14 IMPORTANT!! When entering your answer in scientific notation you must use the

Question

14

IMPORTANT!! When entering your answer in scientific notation you must use the "e". Example: for 1 times 10-3, you enter 1e-3 or 1e-03. (a) The Ksp of Cu(OH)2 is 4.8 times 10-20, calculate the concentration of Cu+2 at equilibrium. Cu(OH)2(s, excess) Cu+2(aq) + 2OH-(aq) The Ksp of Zn(OH)2 is 3.0 times 10-16, calculate the equilibrium concentration of OH-. Zn(OH)2(s, excess) Zn+2(aq) + 2OH-(aq) (Common Ion Problem)Excess Ag2CO3 is added to an 0.2 M K2CO3solution. Calculate the equilibrium concentration of Ag+ under these conditions.Ksp for Ag2CO3 is 8.1 times 10-12. Ag2CO3(s, excess) 2Ag+(aq) + CO3-2(aq)

Explanation / Answer

Ksp = [reactant 1]^n * [reactant 2]^m and represents the solubility of the reactants

m,n = number of moles

For number 1:

Cu(OH)2 < -- > Cu^2+ + 2 OH^ -

There are two moles of OH for every one mole of Cu for every Cu(OH)2 molecule broken down. Each molar equivalent will be the same.

Given the Ksp, we know how much the solid Cu(OH)2 will dissociate.

For every Cu(OH)2 broken down, we can find the concentrations through the Ksp equation above.

4.8e-20 = [x]^1 * [x]^2 = x^3

x = cuberoot (4.8e-20) = 3.63e-7 M

[Cu^ 2+ ] = x = 3.63e-7 M

[OH^ -] = 2 * x = 2 * 3.63e-7 = 7.26e-7 M

Let me know if this works in the comments. If it does, I can help you out with the other two if you can't figure them out from this process. My apologies again if this doesn't work.

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