The solubility product constant (Ksp) for the dissolution of Cu(OH)2 as represen

Question

The solubility product constant (Ksp) for the dissolution of Cu(OH)2 as represented by the chemical equation is 2.6 x 10-19. Cu(OH)2 (s) Cu2+ (aq) + 2 OH- (aq) Calculate the molarity (M) of Cu2+ in a saturated solution of Cu(OH)2. Molar Mass (g/mol) Cu(OH)2 97.55

Explanation / Answer

Cu(OH)2 (s) -----> Cu2+ (aq) + 2 OH- (aq) Ksp=[Cu2+][OH-]2 2*[Cu2+]=[OH-] (From the equation) Replacing this in Ksp Ksp=[Cu2+]*{[Cu2+]*2}^2=4*[Cu2+]^3 2.6*10^-19 = 4* [Cu2+]^3 [Cu2+]=4.02*10^-7 M Molarity (M) of Cu2+ in a saturated solution of Cu(OH)2= (4.02*10^-7) M

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