The molar solubility of a sparingly soluble salt (cation : anion ratio is 1 : 2) is 6.80E-7 M. Calculate the

Ksp
(Tol: ± 5E-020)
concentration of the cation (M)
(Tol: ± 1E-009)
concentration of the anion (M)
(Tol: ± 1E-008)

Question

The molar solubility of a sparingly soluble salt (cation : anion ratio is 1 : 2) is 6.80E-7 M. Calculate the


Ksp 
 (Tol: ± 5E-020) 
concentration of the cation (M) 
 (Tol: ± 1E-009) 
concentration of the anion (M) 
 (Tol: ± 1E-008)

lena772 · Answer

@matt101

matt101 · Answer

Try to work through this one the same way I worked through the last one. Doesn't matter what the identities of the ions are, just as long as you know their ratio and how to set up the general Ksp equation for them!

Let me know if you have any questions!

lena772 · Answer

I got the concentrations right but my ksp is wrong @matt101

matt101 · Answer

Can I see your calculation for Ksp?

lena772 · Answer

Ksp=[cation][anion]

ksp=(0.00000136)(6.80e-7)

matt101 · Answer

Don't forget about the exponents in your equation! Write out the dissociation reaction in its general form as I showed you, then generate your Ksp equation from that!