Calculate Kc of the following reaction: CuBr(s)+Br-(aq)----> CuBr2-(aq) The solubility product constant, Ksp, for CuBr is 6.27× 10–9 and the overall formation constant, Kf (β2), for CuBr2– is 8.0× 105.
CuBr(s)+Br-(aq)----> CuBr2^-(aq)
Kc = [CuBr^2-]/[Br^-] [solid CuBr, [CuBr] = 1]
CuBr(s) ---------------> Cu^+ (aq) + Br^-
Ksp = [Cu^+][Br^-]
Cu^+ (aq) + 2Br^-(aq) ----------------------> CuBr2^-(aq)
Kf = [CuBr2^-]/[Cu^+][Br^-]^2
KsP*Kf = [Cu^+][Br^-]*[CuBr2^-]/[Cu^+][Br^-]^2
= [CuBr^2-]/[Br^-]
Ksp*Kf = Kc
Kc = Ksp*Kf
= 6.27*10^-9 * 8*10^5 = 0.005016 >>>>>>answer
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