When NH₄Cl is added in NH₄OH solution, then pH of the solution

1. Increases

2. Decreases

3. Remains unchanged

4. Firstly decreases and more than decreases

The most hydrolyzed salt among the following is-

(Assume that K_b of all weak bases is the same)
1. NH₄Cl
2. CuSO₄
3. AlCl₃
4. All are equally hydrolyzed.

The pH of 10^-6 M CH₃COOH (K_a = 1.8 X 10^-5) is:

1. 5.37

2. In between 6 & 7

3. 7

4. 8.63

60 ml 1M CH₃COOH is mixed with 20 ml 1 M NaOH then pH of resulting solution will be

(K_a = 1.8 X 10^-5, log1.8 = 0.25)

1. 8.55

2. 4.95

3. 4.45

4. 7.45

In which solvent, solubility of AgCl is maximum ?

1. 0.01 M NaCl

2. Pure Water

3. 0.01 M NH₄OH

4. 0.05 M AgNO₃

$\frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$ for the gaseous reaction:

$\mathrm{I}. 2\mathrm{A} + 3\mathrm{B} \rightleftharpoons 2\mathrm{C}$
$\mathrm{II}. 2\mathrm{A}\rightleftharpoons 4\mathrm{B}$
$\mathrm{III}. \mathrm{A}+\mathrm{B}+2\mathrm{C} \rightleftharpoons 4\mathrm{D}$

Would be respectively:

1. (RT)^-3, (RT)², (RT)⁰ 

2. (RT)^-3, (RT)-², (RT)^-1 

3. (RT)^-3, (RT)², (RT) 

4. None of the above

N₂O₄ dissociates as ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$ at 273 K and 2 atm pressure. The equilibrium mixture has a vapour density of 41. What will be the percentage degree of dissociation ?

1. 14.2%

2. 16.2%

3. 12.2%

4. 87.8%

Inert gas is added to the equilibrium ${\mathrm{PCl}}_5(\mathrm{g}) \rightleftharpoons {\mathrm{PCl}}_3(\mathrm{g})$ $+$ ${\mathrm{Cl}}_2\left(\mathrm{g}\right)$ at constant pressure. The degree of dissociation will :

1. Remain unchanged

2. Decrease

3. Increase

4. Decrease or increase but cannot be predicted with certainty

Dissociation of phosphorus pentachloride is favoured by:

1. High temperature and high pressure

2. High temperature and low pressure

3. Low temperature and low pressure

4. Low temperature and high pressure

1. I,II

2. II,III

3. I,III

4. I,II,III