In an acidic Buffer solution (CH₃COOH + CH₃COONa), the species mainly present in the solution are:

(Ignore negligible amount)

1. CH₃COOH, CH₃COO^-, CH₃COONa, H⁺

2. CH₃COO^-, Na⁺, CH₃COOH

3. CH₃COONa, CH₃COO-, H⁺

4. CH₃COO^-, Na⁺, H⁺, CH₃COONa

What happens to the pH when NH₄Cl is added to an NH₄OH solution?

1. Increases

2. Decreases

3. Remains unchanged

4. First decreases and then increases

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

Find the values of Kₚ/Kc for the following gaseous reactions:

I. 2A + 3B ⇌ 2C
II. 2A ⇌ 4B
III. A + B + 2C ⇌ 4D

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 ${\mathrm{PCl}}_5(\mathrm{g})\hspace{0.17em}\rightleftharpoons \hspace{0.17em}{\mathrm{PCl}}_3(\mathrm{g})$ $+$ ${\mathrm{Cl}}_2\left(\mathrm{g}\right)$ 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