Determine the molar solubility of NiC2O4 in the following solutions.
a) pure water
b) 150.0 mL of a 0.010 M Ni(NO3)2
c) 150.0 mL of a 0.500 M AlCl3.
d) 150.0mL of a 0.030 M Na2C2O4
Ksp for NiC2O4 = Ksp = 4×10−10 (please note that Ksp dat achanges drastically between references, ensure this is near to your KSP data)
a)
pure water
NiC2O4 <--> Ni+2 + C2O4-2
Ksp = [Ni2+][C2O42]
Ksp = S*S
S =Sqrt(KS) = sqrt(4.10*10^-10) = 0.000020 M of NiC2O4
b)
if
Ni(NO3)2 is present, then
[Ni+2] = 0.01 M is fixed
therefore
Ksp = [Ni2+][C2O42]
4.10*10^-10= 0.01*[C2O42]
[C2O2-2] = (4.10*10^-10 / (0.01) = 4.1*10^-8 M
c)
if AlCl3 is present, no effect (ignore activities and side reactions)
Ksp = S*S
S =Sqrt(KS) = sqrt(4.10*10^-10) = 0.000020 M of NiC2O4
d)
Na2C2O4 --> 2Na + C2O4-2
[C2O4-2] = 0.03 M fixed so
Ksp = [Ni2+][C2O42]
4.10*10^-10= [Ni2+]*0.03
[C2O2-2] = (4.10*10^-10) / (0.03) = 1.3666*10^-8 M
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