You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCl with 0.0500

Question

You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCl with 0.0500 M Ag to give Sn2 and Ag3 using a Pt indicator electrode and a saturated calomel electrode (SCE) as the reference electrode.

C) Choose the two different expressions for the potential of the cell, consisting of the Nernst equation forapdO each half-reaction minus the potential of the SCE (0.241 V) cac, holf reaction minlus thte potenisi o t the cell,consisting of the Nernst equation for 0.05916 Sn AE-0.139 0.241 2-0241 0.05916 In [B] E-0.139 [C] [ | |-0.241 Scroll down to answer part D of this question. Sn 0.059 16 log, CE0.139 -0.05916log E= 0.139 0.241 [A] [8] [C] In Sn-021 1tSn2j D E= 0.139-0.059 16 log 0.241 [D] [E] 0.05916 E E1.90 0.241 [G] [H] 3 + 0.05916 F E 1.90 0.241 Ag Ag 1-021 0.241 0.241

Explanation / Answer

B amd E are the correct options

)Fe3+ + e- <-> Fe2+ ... Eo =.732
Sn2+ <-> Sn4+ + 2e- ... Eo = .139

E- = 1.90 -(.05916/2)log([Ag+]/[Ag3+]) - 0.241
E+ = .139 -(.05916/2)log([Sn4+]/[Sn2+]) - 0.241

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