According to Le-Chatelier's principle, adding heat to a solid \(⇌ \)liquid equilibrium will cause the :

1. Temperature to increase

2. Temperature to decrease

3. Amount of liquid to decrease

4. Amount of solid to decrease

H₂S gas when passed through a solution of cations containing HCl precipitates the cations of the second group in qualitative analysis but not those belonging to the fourth group. It is because: 
 

The addition of HCl does not suppress the ionization of:

In which of the following will the solubility of AgCl be the minimum?

Salting out action of the soap is based on:

1. Complex ion formation

2. Common ion effect

3. Solubility product

4. Acid-base neutralization

HI was heated in a sealed tube at 440$°$C till the equilibrium was reached. At this point, HI was found to be 22 % decomposed. The equilibrium constant for this dissociation is :

For the reaction,

  PCl₅(g) \(⇌ \)PCl₃(g) + Cl₂ (g)

The forward reaction at constant temperature is favoured by:

1. Introducing an inert gas at a constant volume

2. Introducing chlorine gas at a constant volume

3. Introducing an inert gas at constant pressure

4. None of the above

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

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.

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