**Buffer and Solubility Calculations**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 \( K_a \) for HF is \( 3.5 \times 10^{-4} \).---5) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M \( \text{NH}_4\text{Cl} \) (which will dissociate into \( \text{NH}_4^+ \) ions) with 100.0 mL of 0.20 M \( \text{NH}_3 \). The \( K_b \) for \( \text{NH}_3 \) is \( 1.8 \times 10^{-5} \).---6A) Calculate the molar solubility of silver sulfate \( \text{Ag}_2\text{SO}_4 \) in water (\( K_{sp} = 1.1 \times 10^{-12} \)).6B) Calculate the solubility in mg/L. (Molar mass = 311.8 g/mol).6C) Calculate the molar solubility of \( \text{Ag}_2\text{SO}_4 \) in 0.60 M \( \text{AgNO}_3 \). ### Chemistry Problem Set#### 1A) Concentration of C₅H₅N SolutionCalculate the concentration of C₅H₅N solution required to provide a pH of 9.29. The Kb of C₅H₅N is 1.7 × 10⁻⁹ at 25°C.#### 1B) Mass of C₅H₅N for Solution PreparationCalculate the mass of C₅H₅N needed to prepare 2.20 L of the above solution. (Molar mass = 79.10 g/mol)---#### 2A) pH of NaCN SolutionThe acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10⁻¹⁰. What is the pH of an aqueous solution of 0.80 M sodium cyanide (NaCN)?#### 2B) pH with NaCN as a Strong BaseWhat would be the pH of the above solution if NaCN was a strong base?---#### 3A) Conjugate BasesWrite the conjugate base of the following:a) C₇H₆O₂b) HCO₃⁻c) HAsO₃²⁻#### 3B) Conjugate AcidsWrite the conjugate acid of the following:a) PH₃b) SiO₃²⁻c) BrO₃⁻#### 3C) Prove \( K_aK_b = K_w \)Using 3A-a (C₇H₆O₂) and its conjugate base as an example, prove that \( K_aK_b = K_w \).

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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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