4) A 2.00 L buffer solution is 0.200 M in HF and 0.400 M in KF. Calculate the pH of thesolution after the addition of 16.00 g of NaOH to this solution. (Assume the volume change isnegligible). 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 NH4CI (which willdissociate 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).6C) Calculate the molar solubility of Ag2SO4 in 0.60 M AgNO3. 1A) Calculate the concentration of C5H5N solution required to provide a pH of 9.29. The Kb ofC5H5N is 1.7 × 10-9 at 25°C.1B) Calculate the mass of C5H5N needed to prepare 2.20 L of the above solution. (Molar mass =79.10 g/ mol)2A) The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10, What isthe pH of an aqueous solution of 0.80 M sodium cyanide (NaCN)?2B) What would be pH of the above solution if NaCN was a strong base?3A) Write the conjugate base of the following:a) C7H602. b) HCO3-c) ) HASO3²-3B) Write the conjugate acid of the following:a) PH3b) SiO32-c) BrO3"3C) Using 3A-a (C7H6O2) and its conjugate-base as an example, prove that "KąKp = Kw"Search or type URLく=

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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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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