Voltaic Cells and the Nernst Equation: A test solution contained 2 mL of 0.10 M

Question

Voltaic Cells and the Nernst Equation: A test solution contained 2 mL of 0.10 M Ag+. A silver strip was dipped into the test solution, and a cell potential of 0.0592 V was measured against an Ag/Ag+ (1.0M) reference half-cell. Then 2 mL of 0.50 M S2O32- was added to the test solution. No precipitate formed. The cell potential of the test solution was measured against the reference half-cell, and was found to have increased to 0.532 V. What is the [Ag+] in the test solution after the S2O32- was added? (Reminder: the Nernst Equation is given in Table 24 of the Chem Data Sheet.)

Explanation / Answer

Nernst Equation: E=E^o-(0.0592/n)logQ

0.532=0.0592-(0.0592/1)log(0.1/[Ag+])
Ag+=1x10^-9

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