Which of the following solvents are aprotic ?

I. NH₃

II. SO₂

III. CH₃CN

IV. CH₃CO₂H

• I, II and III

• I, III and IV

• II and III

• I and III

If 20 g of a solute was dissolve in 500 mL of water and osmotic pressure of the solution was found to be 600 mm of Hg at 15°C, then molecular weight of the solute is

• 1000

• 1200

• 1400

• 1800

Which of the following statement is false?

• Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction

• The osmotic pressure ($\mathrm{\pi }$) of a solution is given by the equation T = MRT, where M is the molarity of the solution

• The correct order of osmotic pressure for 0.01 M aqueous solution of each compound is BaCl₂ > KCl > CH₃COOH > sucrose

• Two sucrose solution of same molality prepared in different solvents will have the same freezing point depression

Glucose is added to 1 L water to sch an extent that $∆{\mathrm{T}}_{\mathrm{f}}/ {\mathrm{K}}_{\mathrm{f}}$becomes equal to 10^-3, the weight of glucose (C₆H₁₂O₆ ) added is

• 180 gm

• 18 gm

• 1.8 gm

• 0.18 gm

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

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