18. Aqueous Equilibrium

Consider the titration of a 26.0-mL sample of 0.175 M CH3NH2 (Kb = 4.4 × 10^(-4)) with 0.150 M HBr. Determine the pH at one-half of the equivalence point.

Consider the titration of a 26.0-mL sample of 0.175 M CH3NH2 (Kb=4.4×10⁻⁴) with 0.150 M HBr. Determine the pH at the equivalence point.

Pyridine, C5H5N, is a weak base with Kb = 1.5 x 10^-9. What is the pH at the equivalence point when 238 mL of 0.78 M pyridine is titrated with 0.78 M HCl?

Pyridine, C5H5N, is a weak base with Kb = 1.5 x 10^-9. What is the pH at the equivalence point when 384 mL of 0.78 M pyridine is titrated with 0.78 M HCl?

What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL of aqueous ammonia (NH3) requires 37.10 mL of 0.1087 mol L^-1 HCl? pKb = 4.75 for ammonia. Report your answer to 2 decimal places.