Assume you dissolve 0.235 g of the weak acid benzoic acid, C₆H₅CO₂H, in enough water to make 1.00 × 10² mL of solution and then titrate the solution with 0.108 M NaOH.

(a) What was the pH of the original benzoic acid solution?
(b) What are the concentrations of all of the following ions at the equivalence point: Na⁺, H₃O⁺, OH⁻, and C₆H₅CO₂⁻?
(c) What is the pH of the solution at the equivalence point?

Transcribed Image Text:

C6H5CO₂H(aq) + OH-(aq) → C6H5CO₂ (aq) + H₂O(l)