An aqueous solution of NaHSO₃ is-

1. Acidic                 
2. Slightly alkaline
3. Alkaline             
4. Slightly Acidic

The solubility product constant (K_sp) of salts of types MX, MX₂ and M₃X at temperature T are 4.0 X 10^-8, 3.2 X 10^-14 and 2.7 X 10^-15 respectively. Solubilities(mol dm^-3) of the salts at temperature T are the order:

1. MX > MX₂ > M₃X

2. M₃X > MX₂ > MX

3. MX >M₃X > MX₂ 

4. M₃X >MX > MX₂

Ostwald dilution law for weak electrolyte HA can be given as

$\left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0$
$\left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above}$

In the reaction, N₂O₄(g) $\rightleftharpoons$ 2NO₂(g), $\mathrm{\alpha }$ is that part of N₂O₄ which dissociates. The number of moles at equilibrium will be:

1. ${\left(1-\mathrm{\alpha }\right)}^2$

2. $3\mathrm{\alpha }$

3. $\mathrm{\alpha }$

4. $1+\mathrm{\alpha }$

In which solution, AgCl has minimum solubility ?

1. 0.05 M AgNO₃

2. 0.01 M NaCl

3. Pure Water

4. 0.01 M NH₄OH

50 ml of HCl (pH=1) is mixed with another 100 ml of HCl (pH=2) then pH of resulting solution will be approximately

1. 1.2

2. 1.4

3. 1.6

4. 1.8

In a nitrating mixture (HNO₃ + H₂SO₄), HNO₃ acts as

1. Acid

2. Base

3. Acid as well as Base

4. Neither acid nor base

When a solution of acetic acid was titrated with NaOH, the pH of the solution when half of the acid, neutralised was 4.2. Dissociation constant of the acid is

1. 6.31 × 10^-5

2. 3.2 × 10^-5

3. 8.7 × 10^-8

4. 6.42 × 10^-4

The strongest Lewis acid among the following is:

1. BBr₃

2. BCl₃

3. BF₃

4. All are same

Calculate the molar solublity of Fe(OH)₂ at a pH of 8

[K_sp of Fe(OH)₂ = 1.6 X 10^-14]

1. 0.06

2. 0.016

3. 0.01

4. 0.16