Given that the ionization constant (\(K_a\)) of acetic acid \((\text{CH}_3\text{COOH})\) is \(1.7 \times 10^{-5}\) and the concentration of hydrogen ions (\(\text{H}^+ \)) is \(3.4 \times 10^{-4}\), what is the initial concentration of acetic acid (\(\text{CH}_3\text{COOH}\))?

1. \(3 . 4 \times \left(10\right)^{- 4}\)

2. \(3 . 4 \times \left(10\right)^{- 3}\)

3. \(6 . 8 \times \left(10\right)^{- 4}\)

4. \(6 . 8 \times \left(10\right)^{- 3}\)

At $25°\mathrm{C}$ the dissociation constant of a base, BOH is $1.0\times {10}^{-12}$, the concentration of hydroxyl ions 0.01 M aqueous solution of the base would become

1. $2.0\times {10}^{-6} \mathrm{mol} {\mathrm{L}}^{-1}$

2. $1.0\times {10}^{-5} \mathrm{mol} {\mathrm{L}}^{-1}$

3. $1.0\times {10}^{-6} \mathrm{mol} {\mathrm{L}}^{-1}$

4. $1.0\times {10}^{-7} \mathrm{mol} {\mathrm{L}}^{-1}$

The solubility product of AgI at $25°\mathrm{C}$ is $1.0\times {10}^{-16} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$. The solubility of AgI in 10^-4 N solution of KI at $25°\mathrm{C}$ is :  (in mol L^-1)

1. $1.0\times {10}^{-10}$

2. $1.0\times {10}^{-8}$

3. $1.0\times {10}^{-16}$

4. $1.0\times {10}^{-12}$

When 0.1 mole of CH₃NH₂ (ionization constant ${\mathrm{K}}_{\mathrm{b}}=5\times {10}^{-4}$) is mixed with 0.08 mol HCl and the volume is made up of 1 litre. The [H⁺] of resulting solution is -

(log 4 =  0.60)

1. $8\times {10}^{-2}$

2. $2\times {10}^{-11}$

3. $1.23\times {10}^{-4}$

4. $8\times {10}^{-11}$

The solution with pH value close to 1.0 among the following is:

If ${\mathrm{Ag}}^{+}+2{\mathrm{NH}}_3\rightleftharpoons \mathrm{Ag}{{\left({\mathrm{NH}}_3\right)}_2}^{+}; {\mathrm{K}}_1=1.8\times {10}^7$

${\mathrm{Ag}}^{+}+{\mathrm{Cl}}^{-}\rightleftharpoons \mathrm{AgCl}; {\mathrm{K}}_2=5.6\times {10}^9$

Then for

$\mathrm{AgCl}+2{\mathrm{NH}}_3\rightleftharpoons {\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+}+{\mathrm{Cl}}^{-},$

Equilibrium constant will be

1. $0.32\times {10}^{-2}$

2. $3.11\times {10}^2$

2. $10.08\times {10}^{16}$

4. $1.00\times {10}^{-17}$

Three sparingly soluble salts A₂X, AX, and AX₃ have the same solubility product. Their solubilities will be in the order:

1. AX₃>AX>A₂X

2. AX₃ < A₂X>AX

3. AX>AX₃>A₂X

4. AX>A₂X>AX₃

Which of the following solution(s) have pH between 6 and 7?

I. $2\times {10}^{-6} \mathrm{M}\hspace{0.17em}\mathrm{NaOH}$

II. $2\times {10}^{-6} \mathrm{M}\hspace{0.17em}\mathrm{HCL}$

III. ${10}^{-8} \mathrm{M}\hspace{0.17em}\mathrm{HCl}$

IV. ${10}^{-13} \mathrm{M}\hspace{0.17em}\mathrm{NaOH}$

1. I, II

2. II, III

3. III, IV

4. II, III, IV

At what pH does Mg(OH)₂ start to precipitate from a solution with 0.10 M Mg²⁺ ions, given that the Ksp of Mg(OH)₂ is 1 × 10⁻¹¹?

1. 3

2. 6

3. 9

4. 11

50 litres of 0.1 M HCl are mixed with 50 litres of 0.2 M NaOH. The pH of the resulting solution will be:

1. 12.70

2. 12.34

3. 8.7

4. 4.2