Consider the titrtation of 25.0mL of 0.0100M Sn2+ by 0.0500M Ti3+ in 1 M HCL, using Pt and Saturated Calomel Electrodes to find the endpoint.
F=96486.7 Cmol
E0 Sn4+/Sn2+ =0.15V
E0 TI3+/TI+ = 1.28
Esce = 0.241V
R=8.3141 J K Mol
(a) Write the balanced reaction.
Sn4+ + 2e- <--> Sn2+
TI3+ <--> TI+ + 2e-
Sn2+ + Tl3+- -> Sn4+ + Tl+
(b) Write two different half reactions for the net cell reaction.
I'm assuming this means
Sn4+ + 2e- <--> Sn2+ E0= 0.15V
TI3+ <--> TI+ + 2e- E0= 1.28 V
(c) Write the two nernst equations for the net cell reaction
Prior to the equivalence point, the equation would be;
E=1.28+RT/F ln(TI3+/TI+)-SCE (0.241)
Where TI3+/TI+ = Conc. products/reactants.
After the equivalence point, reaction then becomes,
E=0.15 + RT/F ln(Sn4+/Sn2+) - SCE
(D) calculate E at the following volumes of TI3+ : 1.00mL, 2.50mL, 4.90mL, 5.00mL,5.10mL and 10.0mL
This is the section I am having difficulty with, if anyone could help, thanks.
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