The precipitate of CaF₂ $({\mathrm{K}}_{\mathrm{sp}}=1.7\times {10}^{-10})$ is obtained when equal volumes of the following are mixed

1. ${10}^{-2} \mathrm{M} {\mathrm{Ca}}^{2+}+{10}^{-3} {\mathrm{MF}}^{-}$

2. ${10}^{-3} \mathrm{M} {\mathrm{Ca}}^{2+}+{10}^{-5} {\mathrm{MF}}^{-}$

3. ${10}^{-4} \mathrm{M} {\mathrm{Ca}}^{2+}+{10}^{-4} {\mathrm{MF}}^{-}$

4. ${10}^{-5} \mathrm{M} {\mathrm{Ca}}^{2+}+{10}^{-3} {\mathrm{MF}}^{-}$

In the exothermic reaction of oxidizing SO₂ by O₂ to SO₃, what factors determine the maximum yield of SO₃?

If a solution of 0.1 M NH₄OH and 0.1 M NH₄Cl has pH 9.25, then the pK_b of NH₄OH will be:

Among the following , the compound with highest pH is : 

1. CH₃COOK

2. Na₂CO₃ 

3. NH₄Cl

4. NaNO₃

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the concentrations of the conjugate acid (HIn) and base (In^-) forms of the indicator by the expression: 

1. $\log \left[\frac{{\mathrm{In}}^{-}}{\mathrm{HIn}}\right]={\mathrm{pK}}_{\mathrm{In}}-\mathrm{pH}$

2. $\log \left[\frac{\mathrm{HIn}}{{\mathrm{In}}^{-}}\right]={\mathrm{pK}}_{\mathrm{In}}+\mathrm{pH}$

3. $\log \left[\frac{\mathrm{HIn}}{\mathrm{In}}\right]=\mathrm{pH}-{\mathrm{pK}}_{\mathrm{In}}$

4. $\log \left[\frac{\mathrm{In}}{\mathrm{HIn}}\right]=\mathrm{pH}-{\mathrm{pK}}_{\mathrm{In}}$

Solubility of a M₂S salt is $3.5\times {10}^{-6}$ then find out solubility product.

1. $1.7\times {10}^{-6}$

2. $1.7\times {10}^{-16}$

3. $1.7\times {10}^{-18}$

4. $1.7\times {10}^{-12}$

The solubility of MX₂ type electrolyte is $0.5\times {10}^{-4}$ mol L^-1. Then find out K_sp of electrolytes.

1. $5\times {10}^{-12}$

2. $25\times {10}^{-10}$

3. $1\times {10}^{-13}$

4. $5\times {10}^{-13}$

The solubility product of a sparingly soluble salt AX₂ is $3.2\times {10}^{-11}$.  Its solubility (in mol L^–1) is:

1. $5.6\times {10}^{-6}$

2. $3.1\times {10}^{-4}$

3. $2\times {10}^{-4}$

4. $4\times {10}^{-4}$

What is the degree of ionization of an acid solution with a concentration of 0.005 M and a pH of 5?
 

1. $0.1\times {10}^{-2}$

2. $0.2\times {10}^{-2}$

3. $0.5\times {10}^{-4}$

4. $0.6\times {10}^{-6}$

pKa value of four acids are given below. The strongest acid is

(I) 4.0

(II) 3.5

(III) 2.5

(IV) 2

1. I

2. II

3. III

4. IV