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

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. $1+\mathrm{\alpha }$

The dissociation of NH₄OH can be suppressed by the addition of:

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.

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

Which of the following silver salts precipitates last when an AgNO₃ solution is
gradually added to a solution containing equal concentrations of Cl⁻, Br⁻, I⁻ , and CrO₄²⁻ ions?

Given:

Kₛₚ(Ag₂CrO₄) = 1.1 × 10⁻¹²
Kₛₚ(AgCl) = 1.8 × 10⁻¹⁰
Kₛₚ(AgBr) = 5.0 × 10⁻¹³
Kₛₚ(AgI) = 8.3 × 10⁻¹⁷

For the equilibrium of the reaction,\(\mathrm{HgO}(\mathrm{~s}) \rightleftharpoons \mathrm{Hg}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_ 2(\mathrm{~g}), \mathrm{K_P}\) for the reaction at a total pressure of "P" will be:

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 :

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

The addition of HCl does not suppress the ionization of: