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

At room temperature, MY and NY₃, two nearly insoluble salts, have the same K_sp values of 6.2 × 10^-13. The true statement regarding MY and NY₃ is:

Given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ is 2 × ${10}^{-\mathrm{15 }}$. The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH is ;
1. 2 × ${10}^{-8}$ M

The solubility of BaSO₄ in water is $2.42$ $\times$ ${10}^{-3}$ g/ litre at 298 K. The value of the solubility product will be: (Molar mass of BaSO₄ = 233 gmol^–1)

The solubility of AgCl (s) with solubility product 1.6×10^–10 in 0.1 M NaCl solution would be?

When equal volumes of the following solutions are mixed, in which case will AgCl (K_sp = 1.8×10^–10) precipitate?

1. 10^–4 M Ag⁺ and 10^–4 M Cl^–

2. 10^–5 M Ag⁺ and 10^–5 M Cl^–

3. 10^–6 M Ag⁺ and 10^–6 M Cl^–

4. 10^–10 M Ag⁺ and 10^–10 M Cl^–