Week 10 Homework
EDTA & Precipitation Titrations and visual representation of titrations
- A 40.00 mL solution contains 30.00 mM Co3+ is to be titrated with a 25.00 mM solution of EDTA. Both the cobalt and EDTA solution are buffered to a pH of 10.00. Determine the concentration of cobalt as pCo3+ (pCo3+ = –㏒[Co3+]) for the volumes of titrant listed in the table below.
Vol. Titrant Added | Solution pCo3+ |
0.00 mL | |
26.00 mL | |
30.50 mL | |
48.00 mL | |
50.00 mL | |
53.25 mL |
- A solution is prepared by mixing the two solutions together. The first solution is 150.0 mL and contains 30.78 mM Ti3+, 29.40 mM Ce3+, and 8.75 mM HCl. The second solution is 200.0 mL and contains 40.23 mM EDTA and 11.48 mM piperidine. Determine the concentration of free (non-complexed) metals when the two solutions are mixed.
- You wish to titrate all the mercury(I) by precipitation with cyanide because you like to play with dangerous chemicals. You obtain a 50.00 mL solution containing 18.00 mM Hg_{2}(NO_{3})_{2} and you titrate it with a 24.00 mM solution of KCN. Determine the concentration of Hg_{2}2+ and CN– at each of the titration volumes listed below.
Vol. Titrant Added | [Hg22+] | [CN–] |
20.00 mL | ||
46.00 mL | ||
68.00 mL | ||
75.00 mL | ||
80.00 mL | ||
90.00 mL |
For this problem I want you to sketch the titration curve for the acid-base titration that was done in problem #2 from the Week 8 homework (use the correct values from the posted solution if you didn’t get the answer correct). Once you have made the graph identify the following elements on the trace:
- The two equivalence points
- The two buffering regions