Solubility Product

Q. The solubility product of $Pb{I}_2$ is $8.0\times {10}^{-9}$. The solubility of lead iodide in 0.1 molar solution of lead nitrate is $x\times {10}^{-6}mol/L$. Given: $\sqrt{2}=1.41$. The value of $x$ is

Q.

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 $K_{sp}=2\times {10}^{–10}$ and the value of ionization constant of HB $K_a=1\times {10}^{–8}$)

Q.

The expression for the solubility product of $A{l}_2(S{O}_4{)}_3$ is

1. K_sp = [Al³⁺] [SO₄^2-]

2. K_sp = [Al³⁺]² [SO₄^2-]³

3. K_sp = [Al³⁺]³ [SO₄^2-]²

4. K_sp = [Al³⁺]² [SO₄^2-]²

Q. In 1 L saturated solution of $AgCl\left[K_{sp}\right(AgCl)=1.6\times {10}^{-10}],$ 0.1 mole of $CuCl[K_{p\left(CuCl\right)}=1.0\times {10}^{-6}]$ is added. The resultant concentration of $A{g}^{+}$ in the solution is $1.6\times {10}^{-x}.$ The value of 'x' is ___

Q.

A solution which has ${10}^{-3}$ M each of $M{n}^{2+},F{e}^{2+},Z{n}^{2+}$ and $H{g}^{2+}$ is treated with ${10}^{-16}$ M sulphide ion. If $K_{sp}$ of $MnS$, $FeS$, $ZnS$and $HgS$ are ${10}^{-15}$, ${10}^{-23}$, ${10}^{-20}$ and ${10}^{-54}$ respectively, which one will precipitate first?

1. $FeS$

2. $MgS$

3. $HgS$

4. $ZnS$

Q.

The solubility product of $Mg(OH{)}_2$ at ${25}^{\circ }C$ is $1.4\times {10}^{-11}$. The solubility of $Mg(OH{)}_2$ in gm per litre is:

1. $1.4\times {10}^{-3}$

2. $2.8\times {10}^{-3}$

3. $8.7\times {10}^{-3}$

4. $1.11\times {10}^{-6}$

Q. pH of a saturated solution of $Ba(OH{)}_2$ is 12. The value of solubility product $\left(K_{sp}\right)ofBa(OH{)}_2$ is

1. $3.3\times {10}^{-7}$
2. $5.0\times {10}^{-7}$
3. $4.0\times {10}^{-6}$
4. $5.0\times {10}^{-6}$

Q.

The solubility of $Ca{F}_2$ is $2\times {10}^{-4}$. Its solubilily product $K_{SP}$ is

1. 2.0 x 10^-4

2. 4.0 x 10^-3

3. 8.0 x 10^-12

4. 3.2 x 10^-11

Q.

Sometimes, Ionic product and solubility product are the same - true or false?

1. True

2. False

Q.

If the solubility of calcium sulphate in water is $1.03\times {10}^{-5}$, what will be its solubility in $0.005M$ solution of sulphuric acid?

1. $1.2\times {10}^{-8}mol{L}^{-1}$

2. $2.1\times {10}^{-8}mol{L}^{-1}$

3. $3.8\times {10}^{-8}mol{L}^{-1}$

4. $7.2\times {10}^{-8}mol{L}^{-1}$