auth-6.php

auth-6.php - y Use the Henderson-Hasselbalch equation to...

Info iconThis preview shows pages 1–11. Sign up to view the full content.

View Full Document Right Arrow Icon
Buffers y Buffered Solution – a solution that resists changes to its pH. It contains a weak acid and its conjugate base or a weak base and its conjugate acid.
Background image of page 1

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

View Full DocumentRight Arrow Icon
Buffers y Calculate the concentrations of all species present, the pH, and the percent dissociation of HC 2 H 3 O 2 (K a = 1.8 x 10 -5 ) in a solution of 0.025 M HC 2 H 3 O 2 and 0.010M NaC 2 H 3 O 2 .
Background image of page 2
Buffers y Excess H + will react with the conjugate base forming more weak acid y Excess OH - will react with the weak acid forming more conjugate base y Recalculate the equilibrium concentrations, pH , percent dissociation, or whatever is asked for
Background image of page 3

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

View Full DocumentRight Arrow Icon
Buffers y Calculate the pH change that occurs when 0.005 mol HCl is added to 1.0 L of the buffered solution described in the previous example. Compare this pH to that of a solution containing 0.005 mol HCl in 1.0 L of water.
Background image of page 4
Henderson-Hasselbalch Equation Lawrence Joseph Henderson 1878 – 1942 American Biochemist Karl Albert Hasselbalch 1874 – 1962 Danish Chemist • Derived a relationship between pH, K a and the concentrations of the conjugate acid base pair in solution.
Background image of page 5

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

View Full DocumentRight Arrow Icon
Henderson-Hasselbalch Equation
Background image of page 6
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
Background image of page 9

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

View Full DocumentRight Arrow Icon
Background image of page 10
Background image of page 11
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 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 ). K a = 1.8 x 10-4 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 Which of the following solutions will have the greatest buffering capacity? 100 m L of 0. 8 M HN. . 100 mL of 0.30 M H. .. 1 o f .1 M H. 05 M H. 90% 3% 3% 4% 1. 100 mL of 0.80 M HNO 2 /0.80 M NaNO 2 2. 100 mL of 0.30 M HNO 2 /0.30 M NaNO 2 3. 100 mL of 0.10 M HNO 2 /0.10 M NaNO 2 4. 100 mL of 0.05 M HNO 2 /0.05 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....
View Full Document

Page1 / 11

auth-6.php - y Use the Henderson-Hasselbalch equation to...

This preview shows document pages 1 - 11. Sign up to view the full document.

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