Mock Test 1 — Equilibrium

$K_c$ for $H_2 + I_2 \rightleftharpoons 2HI$ at $700$ K is $50$. $K_c$ for reverse reaction:

$K_p$ and $K_c$ relation:

Catalyst:

pH of $10^{-8}$ M HCl is approximately:

Buffer capacity is maximum when:

Solubility of $Ag_2CrO_4$ in water is $s$. $K_{sp}$:

pH of $0.001$ M NaOH:

Increasing temperature for exothermic reaction:

Salt of weak acid and weak base in solution has pH:

Among the following, weakest acid:

For $N_2 + 3H_2 \rightleftharpoons 2NH_3$, $\Delta n_g = $ (sign included as integer):

pH of $10^{-3}$ M HCl:

Number of pH units pH changes from $10^{-2}$ M to $10^{-5}$ M HCl:

Assertion (A): Common ion effect reduces the solubility of a sparingly soluble salt. Reason (R): The product of ionic concentrations is restricted to $K_{sp}$; addition of common ion shifts equilibrium backward.

Assertion (A): A catalyst does not alter the equilibrium constant. Reason (R): Catalyst lowers activation energy of both forward and reverse reactions equally.