4) A 2.00 L buffer solution is 0.200 M in HF and 0.400 M in KF. Calculate the pH of the solution after the addition of 16.00 g of NaOH to this solution. (Assume the volume change is negligible). The Ka for HF is 3.5 x 10-4. 5) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4C1 (which will dissociate into NH4+ ions) with 100.0 mL of 0.20 M NH3. The Kb for NH3 is 1.8 x 10-5. 6A) Calculate the molar solubility of silver sulfate Ag2SO4 in water (Ksp = 1.1 x 10-12). 6B) Calculate the solubility in mg / L. (Molar mass = 311.8 g/mol). %3D 6C) Calculate the molar solubility of Ag2S04 in 0.60 M AgNO3.
4) A 2.00 L buffer solution is 0.200 M in HF and 0.400 M in KF. Calculate the pH of the solution after the addition of 16.00 g of NaOH to this solution. (Assume the volume change is negligible). The Ka for HF is 3.5 x 10-4. 5) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4C1 (which will dissociate into NH4+ ions) with 100.0 mL of 0.20 M NH3. The Kb for NH3 is 1.8 x 10-5. 6A) Calculate the molar solubility of silver sulfate Ag2SO4 in water (Ksp = 1.1 x 10-12). 6B) Calculate the solubility in mg / L. (Molar mass = 311.8 g/mol). %3D 6C) Calculate the molar solubility of Ag2S04 in 0.60 M AgNO3.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter13: Acids And Bases
Section: Chapter Questions
Problem 174CP
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