that the concentration of a gas dissolved in a liquid is directly proportional to its partial pressure. The proportionality constant in this relationship is known as the Henry's law constant \((K_H)\). Mathematically, it can be represented as \(P = K_H \chi\), where P is the partial pressure of the gas above the liquid and χ is the molar concentration of the gas in the liquid (v).
(C) Elevation of boiling point: The elevation of boiling point is a colligative property that depends on the concentration of solute particles in a solution. When a nonvolatile solute is added to a solvent, it raises the boiling point of the solvent. The elevation of boiling point can be calculated using the equation \(\Delta T_b = K_bm\), where \(ΔT_b\) is the change in boiling point, \(K_b\) is the molal boiling point elevation constant specific to the solvent, and m is the molality of the solute (iv).
(D) Depression in freezing point: The depression in freezing point is another colligative property that depends on the concentration of solute particles in a solution. When a nonvolatile solute is added to a solvent, it lowers the freezing point of the solvent. The depression in freezing point can be calculated using the equation \(\Delta T_f = K_fm\), where ΔTf is the change in freezing point, \(K_f\) is the molal freezing point depression constant specific to the solvent, and m is the molality of the solute (i).
(E) Osmotic pressure: Osmotic pressure is the pressure exerted by the solvent molecules as they pass through a semipermeable membrane to equalize the concentration of solute on both sides of the membrane. Osmosis is the movement of solvent molecules from an area of lower solute concentration to an area of higher solute concentration. Osmotic pressure can be calculated using the equation \(\pi = CRT\), where π is the osmotic pressure, C is the concentration of the solute, R is the ideal gas constant, and T is the temperature (ii). |
