A compound BA₂ has \(K_{sp} = 4\times 10^{-12}\)$.$ Solubility of this compound will be:

If the solubility of a ${\mathrm{M}}_2\mathrm{S}$ salt is $3.5$ $\times$ ${10}^{-6}$ mol litre^-1 , then the solubility product of ${\mathrm{M}}_2\mathrm{S}$ will be:

1. $1.7$ $\times$ ${10}^{-6}$ mol³ litre^-3

2. $1.7$ $\times$ ${10}^{-16}$ mol³ litre^-3

3. $1.7$ $\times$ ${10}^{-18}$ mol³ litre^-3

4. $1.7$ $\times$ ${10}^{-12}$ mol³ litre^-3

If the solubility of MX₂ – type electrolytes is 0.5 × 10^–4 Mole/lit. then K_sp of electrolytes will be:

1. $5\times {10}^{-12}$

2. $25\times {10}^{-10}$

3. $1\times {10}^{-13}$

4. $5\times {10}^{-13}$

Calculate the solubility of AgI in a 10⁻⁴ N KI solution at 25°C, given that the solubility product constant (Kₛₚ) of AgI is 1.0 × 10⁻¹⁶ mol² L⁻².

1. $1.0\times {10}^{-16}$

2. $1.0\times {10}^{-12}$

3. $1.0\times {10}^{-10}$

4. $1.0\times {10}^{-8}$

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10^–11. Its solubility (in moles/litre) is: