CuCO3 2H2O CuOH2 H2CO3 with this balanced equation of coppe

CuCO3+ 2H2O -> Cu(OH)2 +H2CO3

with this balanced equation of copper carbonate , calculate the concentration of copper in solution (the voltage is .22V) and then calculate the value of Ksp for copper (II) carbonate

Solution

CuCO3 (s)<=> Cu+2 (aq) & CO3)-2 (aq)



b)write the equilibrium expression (Ksp) for the reaction in (a)
Ksp = [Cu+2] [CO3 -2]


c)Using the experimental cell potential ( .22V), calculate the concentration of copper in the saturated solution
this experiment usually
compare the [Cu+2] level in the beaker with CuCO3, with the [Cu+2 level in a 1 molar solution. it is called a concentration cell
the reduction @ cathode has Cu+2 & 2 e- --> Cu ...... ...... Eo = +0.34
while the reverse, oxidation @ anode Cu --> Cu+2 & 2 e- Eo = - 0.34
for the reaction:
Cu+2 & Cu --> Cu+2 & Cu
the standard voltage for a concentration cell is zero

but because the CuCO3 lowers the [Cu+2], that cell will have an EMF of a lower voltage by 0.22 v
nernst equation:
E = Eo - (0.0592 / n) (log Q)

0.22 = zero - (0.0592 / 2 mol e- ) (log prod / reactants)

0.22 = zero - (0.0296) (log [Cu+2] / [Cu+2])

for the cell to work, i,e, to proceed ---> --->
the higher \"usually 1Molar Cu+2\" must be the reactant
0.22 = - (0.0296) (log [Cu+2] / [1M])

0.22 = - (0.0296) (log [Cu+2] )

0.22 / - (0.0296) = (log [Cu+2] )

log [Cu+2] = -7.432

10^x for both sides:
[Cu+2] = 8.711 e-7 Molar