Chemistry questions and answers. A. A 75.0-mL volume of 0.200 mol L^-1 NH3 (Kb=1.8×10^−5) is titrated with 0.500 mol L^−1 HNO3. Calculate the pH after the addition of 13.0 mL of HNO3 . B. A 52.0-mL volume of 0.350 mol L^−1 CH3COOH (Ka=1.8×10^−5. ) is titrated with 0.400 mol L^−1 NaOH. Calculate the pH after the addition of 19.0 mL 1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Kb, NH3 = 1.8 × 10−5. Determine the pH of the solution at each of the following points in the titration: (a) Calculate the volume (mL) of HCl required to reach the equivalence point. Plot the points from part (c) on a graph. Answer to Solved Calculate th pH of 0.00756 M HNO3.. based on rules. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Determine the pH of the solution after the addition of 200.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4. A) 3.34 B) 3.57 C) 3.46 D) 2.89 E) 3.63. B. Vay Tiền Trả Góp 24 Tháng.

calculate ph of hno3