To ensure the measurements of your indicator electrode are accurate, several tim

Question

To ensure the measurements of your indicator electrode are accurate, several times each day a 10.00 mL sample of the plating bath is analyzed by coulometry. In the procedure, the 10.00 mL of solution are added to enough 1.0M KCI to make 100.0 mL of a solution that is then analyzed. If the initial solution was 4.0 M, how much charge, in Coulombs, should have flowed through the cell in the electrolysis process? In other words, how many coulombs should have flowed if you electrolyzed all the Cu^2+ present? 7720 Coulombs 6425 Coulombs 7050 Coulombs 8750 Coulombs

Explanation / Answer

answer : 7720 coulombs

solution:

moles of Cu+2 = 4 x 10 / 1000 = 0.04

1 mole Cu+2 -------------------> 96485 x 2 Coulombs needed

0.04 mole Cu+2 --------------> 0.04 x 2 x96485 = 7718.8 coulombs = 7720 C

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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