Standard cell potentials are determined with 1.0 M solutions of ions. In this ex

Question

Standard cell potentials are determined with 1.0 M solutions of ions. In this experiment, we will use 0.10 M solutions of Zn2+, Cu2+, Pb2+, and Ag1+ to minimize the amount of hazardous waste generated. In this series of questions, you will figure out what effect this will have on the voltages you observe.

Consider a cell consisting of a Cu2+/Cu couple and an Ag1+/Ag couple.
(a) Starting with 1.0 M solutions of ions (standard conditions), evaluate Q in the Nernst Equation.
Q =

(b) What is log Q for this cell?
Q =

(c) The cell potential in this case should be which of the following?
less than E
greater than E
equal to E

(d) Starting with 0.1 M solutions of ions (at room conditions), evaluate Q in the Nernst Equation.
Q =

(e) What is log Q for this cell?
Q =

(f) The cell potential in this case should be which of the following?
less than E
greater than E
equal to E

Explanation / Answer

a) 1

B) 0

C) equal to 0

D) 10

E) 1

f) less than

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

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