Common Ion Effect

Among the given pairs, which pair shows common ion effect?

Which of the following is not an example of common ion effect?

What will be the fluoride ion concentration, if the calcium ion concentration is increased by four times in a saturated solution of sparingly soluble ${\mathrm{CaF}}_2$ salt? 

Given ${\mathrm{K}}_{\mathrm{sp}}$of ${\mathrm{CaF}}_2$ is $4.43 \times {10}^{-16}$.

What is the correct relationship between the solubilities of $\mathrm{AgCl}$ in ${\mathrm{H}}_2\mathrm{O}, 0.01 \mathrm{M} {\mathrm{CaCl}}_2, 0.01 \mathrm{M} \mathrm{NaCl} \& 0.05 \mathrm{M} {\mathrm{AgNO}}_3$ if the values are ${\mathrm{S}}_1, {\mathrm{S}}_2, {\mathrm{S}}_3 \& {\mathrm{S}}_4$, respectively?

(Neglect any complexation)

The pH of gastric juice in human stomach is about 2-3 and pH in the small intestine is about 8. The ${\mathrm{pK}}_{\mathrm{a}}$ of acetylsalicylic acid (aspirin) is 3.5 Aspirin will be.

What is the solubility of $\mathrm{AgCl}$ in 0.1 M KCl solution (in mol/L)?
$\left({\mathrm{K}}_{\mathrm{sp}}=1.2\times {10}^{-10}\right)$ 

What will be the solubility of $\text{AgCl}$ in 0.1M $\text{KCl}$ solution?
$\left({\mathrm{K}}_{\mathrm{sp}}=1.2\times {10}^{-10}\right)$ (in mol/L)

An aqueous solution of ${\mathrm{H}}_2\mathrm{S}$ gas in water attains the following equilibrium.
${\mathrm{H}}_2{\mathrm{S}}_{\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{H}}_{\left(\mathrm{aq}\right)}^{+}+{\mathrm{HS}}_{\left(\mathrm{aq}\right)}^{-}$
If few $\mathrm{mL}$ of dilute $\mathrm{HCl}$ is added to the above solution, what will happen without change in temperature?

If the solubility(s) of ${\mathrm{AgCl}}_{\left(\mathrm{s}\right)}$ in $0.1\mathrm{M} \mathrm{NaCl}$ solution is  $\mathrm{a} \mathrm{X} {10}^{-10}$, then what will be the value of $\text{'}\mathrm{a}\text{'}$ if the given solubility product of $\mathrm{AgCl}$is $1.6 x {10}^{-10}$?

The solubility of ${\mathrm{AgCl}}_{\left(s\right)}$ with solubility product $1.6\times {10}^{-10} \mathrm{in} 0.1 \mathrm{M} \mathrm{NaCl}$ Solution is  $x\times {10}^{-9}$ M. The value of $10\mathrm{x}$ is__(Nearest integer)

Find the molar solubility of Ni(OH)₂ in 0.1 M NaOH, if its solubility product is 2 x 10^-15.

The ionic product of $\mathrm{Ni}(\mathrm{OH}{)}_2$ is$2.0 \times {10}^{-15}$. The molar solubility of$\mathrm{Ni}(\mathrm{OH}{)}_2$ in $0.10 \mathrm{M}$ $\mathrm{NaOH}$ is

The solubility product of $\mathrm{AgCl}\left(\mathrm{s}\right)$ is$1.6\times {10}^{-10}$. Find the solubility of $\mathrm{AgCl}\left(\mathrm{s}\right)$ in $0.1\mathrm{ }\mathrm{M}\mathrm{ }\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$ solution.

What is the molar solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in $1.0 \mathrm{M} \mathrm{NaOH}$?

(Given: Ionic product of $\mathrm{Ni}(\mathrm{OH}{)}_2=1.9\times {10}^{-15}$)

The ionic product of Ni(OH)₂ is 2.0 × 10^-15. The molar solubility of Ni(OH)₂ in 0.10 M NaOH is-

If the maximum concentration of $\mathrm{P}\mathrm{b}\mathrm{C}{\mathrm{l}}_2$ in water is 0.01 M at $25°\mathrm{C}$ , its maximum concentration in 0.1 M NaCl will be

When strong base (NaOH) is added to the weak acid (acetic acid, $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H})$ , then dissociation of acetic acid increases; this effect is known as

If degree of dissociation of 2M $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H}$ is 10% then degree of dissociation of this acetic acid in 3 Molar $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{N}\mathrm{a}$ solution will be

Arrange in increasing order of solubility of AgBr in solutions given here

(i) 0.1 M $\mathrm{N}{\mathrm{H}}_3$ (ii) 0.1 M $\mathrm{A}\mathrm{g}\mathrm{N}{\mathrm{O}}_3$ (iii) 0.2 M NaBr (iv) pure water

The equilibrium that exists in aqueous solution, ${\text{CH}}_{\text{3}}\text{COOH}\stackrel{}{\rightleftharpoons }{\text{CH}}_{\text{3}}{\text{COO}}^{-}\text{+}{\text{H}}^{\text{+}}$ if dil $\text{HCl}$ is added at constant temperature, then