Calculate the pH of a solution that has [H₃O⁺] = 5.2 × 10^-7 M. A)pH = 5.20 B)pH = 6.28 C)pH = 7.00 D)pH = 5.27 E)pH = 7.72

Question

Quizplus · Accepted Answer

This appears to be a bit of a trick question, as the given concentration is not for a known acid or base. However, we can still use the concept of acid dissociation to calculate the pH. Based on the brackets in the given concentration, we can assume that we are dealing with an acid with the formula H₃O⁺. We can write the acid dissociation reaction as: H₃O⁺ ⇌ H+ + ₃O-. The acid dissociation constant (Ka) can be calculated by taking the product of the equilibrium concentrations of the products (H+ and ₃O-) and dividing by the equilibrium concentration of the reactant (H₃O⁺). Using the given concentration of the acid, we can assume that the initial concentration of H+ is negligible, so we can simplify the expression to: Ka = [H+][₃O-] / [H₃O⁺] We can then use the Ka expression to calculate the concentration of H+ at equilibrium, and then use that to calculate the pH. This calculation gives a pH of 6.28. Therefore, the answer is B.

Calculate the PH of a Solution That Has [H3O+] =

Calculate the PH of a Solution That Has [H₃O⁺] =