Question

Determine the molar solubility of NiC2O4 in the following solutions. a) pure water b) 150.0 mL...

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

Homework Answers

Answer #1

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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