acid-base titration labUse Ka (calculate this first) to find the initial pH for your sample and compare the calculated and experimental results.Possible hint: calculate the concentration of the KHP at the start of the titration by assuming that the measured amount of KHP was dissolved in 50mL of water (provided in screenshot)I found the calculated experimental Ka = 8.7096 x 10^-6Refresher: from datapoints, I found equivalenct point and halfway point, found pKa since pH = pKa. found Ka by 10-Ka Data collectedExperimental ProcedureWeigh accurately about 0.51g of KHP and pourinto a clean dry beaker. Add 50mL of distilledwater and swirl until the solid has dissolved.Vol ofNaOHpHaddedUsing a calibrated pH meter, measure the initialpH of the solution.Titrate by adding successive portions of about1mL of the NaOH solution from the buret.Record the buret reading and the pH after eachaddition. Decrease portions to 0.2mL when thepH increase by more than 0.3 pH units.Continue the titration until the pH is about 11.5-12216.(mL)226.24422.26.3114.0522.46.424.1822.66.4634.2922.86.5844.41236.7154.5123.26.894.623.47.2374.6523.68.55Procedure for Part One84.7723.89.3894.86Standardization of NaOH solution:24.19.93104.93KHC3H,O4 + NaOH → KNAC3H,04 + H2O24.410.3211125.0824.610.55The exact molarity of the NaOH solution can bedetermined from the mass of KHP, its molar massand the total volume of NaOH at the equivalencepoint determined from the graph.2510.84135.15145.232611.19155.312711.38165.3828.0511.5175.472911.58Questions185.583011.66195.693111.721. Find equivalence point from the data points.2. Calculate molarity of the NaOH solution fromthe result (equivalence point).3. Find volume and pH at the halfway point.205.823211.774. Using pka, find Ka for KHP.

KHP is slightly acidic. It dissociates as KHP⇔KP-+H+

Answered: Use Ka (calculate this first) to find…

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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acid-base titration lab

Use Ka (calculate this first) to find the initial pH for your sample and compare the calculated and experimental results.

Possible hint: calculate the concentration of the KHP at the start of the titration by assuming that the measured amount of KHP was dissolved in 50mL of water (provided in screenshot)

I found the calculated experimental Ka = 8.7096 x 10^-6

Refresher: from datapoints, I found equivalenct point and halfway point, found pKa since pH = pKa. found Ka by 10^-Ka

Data collected
Experimental Procedure
Weigh accurately about 0.51g of KHP and pour
into a clean dry beaker. Add 50mL of distilled
water and swirl until the solid has dissolved.
Vol of
NaOH
pH
added
Using a calibrated pH meter, measure the initial
pH of the solution.
Titrate by adding successive portions of about
1mL of the NaOH solution from the buret.
Record the buret reading and the pH after each
addition. Decrease portions to 0.2mL when the
pH increase by more than 0.3 pH units.
Continue the titration until the pH is about 11.5-
12
21
6.
(mL)
22
6.24
4
22.2
6.31
1
4.05
22.4
6.4
2
4.18
22.6
6.46
3
4.29
22.8
6.58
4
4.41
23
6.71
5
4.51
23.2
6.89
4.6
23.4
7.23
7
4.65
23.6
8.55
Procedure for Part One
8
4.77
23.8
9.38
9
4.86
Standardization of NaOH solution:
24.1
9.93
10
4.93
KHC3H,O4 + NaOH → KNAC3H,04 + H2O
24.4
10.32
11
12
5.08
24.6
10.55
The exact molarity of the NaOH solution can be
determined from the mass of KHP, its molar mass
and the total volume of NaOH at the equivalence
point determined from the graph.
25
10.84
13
5.15
14
5.23
26
11.19
15
5.31
27
11.38
16
5.38
28.05
11.5
17
5.47
29
11.58
Questions
18
5.58
30
11.66
19
5.69
31
11.72
1. Find equivalence point from the data points.
2. Calculate molarity of the NaOH solution from
the result (equivalence point).
3. Find volume and pH at the halfway point.
20
5.82
32
11.77
4. Using pka, find Ka for KHP.

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