A student measures the potential of a cell made up with 1 M CuSO4in one solution

Question

A student measures the potential of a cell made up with 1 M CuSO4in one solution and 1 M AgNO3 in the other. There is a copperelectrode in the CuSO4 and a silver electrode in the AgNO3. Thecopper electrode is negative.

-from this i figured that the copper electrode is the anode: Cu (s)--> Cu2+ (aq) + 2e-
and the silver electrode cathode: Ag+ (aq) + e- -->Ag(s)    (plz tell me if these arewrong)

Question: The student adds 6 M NH3 to the CuSO4 solution until theCu2+ ion is essentially all converted toCu(NH3)2+4 ion. The cell voltage,Ecell, increases to 0.92 V and the copper electrode isstill negative. Find the concentration of Cu2+ ion in the cell.

They gave this equation in the lab manual: Ecell = E°cell -0.0592/2 x log ([Cu2+]/[Ag+]2)

I've tried it already, but am totally confused by the equation.Please help show me how to solve this,thanks in advance :)

Explanation / Answer

Next, we have Ecell, which is the reduction potential undernon standard conditions, and this was provided in theproblem.
Then there is the concentration of silver and copper; we knowthe concentration of silver from the given information and we nowhave to solve for the copper concentration.
actually reduction potenial is given always or u can refer any bookor chk the web for dat
sometimes the oxidation potenial is given so just put a minus toconvert to reduction potenial!!!

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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