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

To a 200 ml of 0.1 M weak acid HA solution 90 ml of 0.1 M solution of NaOH be added, Now, what volume of 0.1 M NaOH be added into above solution so that pH of resulting solution be 5.

[K_a(HA) = 10^-5]

1. 2 ml               

2. 20 ml

3. 10 ml             

4. 15 ml

If carbon dioxide is 2% dissociated at equilibrium 2CO₂ (g)$\rightleftharpoons$2CO(g) + O₂(g). The mole fraction of CO₂ at equuilibrium is

1. 1.01/0.98           

2. 0.98/1.01

3. 0.01/0.98           

4. 0.098/1.01