question8 from final

# Question8 from final - V 3 e<=> V 2 E =-0.256 V Sn 4 2e<=> Sn 2 E 0 = 0.154 V a Draw(in shorthand notation the electrochemical cell for

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(2005) Given the following reduction potentials for uranium and tin: UO 2 2+ + 4H + + 2e U 4+ + 2H 2 O E O =+0.334V Sn 4+ + 2e Sn 2+ E o =+0.154V a) (i) Calculate E o for the following reaction. (ii) Give one reason why this reaction is suitable for a redox titration. UO 2 2+ + Sn 2+ + 4H + == Sn 4+ + U 4+ + 2 H 2 O b) A 50.0 mL solution of 0.050M UO 2 2+ buffered to pH 0.000 ([H + ]=1.00M) was titrated with 0.100M Sn 2+ and the potential of the redox system measured with a platinum electrode. (i) Calculate the potential of the electrode when 12.50mL of the Sn 2+ solution has been added. (ii) Calculate the potential at the equivalence point. (2004) 8) The standard reduction potentials for vanadium and tin ions are:
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Unformatted text preview: V +3 + e- <=> V +2 E = -0.256 V Sn +4 + 2e-<=> Sn +2 E 0 = +0.154 V a) Draw (in shorthand notation) the electrochemical cell for the following reaction, and calculate the standard cell potential. Sn +4 + 2 V +2 <=> 2 V +3 + Sn +2 b) Calculate the cell potential if [Sn +4 ]=0.051M, [Sn +2 ]=0.318M, [V +2 ]=0.00822M, [V +3 ]=0.119M. In which direction will the reaction occur under these circumstances? c) Briefly describe how Sn +4 can be used to carry out a redox titration of V +2 d) Calculate the cell potential at the equivalence point....
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## This note was uploaded on 12/11/2009 for the course CHM Chm2354 taught by Professor Teitlebaum during the Spring '09 term at University of Ottawa.

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