1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point.c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is:NaOH (aq) + HCl (aq) → NaCl (aq) + H 2O (l) Table of experimental data for the titration of an HCIsolution of unknown concentration with 0.100 M NaOHsolutionVolume of 0.100 M NaOH added (mL) pH of solution0.01.005.01.1810.01.3715.01.6020.01.9522.02.2024.02.6924.53.0024.93.7025.07.0025.110.3025.511.0026.011.2928.011.7530.011.9635.012.2240.012.3645.012.4650.012.52Titration plot of strong acid HCl of unknown concentration with0.100 M NaOH solution14.0013.0012.0011.0010.009.008.007.006.005.004.003.002.001.000.000.05.010.015.020.025.030.035.040.045.050.055.0Volume of 0.100 M NaOH added (mL)pH of Solution

From the graph it is clear that the pH increases during the titration of acids by bases .

Answered: . Answer the following, use the data…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.8QAP

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1. Answer the following, use the data and plot as a reference, answer the following questions:
a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?
b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point.

c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is:
NaOH (aq) + HCl (aq) → NaCl (aq) + H ₂O (l)

Table of experimental data for the titration of an HCI
solution of unknown concentration with 0.100 M NaOH
solution
Volume of 0.100 M NaOH added (mL) pH of solution
0.0
1.00
5.0
1.18
10.0
1.37
15.0
1.60
20.0
1.95
22.0
2.20
24.0
2.69
24.5
3.00
24.9
3.70
25.0
7.00
25.1
10.30
25.5
11.00
26.0
11.29
28.0
11.75
30.0
11.96
35.0
12.22
40.0
12.36
45.0
12.46
50.0
12.52
Titration plot of strong acid HCl of unknown concentration with
0.100 M NaOH solution
14.00
13.00
12.00
11.00
10.00
9.00
8.00
7.00
6.00
5.00
4.00
3.00
2.00
1.00
0.00
0.0
5.0
10.0
15.0
20.0
25.0
30.0
35.0
40.0
45.0
50.0
55.0
Volume of 0.100 M NaOH added (mL)
pH of Solution

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