Find the pH of a 0.183 M aqueous solution of hypobromous acid (HOBr),for which K_a = 2.06 ×10^-⁹.

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Quizplus · Accepted Answer

The pH of a weak acid solution can be calculated using the formula pH = -log[H⁺], where [H⁺] is the concentration of hydrogen ions. For a weak acid HA, [H⁺] can be approximated by √(Ka × [HA]). Here, [HA] = 0.183 M and Ka = 2.06 × 10⁻⁹. Calculating [H⁺] gives √(2.06 × 10⁻⁹ × 0.183) ≈ 1.94 × 10⁻⁵ M. Thus, pH = -log(1.94 × 10⁻⁵) ≈ 4.712.

Find the PH of a 0