The electrodes in the following electrochemical cell are connected to a voltmeter as shown. The half-cell on the right contains a standard silver-silver chloride electrode (a silver wire coated with AgCl(s), as in questions 5 and 6).
AgCl (s) + e- → Ag(s) + Cl- (1 M) E° = 0.2223 V
The half-cell on the left contains a silver electrode immersed in 100.0 mL of 1.00 x 10-3 M AgNO3(aq). A porous plug through which ions can migrate separates the half-cells.
What is the voltmeter reading after 10.00 mL of 0.0100 M K2CrO4 has been added to the half-cell on the left and the mixture has been thoroughly stirred?
Hint: Ksp of Ag2CrO4 = 1.1 x 10-12
Voltmeter reading=0.76V
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