Determine the pH of the following aqueous solution.Initial concentrations are given.
[HF] = 1.296 M,[HCl] = 1.045 M K_a for HF is 6.6 × 10^-4

Question

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[HCl] = 1.045 M K_a for HF is 6.6 × 10^-4 A)14 B)3.1 C)3.2 D)-0.019 E)0.60

Quizplus · Accepted Answer

The presence of HCl, a strong acid, will dominate the pH calculation because it dissociates completely in water, unlike HF which is a weak acid. The concentration of H+ ions from HCl alone will be 1.045 M. To find the pH, use the formula pH = -log[H+]. Thus, pH = -log(1.045) ≈ -0.019. The contribution of HF to the H+ concentration is negligible compared to that of HCl.

Determine the PH of the Following Aqueous Solution