0.5 M NaOH. Write the acid base reaction that is taking place and use an ICE table to show how the number of moles of each species changes. What is the final pH of the buffer solution? (The pK of acetic acid is 4.7.)
0.5 M NaOH. Write the acid base reaction that is taking place and use an ICE table to show how the number of moles of each species changes. What is the final pH of the buffer solution? (The pK of acetic acid is 4.7.)
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
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Transcribed Image Text:2. Making a buffer solution. Suppose you add 100 mL of a solution containing 5M of acetic acid to 400 mL of
0.5 M NaOH. Write the acid base reaction that is taking place and use an ICE table to show how the number of
moles of each species changes. What is the final pH of the buffer solution? (The pK of acetic acid is 4.7.)
a
Expert Solution
Step 1: Number of moles of each species
Number of moles in 100mL of 5M acetic acid can be calculated by the formula
Volume in L × concentration (mol/L)/M
volume = 100mL = 0.1 L
0.1 × 5 = 0.5 mol
In case of NaOH ( 400mL of 0.5M )
400mL = 0.4 L
0.4 × 0.5 = 0.2 mol
The reaction equation is
>CH3COOH + NaOH ---‐----> CH3COONa + H2OConstructing ICE table
| [CH3COOH] | [NaOH] | [CH3COONa] | |
| Initial | 0.5 mol | 0.2mol | 0 |
| Change | - 0.2 mol | -0.2mol | 0.2 mol |
| Equilibrium | 0.3 mol | 0 | 0.2 mol |
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