Solve all parts otherwise I will downvote 4. Determine the pH of an HCN/KCN buffer containing 0.10 mol HCN and o.070 mol KCNbefore and after the addition of 0.0010 mol HCl to 1.0 L of buffer.(Ka = 4.79 x 10-10) (before: 9.16 after: 9.15)%3D5. If 25 mL of 0.20 M NAOH(ag) is added to 50.0 mL of 0.10 M CH3COOH(a)(Ka = 1.8 x 10-5), what is the pH? (pH = 8.78)%3D!3!6. Calculate the mass of (NHA)2SO4ts) that must be added to 1.00 L of 0.50 M NH3(ag) in orderto prepare a buffer with a pH of 8.65. (Ka for NH*=5.6 x 10-10) (130 g)7. Calculate the pH of the solution prepared when 0.250 mol of HCIO, is added to 2.0 L of asolution containing 0.500 M CH;COOH(a) and 0.400 M CH3COONA(ag)-(Ka for CH,COOH = 1.8 x 10-5) (pH = 4.39)%3D8. A buffer is prepared in which the ratio of HCO,/CO,? is 5.00.a) What is the pH of this buffer? (Ka for HCO = 4.80 x 10-11) (pH = 9.62)b) Enough strong acid is added to make the pH of the buffer 9.30. What is the ratio ofHCO, /CO, at this point? (HCO,/Co, 1.0 X 10)

4.) We would use Henderson Hasselbalch equation to calculate pH before adding HCl . To calculate pH…

. Determine the pH of an HCN/KCN buffer containing 0.10 mol HCN and o.070 mol KCN before and after the addition of 0.0010 mol HCI to 1.0 L of buffer. (Ka = 4.79 x 10-10) (before: 9.16 after: 9.15) %3D

. Determine the pH of an HCN/KCN buffer containing 0.10 mol HCN and o.070 mol KCN before and after the addition of 0.0010 mol HCI to 1.0 L of buffer. (Ka = 4.79 x 10-10) (before: 9.16 after: 9.15) %3D

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 15.BCP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Solve all parts otherwise I will downvote

4. Determine the pH of an HCN/KCN buffer containing 0.10 mol HCN and o.070 mol KCN
before and after the addition of 0.0010 mol HCl to 1.0 L of buffer.
(Ka = 4.79 x 10-10) (before: 9.16 after: 9.15)
%3D
5. If 25 mL of 0.20 M NAOH(ag) is added to 50.0 mL of 0.10 M CH3COOH(a)
(Ka = 1.8 x 10-5), what is the pH? (pH = 8.78)
%3D
!3!
6. Calculate the mass of (NHA)2SO4ts) that must be added to 1.00 L of 0.50 M NH3(ag) in order
to prepare a buffer with a pH of 8.65. (Ka for NH*=5.6 x 10-10) (130 g)
7. Calculate the pH of the solution prepared when 0.250 mol of HCIO, is added to 2.0 L of a
solution containing 0.500 M CH;COOH(a) and 0.400 M CH3COONA(ag)-
(Ka for CH,COOH = 1.8 x 10-5) (pH = 4.39)
%3D
8. A buffer is prepared in which the ratio of HCO,/CO,? is 5.00.
a) What is the pH of this buffer? (Ka for HCO = 4.80 x 10-11) (pH = 9.62)
b) Enough strong acid is added to make the pH of the buffer 9.30. What is the ratio of
HCO, /CO, at this point? (HCO,/Co, 1.0 X 10)

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