[alexlinftw]

I had a question on my General Chem 2 Final about concentration and solubility:

I think it went something like this "If .1M of Ca(OH)2 was added to a Ca(OH)2 solution, what would happen to solubility? (Ksp of Ca(OH) = some number)"

The answer choices were raise, lower, or not change. I put that it would not change, but I'm not totally sure, could anyone please explain this to me?

I know that the Qsp = [Ca][OH]^2 but does that actually change the solubility?

Thanks,
-Alex Lin

[AWK]

If .1M of Ca(OH)2 was added to a . Ca(OH)2 solution, what would happen to solubility? (Ksp of Ca(OH).= some number)"

Something is missing

[Borek]

I wonder if it is not a trick question. Amount of dissolved substance may change, but solubility is constant.

It is like asking whether boiling point of water changes after an additional quart is added to a kettle.

[alexlinftw]

If .1M of Ca(OH)2 was added to a . Ca(OH)2 solution, what would happen to solubility? (Ksp of Ca(OH).= some number)"

Something is missing

I'm sorry I can't remember the whole question, the final was like three hours long and really tedious.

I wonder if it is not a trick question. Amount of dissolved substance may change, but solubility is constant.

It is like asking whether boiling point of water changes after an additional quart is added to a kettle.

I see, that's what I thought, thank you.