Which of the following is an example of a reversible reaction?

1.	\(\small{KNO_3(aq) + NaCl(aq) \rightleftharpoons KCl(aq) + NaNO_3(aq)} \)
2.	\(\small{2Na(s) + H_2O(l) \rightleftharpoons 2NaOH(aq) + H_2(g)} \)
3.	\(\small{AgNO_3(aq) + NaCl(aq) \rightleftharpoons AgCl(s) + NaNO_3(aq)} \)
4.	\(\small{Pb{(NO_3)}_2(aq) + 2NaI(aq) \rightleftharpoons PbI_2(s) + 2NaNO_3(aq)} \)

A certain weak acid has a dissociation constant of $1.0\times {10}^{-4}.$ The equilibrium constant for its reaction with a strong base is

1. $1.0\times {10}^{10}$

2. $1.0\times {10}^{14}$

3. $1.0\times {10}^{-10}$

4. $1.0\times {10}^{-4}$

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

1. ${10}^{-2}<mspace\; width="1em"></mspace>\mathrm{M}<mspace\; width="1em"></mspace>{\mathrm{Ca}}^{2+}+{10}^{-3}<mspace\; width="1em"></mspace>{\mathrm{MF}}^{-}$

2. ${10}^{-3}<mspace\; width="1em"></mspace>\mathrm{M}<mspace\; width="1em"></mspace>{\mathrm{Ca}}^{2+}+{10}^{-5}<mspace\; width="1em"></mspace>{\mathrm{MF}}^{-}$

3. ${10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}<mspace\; width="1em"></mspace>{\mathrm{Ca}}^{2+}+{10}^{-4}<mspace\; width="1em"></mspace>{\mathrm{MF}}^{-}$

4. ${10}^{-5}<mspace\; width="1em"></mspace>\mathrm{M}<mspace\; width="1em"></mspace>{\mathrm{Ca}}^{2+}+{10}^{-3}<mspace\; width="1em"></mspace>{\mathrm{MF}}^{-}$

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 sharp pH change near the equivalence point in acid-base titration enables indicator detection. Which of the following equations correctly explains the pH change based on the concentration ratio of an indicator's conjugate acid (HIn) and base (In⁻) forms?

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. $4\times {10}^{-4}$