A mixture having a volume of 10.00 mL and containing 0.1000 M Ag+ and 0.04500 M Hg22+ was titrated with 0.0800 M KCN to precipitate Hg2(CN)2 and AgCN.
-
-
Calculate volume of KCN required to reach first and second equivalence points
and sketch by hand the expected titration curve.
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Calculate pCN- at 8.00 mL KCN added.
A mixture having a volume of 10.00 mL and containing 0.1000 M Ag+ and 0.04500 M Hg22+ was titrated with 0.0800 M KCN to precipitate Hg2(CN)2 and AgCN.
-
-
Calculate volume of KCN required to reach first and second equivalence points
and sketch by hand the expected titration curve.
-
Calculate pCN- at 8.00 mL KCN added.
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Related questions
5. A 40 mL aliquot of 0.0500 M HNO2 is diluted to 75.0 mL and titrated with 0.0800 M Ce4+ Assume the [H+ ] = 1.00M throughout the titration. Use +1.44 V as the formal potential of the cerium system.
(a) Calculate the potential of the indicator electrode with respect to a Ag/AgCl(satâd) reference electrode after the addition the each volumes of Ce4+ solution listed in the adjacent table
. (b) Construct a titration curve for based upon the data and determine the equivalence point using first- and second derivative plots. Does the volume at which the 2nd â derivative plot crosses zero correspond to the theoretical equivalence point? Why or why not? The following redox equation may be useful:
Ce4+ + e- <-> Ce3+ Eo= 1.44v
NO-3 + 3H+ + 2e- <-> HNO2 + H2O Eo = 0.94V
Volume of Ce(IV) solution added (mL) |
5.00 |
10.00 |
15.00 |
20.00 |
25.00 |
30.00 |
35.00 |
40.00 |
45.00 |
49.00 |
49.50 |
39.60 |
49.70 |
49.80 |
49.90 |
49.95 |
49.99 |
50.00 |
50.01 |
50.05 |
50.10 |
50.20 |
50.30 |
50.40 |
50.50 |
51.00 |
55.00 |
60.00 |
75.00 |
90.00 |
NO