We have titration of 20,0 mL of Sn2+(aq) 0,00500 M with Ce4+ 0,0200 M in HCl 1 M

Question

We have titration of 20,0 mL of Sn2+(aq) 0,00500 M with Ce4+ 0,0200 M in HCl 1 M that gives Sn4+ and Ce3+. The equivalent point is found par potentiometric method with Pt as electrode indicator and the referencen electrode is a type Ag/AgCl (EAg/AgCl = 0,197V) a) Write down the balanced reaction of this redox titration. Which the analyte and which the titrant b) Calculate the standard potential of redox reaction and equilibrium constant c) Calculate the cell potential after adding 7,50 ml, 10,0 ml and 10,10 ml of Ce4+

Explanation / Answer

a) Sn(+2) (aq) + Ce(+4) (aq) + e- = Sn(+4) (aq) + Ce(+3) (aq)

analyte - Sn +2 solution .

titrant - Ce+4 solution

b) Reduction potentials of each individual steps needs to be specified

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.