What is the pH in the following reaction: HI ⇌ H⁺ + I^- , if the [HI] = 0.250 M and K = 1 × 10^-6?

Question

Quizplus · Accepted Answer

The pH of the solution can be calculated using the dissociation constant (K) and the concentration of HI. Given K = 1 × 10^-6 and [HI] = 0.250 M, we can set up the equation for the dissociation of HI into H+ and I- ions. Since K is small, we can assume that the change in concentration of HI due to dissociation is negligible, and thus [H+] ≈ [I-] at equilibrium. Using the formula K = [H+][I-]/[HI], we find that [H+]^2 = K[HI] = (1 × 10^-6)(0.250) = 2.5 × 10^-7. Taking the square root gives [H+] = 1.58 × 10^-4 M. The pH is then calculated using pH = -log[H+], which gives a pH of approximately 3.30.

What Is the PH in the Following Reaction: HI ⇌