Answer to Question #213746 in Physical Chemistry for Shefe

Question

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: K_sp of Ag₂CrO₄ = 1.1 x 10^-12

Answer 1

Molar Mass of K2CrO4 = 194.1896

Molar Mass of Ag2CrO4 = 331.73

= 10×0.01×194.1896

= 19.41896

1.1 x 10^-12 ×331.73×100

= 3.65+19.42

= 23.07