In: Chemistry
From one of the documents, Determination of Ka of a weak acid Version Version 42-0151-00-02, they got the answers Data5 Table 3. Determination of Unknown pKa of Unknown Weak Acid: 4.75 Ka of Unknown Weak Acid: 1.76 x 10-5 % error pKa: 0% % Error Ka: 1.67% Can someone show work on how they got this?
Drops NaOH Added |
pH Value Trial 1 |
pH Value Trial 2 |
pH Value (Average) |
---|---|---|---|
Half-Equivalent Point = (53 Drops) |
4 |
5 |
4.5 |
Equivalent Point = (106 Drops) |
8 |
8.5 |
8.5 |
0 |
2 |
2 |
2 |
10 |
2 |
3 |
2.5 |
20 |
3 |
3 |
3 |
30 |
4 |
4 |
4 |
40 |
4 |
4 |
4 |
50 |
4 |
5 |
4.5 |
60 |
6 |
6 |
6 |
70 |
6 |
7 |
6.5 |
80 |
7 |
7 |
7 |
90 |
7 |
7 |
7 |
100 |
8 |
7 |
7.5 |
110 |
8 |
8.5 |
8.5 |
120 |
13 |
13 |
13 |
This is all about making a graph, here´s a graph for your ph value at half equivalence point = 5
you know where is your equivalence point, now you need to determine where is your half eequivalence point, it is at the half of it
I´m using your value of 53 drops (approximately because it is a graph method)
you have to read the ph from the half equivalence point which is 5
at half equivalence point PH = PKa, you can repeat this same procedure for the other graph , you already have that info the ph at 50 drops is 4 and 5, that´s why pka are 4 and 5 for this trials
Remember that PKa = - log (ka)
so the exact value is 4.75 for pka
ka = 10-pka = 10-4.75 = 1.778 x10-5
Ka for experiment (from average ph = 4.5)
ka = 10-pka = 10-4.5 = 3.162 x10-5
% error is ( theoretical value - actual value) / theoretical value * 100
pka experimntal average = 4.5
Pka theoretical = 4.75
% error = (4.75 - 4.5) / 4.75 = 0.052 * 100 = 5.2% error for pka
similarly for ka you will get a value of 77.8% error
this constrast your information but this is the formula, it depends on the values you are trying to compare.
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