NEET Chemistry Chemical Equilibrium MCQs

A solution containing a weak acid HA and its conjugate base A$^-$ has a pH of 4.8. If the pK$_a$ of HA is 4.74, which of the following is TRUE?

100 mL of a buffer solution contains 0.1 M NH$_4$OH and 0.1 M NH$_4$Cl. If K$_b$ for NH$_4$OH is 1.8 x 10$^{-5}$, what is the pH change when 0.01 moles of HCl are added?

A buffer solution with pH 9 is to be prepared using NH$_4$OH (K$_b$= 1.8 x 10$^{-5}$) and NH$_4$Cl. What should be the ratio of [NH$_4$Cl]/[NH$_4$OH]?

A 0.1 M solution of a salt of a weak acid (HA) and a weak base (BOH) has a pH of 8.2. Given $K_a(HA) = 1 imes 10^{-5}$ and $K_b(BOH) = 2 imes 10^{-6}$, what is the value of $K_h$ for the salt?

A solution of $NH_4CN$ ($K_a(HCN) = 6.2 imes 10^{-10}$, $K_b(NH_3) = 1.8 imes 10^{-5}$) is:

(A) Acidic

(B) Basic

(C) Neutral

(D) Cannot be determined

The pH of a 0.1M solution of $NaA$ is 9. The $K_a$ of $HA$ is:

The hydrolysis constant $K_h$ for the salt of a weak acid ($K_a = 10^{-6}$) and a weak base ($K_b = 10^{-8}$) is:

For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, if the concentrations of $N_2$, $H_2$, and $NH_3$ are 1 M, 3 M, and 2 M respectively at equilibrium, what is the value of $K_c$?

If $K_p$ for a reaction is $1 \, atm$ and $Δn = 1$, what is the value of $K_c$ at 298 K? (R = 0.0821 L atm/mol K)

A sparingly soluble salt MX$_2$ has a solubility product K$_{sp}$ = 4 x 10$^{-12}$. In a solution containing 0.01 M NaX, the molar solubility of MX$_2$ is: