Use the nernst equation to calculate the cell potentials of the following cells at 298K: a.) Cu(s) + PtCl62-(0.10M) -> Cu2+(aq)(0.20M) + PtCl42-(aq)(0.10M) + 2Cl-(aq)(0.40M) b.)Pb(s) + SO42-(aq)(0.30M)+2AgCl(s) -> PbSO4(s) + 2Ag(s) + Cl-(aq)(0.20M)
Use the nernst equation to calculate the cell potentials of the following cells at 298K: a.) Cu(s) + PtCl62-(0.10M) -> Cu2+(aq)(0.20M) + PtCl42-(aq)(0.10M) + 2Cl-(aq)(0.40M) b.)Pb(s) + SO42-(aq)(0.30M)+2AgCl(s) -> PbSO4(s) + 2Ag(s) + Cl-(aq)(0.20M)
Chapter21: Potentiometry
Section: Chapter Questions
Problem 21.26QAP
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1. Use the nernst equation to calculate the cell potentials of the following cells at 298K:
a.) Cu(s) + PtCl62-(0.10M) -> Cu2+(aq)(0.20M) + PtCl42-(aq)(0.10M) + 2Cl-(aq)(0.40M)
b.)Pb(s) + SO42-(aq)(0.30M)+2AgCl(s) -> PbSO4(s) + 2Ag(s) + Cl-(aq)(0.20M)
2. One-half cell in a voltaic cell is constructed from a silver wire dipped into a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.0 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag+(aq).
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