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. $2.0\times {10}^{-6}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}$

2. $1.0\times {10}^{-5}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}$

3. $1.0\times {10}^{-6}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}$

4. $1.0\times {10}^{-7}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}$

The solubility product of AgI at $25°\mathrm{C}$ is $1.0\times {10}^{-16}<mspace\; width="1em"></mspace>{\mathrm{mol}}^2<mspace\; width="1em"></mspace>{\mathrm{L}}^{-2}$. 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 \(Ag^+ + 2NH_3 \rightleftharpoons Ag(NH_3)_2^+ : K_1 = 1.8 \times 10^7\)
\(Ag^+ + Cl^-\rightleftharpoons AgCl : K_2 =5.6 \times 10^9\)
Then for \(AgCl + 2 NH_3 \rightleftharpoons [Ag(NH_3)_2]^+ + Cl^-\)
Equilibrium constant will be:
1. \(0.32 \times 10^{-2}\)
2. \(3.11 \times 10^2 \)
3. \(10.08 \times 10^{16} \)
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. \(2 \times 10^{-6}~ \text {M NaOH}\)
II. \(2 \times 10^{-6}~ \text {M HCl}\)
III. \( 10^{8}~ \text {M HCl}\)
IV. \(10^{-13}~ \text {M NaOH}\)

1. I, II
2. III only
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