Question

Henry's constant for \[\ce{CH3Br_{(g)}}\] is 0.159 mol dm⁻³ bar⁻¹ 25°C. Calculate its solubility in water at 25°C, if its partial pressure is 0.164 bar.

Answer 1

Given:

Henry's constant for \[\ce{CH3Br_{(g)}}\] = K_H = 0.159 mol dm⁻³ bar⁻¹

Partial pressure (P) = 0. 164 bar

To find:

Solubility, S = ?

Formula:

S = K_HP

S = 0.159 × 0.164

S = 0.02607 mol L⁻¹

∴ Solubility of \[\ce{CH3Br_{(g)}}\] at the given condition, is 0.2607 ≅ 0.0261 mol L⁻¹.