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 50.0 mL of 0.20 M NH3 (Kb=1.8×10⁻⁵) with 0.20 M HNO3. Calculate the pH after the addition of 50.0 mL of the titrant at 25 °C.

Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. What is the initial pH of the CH3NH2 solution before any HBr is added?

Consider the titration of a 26.0-mL sample of 0.185 M CH3NH2 (Kb=4.4×10⁻⁴) with 0.155 M HBr. What is the pH after adding 6.0 mL of HBr?

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 5.0 mL of added acid.

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.