Volume of NaOH added (mL) |
pH of the solution (measured) |
Mols of CH3COO-formed |
Mols CH3COOH remained |
pH of the solution (calculated) |
0.00 |
2.72 |
0 |
0.005 |
2.70 |
10.00 |
4.57 |
0.002 |
0.003 |
4.57 |
12.50 |
4.7 |
0.0025 |
0.0025 |
4.75 |
24.90 |
7.14 |
0.0049 |
2 x 10-5 |
7.14 |
24.99 |
8.14 |
0.00 |
2 x 10-6 |
8.15 |
25.00 |
8.88 |
0.005 |
0 |
8.88 |
25.01 |
9.60 |
0.05 |
0 |
9.60 |
25.10 |
10.60 |
0.005 |
0 |
10.60 |
26.00 |
11.59 |
0.0052 |
0 |
11.59 |
35.00 |
12.52 |
0.007 |
0 |
12.52 |
a. Find the pH at equivalent point
b. find the concentration of H+ ions at the equivalence point
Please show work.
The following table shows the data for the titration of 25.00 mL of 0.200 M CH3COOH...
8. Calculate the pH for the following cases in the titration of 25.00 mL of 0.200-M acetic acid, CH3COOH(aq), with 0.200 M NaOH(aq): (a) before addition of any NaOH(aq) (b) after addition of 5.00 mL of NaOH(aq) (c) after addition of 12.50 mL of NaOH(aq) (d) after addition of 25.00 mL of NaOH(aq) (e) after addition of 26.00 mL of NaOH(aq)
Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. How many mL of NaOH is required to reach the equivalence point? Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. What will the initial pH of the analyte be if 0.00 mL of NaOH is added?