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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![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 NH4CI (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).
6C) Calculate the molar solubility of Ag2SO4 in 0.60 M AgNO3.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbdd570d-a0c9-44fd-80de-e8b53629889d%2Fa1a04b74-00fc-4a15-b8e3-f50c7ea3a316%2Fbcylexr_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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 NH4CI (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).
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 of
C5H5N 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 is
the 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) PH3
b) SiO32-
c) BrO3"
3C) Using 3A-a (C7H6O2) and its conjugate-base as an example, prove that "KąKp = Kw"
Search or type URL
く=](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbdd570d-a0c9-44fd-80de-e8b53629889d%2Fa1a04b74-00fc-4a15-b8e3-f50c7ea3a316%2Filtao49_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1A) Calculate 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) 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 is
the 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) PH3
b) 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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