50 g of saturated aqueous solution of potassium chloride at 30°C is evaporated to dryness, when 13.2 gm of dry KCl was obtained. The solubility of KCl in water at 30°C is

• 35.87 g

• 25.62 g

• 28.97 g

• 27.81 g

462.

A 0.001 molal solution of [Pt(NH₃)₄Cl₄] in water had a freezing point depression of 0.0054°C. If K_f for water is 1.80, the correct formulation of the above molecules is

• [Pt(NH₃)₄Cl₃]Cl

• [Pt(NH₃)₄Cl₂]Cl₂

• [Pt(NH₃)₄Cl]Cl₂

• [Pt(NH₃)₄Cl₄]

If M is molecular weight of solvent, K_b is molal elevation constant, T_b is its boling point p° is its vapour pressure at temperature T and p_s is vapour pressure of its solution having a non- volatile solute at T K , then

• $\frac{{\mathrm{p}}^{°}-{\mathrm{p}}_{\mathrm{s}}}{{\mathrm{p}}^{°}}= \frac{∆{\mathrm{T}}_{\mathrm{b}}}{{\mathrm{K}}_{\mathrm{b}}}\times \mathrm{M}$

• $\frac{{\mathrm{p}}^{°}-{\mathrm{p}}_{\mathrm{s}}}{{\mathrm{p}}^{°}}=\frac{{\mathrm{K}}_{\mathrm{b}}}{∆{\mathrm{T}}_{\mathrm{b}}}\times \mathrm{M}$

• $\frac{{\mathrm{p}}^{°}-{\mathrm{p}}_{\mathrm{s}}}{{\mathrm{p}}^{°}}=\frac{{\mathrm{K}}_{\mathrm{b}}}{∆{\mathrm{T}}_{\mathrm{b}}}\times \frac{\mathrm{M}}{1000}$

• $\frac{{\mathrm{p}}^{°}-{\mathrm{p}}_{\mathrm{s}}}{{\mathrm{p}}^{°}}=\frac{∆{\mathrm{T}}_{\mathrm{b}}}{{\mathrm{K}}_{\mathrm{b}}}\times \frac{\mathrm{M}}{1000}$

For a non-volatile solute,

• vapour pressure of solution is more than vapour pressure of solvent

• Vapour pressure of solvent is zero

• Vapour pressure of solvent is zero

• All of the above

What will happen if a cell is placed into 0.4% (mass/volume) NaCl solution?

• There will be no change in cell volume

• Cell will dissolve

• cell will swell

• cell will shrink

Calculate the osmotic pressure of 0.01 M solution of cane sugar at 300 K (R = 0.08212 atm degree^-1 mol^-1)

• 0.3568 atm

• 0.2463 atm

• 0.1562 atm

• 0.5623 atm

An aqueous dilute solution containing non-volatile solute boils at 100.52° C. What is the molality of solution?(K_b = 0.52 kg mol^-1K, boiloing temperature of water = 100° C)

• 0.1 m

• 0.01 m

• 0.001 m

• 1.0 m

The experimental depression in freezing point of a dilute solution is 0.025 K. If the van't Hoff factor (i) is 2.0, the calculated depression in freezing point (in K) is

• 0.00125

• 0.025

• 0.0125

• 0.05

The molality of an aqueous dilute solution containing non-volatile solute is 0.1 m. What is the boiling temperature (in °C) of solution? (Boiling point elevation constant, K_b = 0.52 kg mol^-1K; boiling temperature of water = 100°C).

• 100.0052

• 100.052

• 100.0

• 100.52

The vapour pressure of a non-ideal two component solution is given below