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vera_ewing
 one year ago
At equilibrium, the concentration of calcium ions in a calcium chromate (CaCrO4) solution is 1 x 10^–4 mol/L at 25°C. In the same solution, the concentration of chromate ions is also 1 x 10^–4 mol/L. What is the Ksp of calcium chromate? Show your work.
vera_ewing
 one year ago
At equilibrium, the concentration of calcium ions in a calcium chromate (CaCrO4) solution is 1 x 10^–4 mol/L at 25°C. In the same solution, the concentration of chromate ions is also 1 x 10^–4 mol/L. What is the Ksp of calcium chromate? Show your work.

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vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1@aaronq Please help!

welshfella
 one year ago
Best ResponseYou've already chosen the best response.0sorry I've forgotten this stuff

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1Write the dissociation, then it's corresponding equilibrium equation (which is the Ksp equation). Plug in your values and solve

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1What's the dissociation and corresponding equilibrium equation?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1the dissociation of CaCrO4 (in water)

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1and by that i mean a chemical equation

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1Okay, so what does the chemical equation look like? Can you set it up and then I solve?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1nah, you have to try it

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1I don't know how :( Can you maybe explain it?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1CaCrO4 is an ionic compound, right? what ions make up CaCrO4?

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1Not sure. It's covalent and ionic though, right?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1it's ionic only. You should be able to identify the ions here, if you can't look the compound up on wikipedia and read a little about it

welshfella
 one year ago
Best ResponseYou've already chosen the best response.0what i do remember is that Ca CrO4 disassociates in water to [Ca++] and [Cr2O4 ]

welshfella
 one year ago
Best ResponseYou've already chosen the best response.0and sp means solubility product so i guess Ksp is the product of Ca++ ions and CrO4 ions

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.1Yep, I figured it out :) thanks

welshfella
 one year ago
Best ResponseYou've already chosen the best response.0so that 104 8 10^4 = 10^8

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0CaCrO4 > Ca^2+ + CrO4^2 Ksp = [Ca^2+][CrO4^2] Ksp = [x][x] Ksp = concentration of ions dissolved, like any K it's an equilibrium value, and it is temperature dependent. I'm assuming that the equilibrium is already reached and that the solution is saturated. B.c from my understanding that's what Ksp is. (Qsp = Ksp) Their concentrations are equal for both ions in the problem. So I think it's (1x10^4)(1x10^4) = Ksp. 10^8
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