A Cu2+ solution is prepared by dissolving a 0.4749 g piece of copper wire in acid. The solution is then passed through a Walden reductor, reducing Cu2+ to Cu+ . The resulting Cu+ solution required 40.15 mL of each of the titrants to reach the endpoint. Calculate the concentration of each titrant.

Concentration of = 0.03101 M

Concentration of = 0.03721 M

Explanation:

A)

The reduction for is;

6 moles of = 1 mole of

number of moles of Cu reacted =

number of moles of Cu reacted =

number of moles of Cu reacted = 0.00747 mole

number of moles of reacted =

number of moles of reacted = 0.001245 mole

Concentration of =

Given that the volume = 40.15 mL = ; we have:

Concentration of =

Concentration of = 0.03101 M

B)

The reduction for is;

5 moles of = 1 mole of

number of moles of Cu reacted =

number of moles of Cu reacted =

number of moles of Cu reacted = 0.00747 mole

number of moles of reacted =

number of moles of reacted = 0.001494 mole

Concentration of =

Given that the volume = 40.15 mL = ; we have:

Concentration of =

Concentration of = 0.03721 M