071608 - 1874 – 1962 Danish Chemist Henderson-Hasselbalch Equation y Use the Henderson-Hasselbalch equation to calculate the pH of a buffer

Info iconThis preview shows pages 1–19. Sign up to view the full content.

View Full Document Right Arrow Icon
APPLICATIONS OF AQUEOUS EQUILIBRIA Zumdahl Chapter 15
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Common Ion y Common Ion – y Common Ion Effect –
Background image of page 2
Common Ion 0.025 M HCN 0.025 M HCN 0.010 M NaCN
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Common Ion y In 0.15 M NH 3 , the pH is 11.21 and the percent dissociation is 1.1 %. Calculate the concentration of all species present, the pH, and the percent dissociation of ammonia in a solution that is 0.15 M NH 3 and 0.45 M NH 4 Cl.
Background image of page 4
Common Ion
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Buffers y Buffered Solution –
Background image of page 6
Buffers y Calculate the concentrations of all species present, the pH, and the percent dissociation of HCN (K a = 4.9 x 10 -10 ) in a solution of 0.025 M HCN and 0.010M NaCN.
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 8
Buffers y Calculate the pH change that occurs when 0.010 mol HCl is added to 1.0 L of the buffered solution described on the previous slide. Compare this pH change with that which occurs when 0.010 mol HCl is added to 1.0 L of water.
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Buffers
Background image of page 10
Buffers
Background image of page 11

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Henderson-Hasselbalch Equation Lawrence Joseph Henderson 1878 – 1942 American Biochemist Karl Albert Hasselbalch
Background image of page 12
Background image of page 13

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 14
Background image of page 15

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 16
Background image of page 17

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 18
Background image of page 19
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 1874 – 1962 Danish Chemist Henderson-Hasselbalch Equation y Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.25 M in formic acid (HCHO 2 ) and 0.50M in sodium formate (NaCHO 2 ). Henderson-Hasselbalch Equation y What happens to the pH of the solution on the previous slide when the solution is diluted by a factor of two? Buffering Capacity Buffering Capacity y Which of the following solutions has the greater buffer capacity? { 100 mL of 0.30 M HNO 2 /0.30 M NaNO 2 { 100 mL of 0.10 M HNO 2 /0.10 M NaNO 2 Preparing a Buffer y In what volume ratio should you mix 1.0 M solutions of NH 4 Cl and NH 3 to produce a buffer solution having a pH 9.80. (NH 3 K b = 1.8 x 10-5 ) Preparing a Buffer y Using the following table determine the best acid and its conjugate base that would best form a buffer with a pH of 2.9. Buffers: A Summary...
View Full Document

This note was uploaded on 07/22/2008 for the course CHEM 105A taught by Professor Bau during the Summer '04 term at USC.

Page1 / 19

071608 - 1874 – 1962 Danish Chemist Henderson-Hasselbalch Equation y Use the Henderson-Hasselbalch equation to calculate the pH of a buffer

This preview shows document pages 1 - 19. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online