Determine the pH of the following solution. Initial concentrations are given. [HC₂H₃O₂] = 0.250 M, [NaC₂H₃O₂] = 0.120 M [Ka = 1.8 × 10^-5] A) 5.1 B) 4.4 C) 8.9 D) 9.6 E) 7.0

Question

Quizplus · Accepted Answer

1. Write the balanced equation for the dissociation of HC₂H₃O₂: HC₂H₃O₂ + H2O ⇌ H3O+ + C₂H₃O- 2. Write the expression for the equilibrium constant: Ka = [H3O+][C₂H₃O-] / [HC₂H₃O₂] 3. Substitute the given concentrations into the expression and solve for [H3O+]: Ka = 1.8 × 10^-5 = [H3O+][0.120] / [0.250] [H3O+] = 6.48 × 10^-5 4. Convert [H3O+] to pH: pH = -log[H3O+] = -log(6.48 × 10^-5) ≈ 4.4 Therefore, the answer is B.

Determine the PH of the Following Solution