List of top Chemistry Questions on Ionic Equilibrium In Solution

The solubility product of \(PbCl_2\) at \(298\ \text{K}\) is \(3.2 \times 10^{-5}\). What is its solubility in \(\text{mol dm}^{-3}\)?

Identify \(Base_2\) for the following equation according to Brønsted-Lowry theory:
\( HCl(aq) + H_2O(l) \rightleftharpoons H_3O^+(aq) + Cl^-(aq) \)

The solubility of \(BaCO_3\) (molar mass \(197\,g\,mol^{-1}\)) is \(1.4\times10^{-3}\) g per 100 mL. The solubility product constant of \(BaCO_3\) is \(x\times10^{-9}\,mol^2L^{-2}\). The value of \(x\) (nearest integer) is:

Buffer contains $[X^-]:[HX]=1:10$, and $K_b = 10^{-10}$. Find pH.}

Select the set of incorrect statements: Statement-I : The pH of neutral water at \(310\,K\) is lower than 7. Statement-II : The pH of an aqueous solution of \(1\times10^{-8}\,M\) HCl is 8. Statement-III : The ionization of \(CH_3COONa\) is suppressed in presence of \(CH_3COOH\). Statement-IV : CuS is precipitated when \(H_2S\) is passed through a solution of \(Cu^{2+}\) and \(Zn^{2+}\) ions in presence of dilute HCl since \(K_{sp}(CuS)\lt K_{sp}(ZnS)\).

The pH of a 0.1 M solution of a weak monobasic organic acid is 4.0. What is the dissociation constant of the acid?

The exhausted anion-exchange resin is regenerated with

Which of the following is a weak electrolyte?

Electrolysis of an aqueous solution of \(Na_2SO_4\) between Pt electrodes liberates a gas \(X\) at anode and gas \(Y\) at cathode. \(X\) and \(Y\) respectively are

According to Arrhenius theory of acids and bases, which of the following is an example of Arrhenius base?

\(100\ \text{mL}\) of \(0.1M\ HCl\) and \(100\ \text{mL}\) of \(0.05M\ H_2SO_4\) are mixed and the solution is diluted to \(2.0\ L\) by adding water. The pH of the resulting solution is

Which of the following has highest equivalent weight? Given: At.wt \(H=1,\ C=12,\ O=16,\ S=32,\ Na=23,\ Ca=40\)

\(12.6\ \text{g}\) of oxalic acid, \(H_2C_2O_4\cdot 2H_2O\) \((\text{M.wt. }126)\), is present in \(1500\ \text{mL}\) of solution. The normality of that solution is

The pH of a $0.01\text{ M NaOH}$ solution is}

Which of the following is a conjugate acid-base pair?

Identify conjugate acid and conjugate base for \( HCO_3^- \) ion respectively:

What is the pH of \(2 \times 10^{-3}\ \text{M}\) solution of a monacidic weak base if it ionises to the extent of \(5\%\)?

Calculate the pH of \(0.01\ \text{M}\) strong dibasic acid.

Calculate the solubility in \(\text{mol dm}^{-3}\) of sparingly soluble salt BaBr if its solubility product is \(4.9 \times 10^{-13}\) at the same temperature.

Find the concentration of sodium acetate when added to \(0.1\ \text{M}\) solution of acetic acid to form a buffer solution of \(pH = 5.5\). (Given: \(pK_a\) of \(\text{CH}_3\text{COOH} = 4.5\))

The solubility product of AgBr is \(4.9 \times 10^{-13}\) at a certain temperature. Calculate the molar solubility of AgBr.

What is the pH of a weak dibasic acid that is 2% dissociated in its M/100 solution at 298 K?

Calculate the pH of 0.01 M sulphuric acid.

Identify $\text{base}_2$ for the following equation according to Br\o{}nsted--Lowry theory: \[HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O^+_{(aq)} + Cl^-_{(aq)}\]}

What is the pH of $2 \times 10^{-3}$ M solution of monoacidic weak base if it ionises to the extent of 5%?