Ionic Equilibrium

The solubility of barium iodate in an aqueous solution prepared by mixing 200 mL of 0.010 M barium nitrate with 100 mL of 0.10 M sodium iodate is $\boldsymbol{X} \times 10^{-6} \mathrm{~mol} \mathrm{dm}^{-3}$. The value of $\boldsymbol{X}$ ...

At 25 °C, the concentration of H+ ions in 1.00 × 10−3 M aqueous solution of a weak monobasic acid having acid dissociation constant (Ka) of 4.00 × 10−11 is X × 10−7 M. The value of X is ______.Use: Ionic product of water (Kw) = 1.00 × 10−14...

On decreasing the $p \mathrm{H}$ from 7 to 2 , the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from $10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$ to $10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$. The $p \mathrm{~K}_{\mat...

Concentration of $\mathrm{H}_{2} \mathrm{SO}_{4}$ and $\mathrm{Na}_{2} \mathrm{SO}_{4}$ in a solution is $1 \mathrm{M}$ and $1.8 \times 10^{-2} \mathrm{M}$, respectively. Molar solubility of $\mathrm{PbSO}_{4}$ in the same solution is $\mat...

A solution is prepared by mixing $0.01 \mathrm{~mol}$ each of $\mathrm{H}_{2} \mathrm{CO}_{3}, \mathrm{NaHCO}_{3}, \mathrm{Na}_{2} \mathrm{CO}_{3}$, and $\mathrm{NaOH}$ in $100 \mathrm{~mL}$ of water. $p \mathrm{H}$ of the resulting solutio...

A solution of 0.1 M weak base (B) is titrated with 0.1 M of a strong acid (HA). The variation of pH of the solution with the volume of HA added is shown in the figure below. What is the pKb of the base? The neutralisation reaction is given ...

An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS?Use Ksp(ZnS) = 1.25 \(\times\) 10\(-\)22 and overall dissociation constant of...

Dilution processes of different aqueous solutions, with water, are given in LIST - I. The effects of dilution of the solutions on \(\left[ {{H^ + }} \right]\) are given in LIST - II
(Note: Degree of dissociation (a) of weak acid and weak ...

The solubility of a salt of weak acid \((AB)\) at \(pH\,\) \(3\) is \(Y \times {10^{ - 3}}\) \(mol\,{L^{ - 1}}.\) The value of \(Y\) is ________________.
(Given that the value of solubility product of \(AB\) $$\left( {{K_{sp}}} \right) = 2...

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When 100 mL of 1.0 M KCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7o C was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralizat...

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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7o C was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralizat...

The Ksp of Ag2CrO4 is 1.1 \(\times\) 10-12 at 298 K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is

The initial rate of hydrolysis of methyl acetate (1M) by a weak acid (HA, 1M) is 1/100th of that of a strong acid (HX, 1M), at 25oC. The Ka of HA is

In 1 L saturated solution of AgCl [Ksp(AgCl) = 1.6 \(\times\) 10-10], 0.1 mol of CuCl [Ksp(CuCl) = 1.0 \(\times\) 10-6] is added. The resultant concentration of Ag+ in the solution is 1.6 \(\times\) 10-x. The value of "x" is

Amongst the following the total number of compounds whose aqueous solution turns red litmus paper blue is
KCN, K2SO4, (NH4)2C2O4, NaCl, Zn(NO3)2, FeCl3, K2CO3, NH4NO3 and LiCN

Aqueous solution of HNO3, KOH and CH3COOH and CH3COONa of identical concentrations are provided. The pairs of solutions which form a buffer upon mixing is(are)

The dissociation constant of a substituted benzoic acid at 25\(^\circ\)C is 1.0 \(\times\) 10\(^{-4}\). The pH of a 0.01 M solution of its sodium salt is __________.

Solubility product constants (K\(_{sp}\)) of salts of types MX, MX\(_2\) and M\(_3\)X at temperature T are 4.0 \(\times\) 10\(^{-8}\), 3.2 \(\times\) 10\(^{-14}\) and 2.7 \(\times\) 10\(^{-15}\), respectively. Solubilities (mol dm\(^{-3}\))...

2.5 mL of \(\frac{2}{5}\)M weak monoacidic base (K\(_b\) = 1 \(\times\) 10\(^{-12}\) at 25\(^\circ\)C) is titrated with \(\frac{2}{15}\)M HCl in water at 25\(^\circ\)C. The concentration of H\(^+\) at equivalence point is (K\(_w\) = 1 $$\ti...