Question

(a) When 300.0 milliliters of a solution of 0.200 molar AgNO3 is mixed with 100.0 milliliters of a 0.0500 molar CaCl2 solution, what is the concentration of silver ion after the reaction has gone to completion?

(b)Write the net cell reaction for a cell formed by placing a silver electrode in the solution remaining from the reaction above and connecting it to a standard hydrogen electrode.

(c)Calculate the voltage of a cell of this type in which the concentration of silver ion is 410-2 M.

(d)Calculate the value of the standard free energy change ∆G˚ for the following half reaction:
Ag+ (1M) + e- ⁄ Ag˚

Answer 1

(a) When 300.0 milliliters of a solution of 0.200 molar AgNO3 is mixed with 100.0 milliliters of a 0.0500 molar CaCl2 solution, what is the concentration of silver ion after the reaction has gone to completion?
<B>
2AgNO3 + CaCl2 ==> 2AgCl + Ca(NO3)2

initial:
AgNO3 = M x L = 0.06 moles.
CaCl2 = M x L = 0.005 moles.

CaCl2 is limiting reagent; 0.005 moles react to leave 0 moles CaCl2 and 0.06-0.005 = 0.055 moles AgNO3 unreacted.(It forms 0.005 moles solid AgCl which ppts).
Concn of AgNO3 remaining after reaction is ?moles/?L = 0.055 moles/0.400 L = ??

Answer 2

.138M