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Given the solubility-product constant, what is the ion concentration?
The solubility-product constant for Ce(IO3)3 is 3.2*10^-10
What is [Ce3+] in a solution prepared by mixing 50 mL of .05 M Ce3+ with 50 mL of .05 M IO3-?
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Attempt at solution (what I know so far):
.0025 mol Ce3+
.0025 mol IO3-
Ce(IO3)3 <----> Ce3+ + 3 IO3-
ksp = [Ce3+] [IO3-]^3
The answer is 1.7*10^-2 M. Does anyone know how to get to that?
2 Answers
- reb1240Lv 79 years agoFavorite Answer
you have the moles of each, but you must convert that to molarity. They are now both in 100 mL of solution, so they are both 0.025M. Then follow your set up
- 9 years ago
Try using an ICE table.
-------------------Ce3+ +. 3 IO3- <--> Ce(IO3)3
Initial.-----------0.0025. 0.0025
Change.------ -0.0025/3. -0.0025
Equilibrium.-- 1.67x10^-3. 0
No. of moles of Ce3+ = 1.67x10^-3
Concentration of Ce3+
= no. of moles of Ce3+ / total volume
= 1.67x10^-3 / [(50+50)/1000]
= 1.67x10^-2, which is 1.7x10^-2 after rounding up
