(a) The Ksp of Cu(OH)2 is 4.8 x 10-20, calculate the concentration of Cu+2 at eq
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(a) The Ksp of Cu(OH)2 is 4.8 x 10-20, calculate the concentration of Cu+2 at equilibrium. Cu(OH)2(s, excess)Cu+2(aq) + 2OH-(aq) (b) The Ksp of Zn(OH)2 is 3.0 x 10-16, calculate the equilibrium concentration of OH-. Zn(OH)2(s, excess)Zn+2(aq) + 2OH-(aq) (c) (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 x 10-12. Ag2CO3(s, excess)2Ag+(aq) + CO3-2(aq)Explanation / Answer
a) The Ksp of Cu(OH)2 is 4.8 x 10-20, calculate the concentration of Cu+2 at equilibrium. Cu(OH)2(s) --> Cu+2(aq) + 2OH-(aq) Cu(OH)2(s) --> [X] + [2X] Ksp = [Cu+2] [OH-]^2 4.8 e-20 = [X] [2X]^2 4X3 = 4.8 e-20 X3 = 1.2 e-20 X = [Cu+2] = 2.3 X 10^-7 Molar ======================================… b) The Ksp of Zn(OH)2 is 3.0 x 10-16, calculate the equilibrium concentration of OH-. Zn(OH)2(s) > Zn+2(aq) + 2OH-(aq) Zn(OH)2(s) > [X] + [2X] Ksp = [Zn+2] [OH-]^2 3.0 e-16 = [X] [2X]^2 4X3 = 3.0 e-16 X3 = 7.5 e-17 X = 4.2 e-6 2X = [OH-] = 8.4 X 10^-6 Molar ======================================… c) 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 x 10^-12. Ag2CO3(s) > 2Ag+(aq) + CO3-2(aq) Ksp = [Ag+]^2 [CO3-2] 8.1 e-12 = [Ag+]^2 [0.2 Molar] [Ag+]^2 = 4.05 e-11 [Ag+] = 6.4 X 10^-6 Molar but because the "0.2 M K2CO3" has only 1 sig fig, you might be expected to round off to [Ag+] = 6 X 10^-6 Molar
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