Calculate the solubility of AgI in a 10⁻⁴ M KI solution at 25°C, given that the solubility product constant (Kₛₚ) of AgI
is 1.0 × 10⁻¹⁶ mol² L⁻².

1. $1.0\times {10}^{-10}$

2. $1.0\times {10}^{-12}$

3. $1.0\times {10}^{-16}$

4. $1.0\times {10}^{-8}$

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. \(8 \times10^{-11} M~\)
2. \(6 \times10^{-5} M~\)
$\mathrm{}$3. \(1.6 \times10^{-11} M~\)
4. \(8 \times10^{-2} ~M~ \)$\mathrm{}$

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

Given the following equilibrium reactions:

Ag⁺ + 2NH₃ ⇌ [Ag(NH₃)₂]⁺  K₁ = 1.8 × 10⁷

Ag⁺ + Cl⁻ ⇌ AgCl(s)  K₂ = 5.6 × 10⁹

Calculate the equilibrium constant for the reaction:

AgCl(s) + 2NH₃ ⇌ [Ag(NH₃)₂]⁺ + Cl⁻

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

Find the solution(s) having a pH between 6 and 7.

I. 2 × 10⁻⁶ M NaOH
II. 2 × 10⁻⁶ M HCl
III. 10⁻⁸ M HCl
IV. 10⁻¹³ M NaOH

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

1. Three (3)

2. Six (6)

3. Nine (9)

4. Eleven (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:

The pH of a 0.05 M aqueous solution of diethylamine is 12. Its K_b value will be:

1. $2\times {10}^{-3}$

2. $2.5\times {10}^{-3}$

3. $3\times {10}^{-3}$

4. $4.5\times {10}^{-3}$

K_a for HCN is $5\times {10}^{-10}$ at $25°\mathrm{C}$. For maintaining a constant pH of 9, the volume of 5 M KCN solution required to be added to 10 mL of 2 M HCN solution is-

1. 2 mL

2. 3 mL

3. 4.2 mL

4. 5.6 mL