18. Aqueous Equilibrium

A 10.0 mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH. What is the pH at the equivalence point? For hydrocyanic acid, pKₐ = 9.31.

What is the pH at the equivalence point for the titration of 25.0 mL of 0.414 M HNO2 (Ka = 5.6 × 10^-4) with 0.414 M NaOH?

What is the pH of a 35.0-mL sample of 0.150 M acetic acid (CH3COOH, Ka=1.8×10⁻⁵) before any 0.150 M NaOH solution is added?

Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 x 10^-5) with 0.200 M NaOH. What is the pH of the solution at the equivalence point of the titration?

In a titration of a weak acid with a strong base, what determines the pH at the equivalence point?