A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5. A)4.74 B)9.26 C)11.13 D)13.00 E)12.55

Question

Quizplus · Accepted Answer

The pH of the solution before any HNO₃ is added is determined by the ammonia solution itself. Ammonia is a weak base, and its pH can be calculated using the formula for the pH of a weak base: pH = 14 - pOH, where pOH = -log(√(Kb × [NH₃])). Substituting the given values, pOH ≈ 2.87, so pH ≈ 14 - 2.87 = 11.13.

A 1000 ML Sample of 0