NEET Chemistry Chemical Equilibrium MCQs

100 mL of 0.1M $HCN$ ($K_a= 6.2 imes 10^{-10}$) is titrated with 0.2M $NaOH$. Calculate the pH at the half-equivalence point.

The solubility product ($K_{sp}$) of $Ag_2CrO_4$ is $1.1 imes 10^{-12}$. What is the molar solubility of $Ag_2CrO_4$ in a 0.1 M $Na_2CrO_4$ solution?

A buffer solution is prepared by mixing 50 mL of 0.2 M acetic acid ($K_a = 1.8 imes 10^{-5}$) with 25 mL of 0.2 M NaOH. What is the change in pH when 0.5 mL of 1.0 M HCl is added to this buffer solution? (Assume volumes are additive.)

For an exothermic reaction at equilibrium, increasing the temperature will:

For the reaction $A(g) \rightleftharpoons B(g) + C(g)$, if the total pressure at equilibrium is P, and the partial pressure of A is $P_A$, the equilibrium constant $K_p$ is:

The solubility product ($K_{sp}$) of a salt AB is $4 imes 10^{-8}$. What is the molar solubility of AB?

The solubility of $AgCl$ in pure water is $s$. What is its solubility product ($K_{sp}$) ?

The solubility product ($K_{sp}$) of $CaF_2$ is represented as:

For a salt $A_2B$, the expression for the solubility product ($K_{sp}$) is:

The solubility product ($K_{sp}$) of $Ag_2CrO_4$ is $1.1 imes 10^{-12}$ at 298K. The solubility (in mol/L) of $Ag_2CrO_4$ in pure water at 298K is: