Posted by **Maggie** on Monday, April 12, 2010 at 7:44pm.

Hi, I have a few chemistry problems that I'm having trouble solving. I put my attempted solutions after the problems in *'s. There was one problem I had no idea how to solve.

What concentration of silver chromate (Ksp = 9.0 x 10-12) will dissolve to make a saturated solution in water?

*For this one the formula is Ag2CrO4, which is [Ag]^2[CrO4]. I plugged x in for CrO4, so x^3 is equal to Ksp. I then got that x = 2.0e-4. However, that x is for CrO4, not for silver chromate. Is the answer for silver chromate just the Ksp value?*

What concentration of silver chromate (Ksp = 9.0 x 10-12) will dissolve in 500. mL of 0.01 M aqueous silver nitrate?

A saturated solution of CaSO4(aq) is made in a beaker until there is excess calcium sulfate resting at the bottom. Then solid potassium sulfate is added. Which of the following is true? (The Ksp for potassium sulfate is larger than the Ksp for calcium sulfate)

a. More calcium sulfate will start to precipitate out of solution

b. More calcium sulfate will start to dissolve in solution

*I know that when a smaller Ksp is added to a bigger Ksp it precipitates out of solution. Is that the same in the reverse?*

How does the solubility of AgCl in pure 1.0 M NaCl(aq) compare with its solubility in pure water?

*It is less, right? because there are already chloride ions present.*

- Chemistry -
**DrBob222**, Monday, April 12, 2010 at 11:09pm
Worked above.

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