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Data Table 1: Adding 0.1 M HCl from D1 to A1
With a solution of 0.01 moles of sodium acetate, in order to find the molarity of sodium
acetate to add to the solution, the following equation as below:
pH=pKa+log(sodium acetate/acetate acid
5.47=4.74+log(sodium acetate/1)
log(sodium acetate)=5.47-4.74
log(sodium acetate)=0.53
Number of moles of Sodium acetate = 100.53 = 3.39 moles.
We would need a sodium acetate molarity of 3.39 moles
6. An acetic acid buffer solution is required to have a pH of 5.27. You have a
solution that contains 0.01 mol of acetic acid. What molarity of sodium
acetate will you need to add to the solution? The pK of acetic acid is 4.74.
Show all calculations in your answer.
a
Number of Drops pH of Solution
0
2
4
6
8
10
12
14
16
6.0
6.0
6.0
6.0
6.0
6.0
6.0
6.0
6.0

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Data Table 2: Adding 0.1 M NaOH from D6 to A6
Data Table 3: Adding 6 M HCl from Pipet into B1
Data Table 4: Adding 6 M NaOH from Pipet into B6
Number of Drops pH of Solution
0
2
4
6
8
10
12
14
16
6.0
6.0
6.0
6.0
6.0
6.0
6.0
6.0
6.0
Number of Drops pH of Solution
0
2
4
6
8
10
6.0
6.0
5.0
4.0
4.0
3.0

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Data Table 5: Adding 0.1 M HCl from D1 into C1
Data Table 6: Adding 0.1 M NaOH from D6 into C6
Number of Drops pH of Solution
0
2
4
6
8
10
6.0
7.0
8.0
8.0
9.0
11.0
Number of Drops pH of Solution
0
2
4
6
8
10
6.0
5.0
4.0
4.0
3.0
2.0

Competency Review
Number of Drops pH of Solution
0
2
4
6
8
10
6.0
7.0
8.0
9.0
11.0
11.0
1. A chemical buffer is a solution that increases pH changes when small
quantities of an acid or base are added.
2. Every buffer that is made has a certain _____ and _____. 3. Weak acids make better buffers than strong acids because they have _____.
Copyright 2021 - Science Interactive |

Copyright 2021 - Science Interactive |