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?

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 11.2 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

A 25.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. What is the pH of the solution after the addition of 15.0 mL of KOH? The Ka of HF is 3.5×10^-4.

Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 M HNO2 by 0.200 M KOH. (The pKa of nitrous acid is 3.34.)

For a titration of 1.0 M benzoic acid (C6H5COOH, Ka = 6.5×10^-5) with 1.0 M NaOH, what is the pH at the equivalence point?

What is the approximate pH at the equivalence point of a titration between formic acid (HCOOH) and sodium hydroxide (NaOH), given that 25 mL of formic acid is titrated with 29.80 mL of 0.1567 mol L⁻¹ NaOH? The acid dissociation constant (Ka) for formic acid is 1.8 × 10⁻⁴.

For a titration of a weak acid with a strong base, the pH at the equivalence point ________.