The hydrolysis constant (Kh) of NH₄Cl is 5.6 × 10⁻¹⁰. The concentration of H₃O⁺ in a 0.1 M solution of NH₄Cl… · ABC26PH0742

Subject: Physical Chemistry · Chapter: Ionic Equilibrium · Topic: Ionic Equilibrium – General · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Medium

The hydrolysis constant ($K_h$) of $\mathrm{NH_4Cl}$ is $5.6 \times 10^{-10}$. The concentration of $\mathrm{H_3O^+}$ in a 0.1 M solution of $\mathrm{NH_4Cl}$ at equilibrium is

(a)$\sqrt{5.6 \times 10^{-11}}$

(b)$\sqrt{5.6 \times 10^{-10}}$

(c)$5.6 \times 10^{-10}$

(d)$2.8 \times 10^{-5}$

Answer

Answer: A ✓ checked by 4AB · confidence high

Explanation

[H₃O⁺] = √(K_h·c) = √(5.6 × 10⁻¹⁰ × 0.1) = √(5.6 × 10⁻¹¹) (a).

Study loop for Ionic Equilibrium

1. Practise the PYQsPrevious-year questions, with answers

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