6.02×10²⁰ molecules of urea are present in 100 ml of its solution. The concentration of urea solution is

• 0.001 M

• 0.1 M

• 0.02 M

• 0.02 M

312.

To neutralize completely 20 mL of 0.1 M aqueous solution of phosphorous acid (H₃PO₃), the volume of 0.1 M aqueous KOH solution required is

• 10 mL

• 60 mL

• 40 mL

• 40 mL

Which of the following liquid pairs shows a positive deviation from Raoult’s law?

• Water – hydrochloric acid

• Acetone – chloroform

• Water – nitric acid

• Water – nitric acid

Which one of the following statements is false?

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

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

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

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

The molar solubility product is K_sp. ‘s’ is given in terms of K_sp by the relation

• 
• 

• s = (256 K_sp)^1/5

• s = (256 K_sp)^1/5

For 1 molal aqueous solution of the following compounds, which one will show the highest freezing point?

• [Co(H₂O)₃ Cl₃].3H₂O

• [Co(H₂O)₆]Cl₃

• [Co(H₂O)₅Cl] Cl₂.H₂O

• [Co(H₂O)₄Cl2]Cl.2H₂O

An aqueous solution contains an unknown concentration of Ba²⁺. When 50 mL of a 1 M solution of Na₂SO₄ is added, BaSO₄ just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO₄ is 1 x 10–10. What is the original concentration of Ba²⁺?

• 1.0 x 10^–10 M

• 5 x 10^–9 M

• 2x10^–9 M

• 1.1 x 10^–9M

Assuming the compounds to be completely dissociated in aqueous solution, identify the pair of the solutions that can be expected to be isotonic at the same temperature.

• 0.01 M urea and 0.01 M NaCl

• 0.02 M NaCl and 0.01 M Na₂SO₄

• 0.03 M NaCl and 0.02 M MgCl₂

• 0.01 M sucrose and 0.02 M glucose

If $\mathrm{p}°$and p are the vapour pressure of the pure solvent and solution and n₁ and n₂ are the moles of solute and solvent respectively in the solution then the correct relation between p and p° is

• $\mathrm{p}°=\mathrm{p}\left[\frac{{\mathrm{n}}_1}{{\mathrm{n}}_1+{\mathrm{n}}_2}\right]$

• $\mathrm{p}°=\mathrm{p}\left[\frac{{\mathrm{n}}_2}{{\mathrm{n}}_1+{\mathrm{n}}_2}\right]$

• $\mathrm{p}=\mathrm{p}°\left[\frac{{\mathrm{n}}_2}{{\mathrm{n}}_1+{\mathrm{n}}_2}\right]$

• $\mathrm{p}=\mathrm{p}°\left[\frac{{\mathrm{n}}_1}{{\mathrm{n}}_1+{\mathrm{n}}_2}\right]$

In aqueous alkaline solution, two electrons reduction of HO${}_2^{-}$ gives

• HO^-

• H₂O

• O₂

• O${}_2^{-}$