The K_sp of Ag₂CrO₄ and AgBr is 1.1 × 10^–12 and 5.0 × 10^–13 respectively.

When equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together (K_{sp  (cupric iodate)} = 7.4 × 10^–8 ), from the following, the correct observation would be :

The minimum volume of water required to dissolve 1g of calcium sulphate at 298 K is

(For CaSO₄ , K_sp is 9.1 × 10^–6)

1. 1.22 L

2. 0.69 L

3. 2.44 L

4. 1.87 L

The maximum concentration of equimolar solutions, of ferrous sulphate and sodium sulphide, so that when mixed in equal volumes, there is no precipitation of iron sulphide, will be:

(For iron sulphide, K_sp = 6.3 × 10^–18). 

$1.$ $5.02$ $\times {10}^{-9}$ $\mathrm{M}$

$2.$ $5.02$ $\times$ ${10}^9$ $\mathrm{M}$

$3.$ $2.$ $25$ $\times$ ${10}^{-13}$ $\mathrm{M}$

$4.$ $\mathrm{Can}\text{'}\mathrm{t}$ $\mathrm{predict}$

If the solubility product of CuS is 6 × 10^–16, the maximum molarity of CuS in an aqueous solution will be:
1. 1.45 × 10⁻⁸ mol L⁻¹
2. 3.45 × 10⁻⁸ mol L⁻¹
3. 2.45 × 10⁻⁸ mol L⁻¹
4. 4.25 × 10⁻⁸ mol L⁻¹

The ionization constant of benzoic acid is 6.46×10⁵ and K_sp for silver benzoate is 2.5×10^–13. Silver benzoate is x times more soluble in a buffer of pH 3.19 compared to its solubility in pure water. The value of x will be:

1. 6.8 

2. 16.8 

3. 33.3 

4.  3.3 

The solubility product of silver chromate is $1.1\times {10}^{-12}$. The solubility of silver chromate will be:

1. $6.5\times {10}^{-5}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

2. $6.5\times {10}^{-6}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

3. $5.5\times {10}^{-5}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

4. $5.5\times {10}^{-6}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

The solubility product of mercurous iodide is $4.5\times {10}^{-29}$. The solubility of mercurous iodide will be:

1. $6.5\times {10}^{-7}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

2. $2.24\times {10}^{-10}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

3. $4.09\times {10}^{-7}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

4. $6.5\times {10}^{-8}\mathrm{mol}$ ${\mathrm{L}}^{-1}$