01. Solubility and Solubility Product Constant
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Ionic Equilibrium

229445 If the solubility of a sparingly soluble salt $\mathbf{A X}_2$ is $\mathrm{s} \mathrm{mol} /lit$., the solubility product is

1 $4 \mathrm{~s}^3$
2 $8 \mathrm{~s}^3$
3 $4 \mathrm{~s}^2$
4 $s^2$
J and K CET-(2015)
Ionic Equilibrium

229452 A solution contains $0.05 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M}$ NaI. The concentration of iodied ion in solution when $\mathrm{AgCl}$ just starts precipitating is equal to $\left(\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1 \times 10^{-10} ; \mathrm{K}_{\mathrm{sp}} \mathrm{AgI}=4 \times 10^{-16}\right.$ )

1 $4.0 \times 10^{-8} \mathrm{M}$
2 $2.0 \times 10^{-7} \mathrm{M}$
3 $8.0 \times 16^{-16} \mathrm{M}$
4 $2.0 \times 10^{-8} \mathrm{M}$
J and K CET-(1999)
Ionic Equilibrium

229462 Solubility of $\mathrm{AgCl}$ is least in

1 $0.1 \mathrm{M} \mathrm{NaCl}$
2 pure water
3 $0.1 \mathrm{M} \mathrm{BaCl}_2$
4 $0.1 \mathrm{M} \mathrm{AlCl}_3$
Karnataka-CET-2019
Ionic Equilibrium

229466 Choose the correct statement.

1 $\mathrm{K}_{\mathrm{H}}$ value is same for a gas in any solution.
2 Higher the $\mathrm{K}_{\mathrm{H}}$ value more the solubility of gas.
3 $\mathrm{K}_{\mathrm{H}}$ value increases on increasing the temperature of the solution.
4 Easily liquefiable gases usually has lesser $\mathrm{K}_{\mathrm{H}}$ values.
Karnataka-CET-2021
Ionic Equilibrium

229479 Solubility of $\mathrm{Ca}(\mathrm{OH})_2$ is $\mathrm{s} \mathrm{mol} \mathrm{L}^{-1}$. The solubility product ( $K_{\mathrm{sp}}$ ) under the same condition is

1 $4 \mathrm{~s}^3$
2 $3 \mathrm{~s}^4$
3 $4 \mathrm{~s}^2$
4 $\mathrm{s}^3$
MHT CET-2008
Join With Us for More Updates
Ionic Equilibrium

229445 If the solubility of a sparingly soluble salt $\mathbf{A X}_2$ is $\mathrm{s} \mathrm{mol} /lit$., the solubility product is

1 $4 \mathrm{~s}^3$
2 $8 \mathrm{~s}^3$
3 $4 \mathrm{~s}^2$
4 $s^2$
J and K CET-(2015)
Ionic Equilibrium

229452 A solution contains $0.05 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M}$ NaI. The concentration of iodied ion in solution when $\mathrm{AgCl}$ just starts precipitating is equal to $\left(\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1 \times 10^{-10} ; \mathrm{K}_{\mathrm{sp}} \mathrm{AgI}=4 \times 10^{-16}\right.$ )

1 $4.0 \times 10^{-8} \mathrm{M}$
2 $2.0 \times 10^{-7} \mathrm{M}$
3 $8.0 \times 16^{-16} \mathrm{M}$
4 $2.0 \times 10^{-8} \mathrm{M}$
J and K CET-(1999)
Ionic Equilibrium

229462 Solubility of $\mathrm{AgCl}$ is least in

1 $0.1 \mathrm{M} \mathrm{NaCl}$
2 pure water
3 $0.1 \mathrm{M} \mathrm{BaCl}_2$
4 $0.1 \mathrm{M} \mathrm{AlCl}_3$
Karnataka-CET-2019
Ionic Equilibrium

229466 Choose the correct statement.

1 $\mathrm{K}_{\mathrm{H}}$ value is same for a gas in any solution.
2 Higher the $\mathrm{K}_{\mathrm{H}}$ value more the solubility of gas.
3 $\mathrm{K}_{\mathrm{H}}$ value increases on increasing the temperature of the solution.
4 Easily liquefiable gases usually has lesser $\mathrm{K}_{\mathrm{H}}$ values.
Karnataka-CET-2021
Ionic Equilibrium

229479 Solubility of $\mathrm{Ca}(\mathrm{OH})_2$ is $\mathrm{s} \mathrm{mol} \mathrm{L}^{-1}$. The solubility product ( $K_{\mathrm{sp}}$ ) under the same condition is

1 $4 \mathrm{~s}^3$
2 $3 \mathrm{~s}^4$
3 $4 \mathrm{~s}^2$
4 $\mathrm{s}^3$
MHT CET-2008
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Ionic Equilibrium

229445 If the solubility of a sparingly soluble salt $\mathbf{A X}_2$ is $\mathrm{s} \mathrm{mol} /lit$., the solubility product is

1 $4 \mathrm{~s}^3$
2 $8 \mathrm{~s}^3$
3 $4 \mathrm{~s}^2$
4 $s^2$
J and K CET-(2015)
Ionic Equilibrium

229452 A solution contains $0.05 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M}$ NaI. The concentration of iodied ion in solution when $\mathrm{AgCl}$ just starts precipitating is equal to $\left(\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1 \times 10^{-10} ; \mathrm{K}_{\mathrm{sp}} \mathrm{AgI}=4 \times 10^{-16}\right.$ )

1 $4.0 \times 10^{-8} \mathrm{M}$
2 $2.0 \times 10^{-7} \mathrm{M}$
3 $8.0 \times 16^{-16} \mathrm{M}$
4 $2.0 \times 10^{-8} \mathrm{M}$
J and K CET-(1999)
Ionic Equilibrium

229462 Solubility of $\mathrm{AgCl}$ is least in

1 $0.1 \mathrm{M} \mathrm{NaCl}$
2 pure water
3 $0.1 \mathrm{M} \mathrm{BaCl}_2$
4 $0.1 \mathrm{M} \mathrm{AlCl}_3$
Karnataka-CET-2019
Ionic Equilibrium

229466 Choose the correct statement.

1 $\mathrm{K}_{\mathrm{H}}$ value is same for a gas in any solution.
2 Higher the $\mathrm{K}_{\mathrm{H}}$ value more the solubility of gas.
3 $\mathrm{K}_{\mathrm{H}}$ value increases on increasing the temperature of the solution.
4 Easily liquefiable gases usually has lesser $\mathrm{K}_{\mathrm{H}}$ values.
Karnataka-CET-2021
Ionic Equilibrium

229479 Solubility of $\mathrm{Ca}(\mathrm{OH})_2$ is $\mathrm{s} \mathrm{mol} \mathrm{L}^{-1}$. The solubility product ( $K_{\mathrm{sp}}$ ) under the same condition is

1 $4 \mathrm{~s}^3$
2 $3 \mathrm{~s}^4$
3 $4 \mathrm{~s}^2$
4 $\mathrm{s}^3$
MHT CET-2008
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Ionic Equilibrium

229445 If the solubility of a sparingly soluble salt $\mathbf{A X}_2$ is $\mathrm{s} \mathrm{mol} /lit$., the solubility product is

1 $4 \mathrm{~s}^3$
2 $8 \mathrm{~s}^3$
3 $4 \mathrm{~s}^2$
4 $s^2$
J and K CET-(2015)
Ionic Equilibrium

229452 A solution contains $0.05 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M}$ NaI. The concentration of iodied ion in solution when $\mathrm{AgCl}$ just starts precipitating is equal to $\left(\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1 \times 10^{-10} ; \mathrm{K}_{\mathrm{sp}} \mathrm{AgI}=4 \times 10^{-16}\right.$ )

1 $4.0 \times 10^{-8} \mathrm{M}$
2 $2.0 \times 10^{-7} \mathrm{M}$
3 $8.0 \times 16^{-16} \mathrm{M}$
4 $2.0 \times 10^{-8} \mathrm{M}$
J and K CET-(1999)
Ionic Equilibrium

229462 Solubility of $\mathrm{AgCl}$ is least in

1 $0.1 \mathrm{M} \mathrm{NaCl}$
2 pure water
3 $0.1 \mathrm{M} \mathrm{BaCl}_2$
4 $0.1 \mathrm{M} \mathrm{AlCl}_3$
Karnataka-CET-2019
Ionic Equilibrium

229466 Choose the correct statement.

1 $\mathrm{K}_{\mathrm{H}}$ value is same for a gas in any solution.
2 Higher the $\mathrm{K}_{\mathrm{H}}$ value more the solubility of gas.
3 $\mathrm{K}_{\mathrm{H}}$ value increases on increasing the temperature of the solution.
4 Easily liquefiable gases usually has lesser $\mathrm{K}_{\mathrm{H}}$ values.
Karnataka-CET-2021
Ionic Equilibrium

229479 Solubility of $\mathrm{Ca}(\mathrm{OH})_2$ is $\mathrm{s} \mathrm{mol} \mathrm{L}^{-1}$. The solubility product ( $K_{\mathrm{sp}}$ ) under the same condition is

1 $4 \mathrm{~s}^3$
2 $3 \mathrm{~s}^4$
3 $4 \mathrm{~s}^2$
4 $\mathrm{s}^3$
MHT CET-2008
Join With Us for More Updates
Ionic Equilibrium

229445 If the solubility of a sparingly soluble salt $\mathbf{A X}_2$ is $\mathrm{s} \mathrm{mol} /lit$., the solubility product is

1 $4 \mathrm{~s}^3$
2 $8 \mathrm{~s}^3$
3 $4 \mathrm{~s}^2$
4 $s^2$
J and K CET-(2015)
Ionic Equilibrium

229452 A solution contains $0.05 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M}$ NaI. The concentration of iodied ion in solution when $\mathrm{AgCl}$ just starts precipitating is equal to $\left(\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1 \times 10^{-10} ; \mathrm{K}_{\mathrm{sp}} \mathrm{AgI}=4 \times 10^{-16}\right.$ )

1 $4.0 \times 10^{-8} \mathrm{M}$
2 $2.0 \times 10^{-7} \mathrm{M}$
3 $8.0 \times 16^{-16} \mathrm{M}$
4 $2.0 \times 10^{-8} \mathrm{M}$
J and K CET-(1999)
Ionic Equilibrium

229462 Solubility of $\mathrm{AgCl}$ is least in

1 $0.1 \mathrm{M} \mathrm{NaCl}$
2 pure water
3 $0.1 \mathrm{M} \mathrm{BaCl}_2$
4 $0.1 \mathrm{M} \mathrm{AlCl}_3$
Karnataka-CET-2019
Ionic Equilibrium

229466 Choose the correct statement.

1 $\mathrm{K}_{\mathrm{H}}$ value is same for a gas in any solution.
2 Higher the $\mathrm{K}_{\mathrm{H}}$ value more the solubility of gas.
3 $\mathrm{K}_{\mathrm{H}}$ value increases on increasing the temperature of the solution.
4 Easily liquefiable gases usually has lesser $\mathrm{K}_{\mathrm{H}}$ values.
Karnataka-CET-2021
Ionic Equilibrium

229479 Solubility of $\mathrm{Ca}(\mathrm{OH})_2$ is $\mathrm{s} \mathrm{mol} \mathrm{L}^{-1}$. The solubility product ( $K_{\mathrm{sp}}$ ) under the same condition is

1 $4 \mathrm{~s}^3$
2 $3 \mathrm{~s}^4$
3 $4 \mathrm{~s}^2$
4 $\mathrm{s}^3$
MHT CET-2008