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Homework answers / question archive / Consider an amphoteric hydroxide, M(OH)2(s)
Consider an amphoteric hydroxide, M(OH)2(s). where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0. Copper(l) ions in aqueous solution react with NH3(ag) according to Calculate the solubility (in g- L-1) of CuBr(s) (Kgp = 6.3 times 10-9) in 0.88 M NH3(aq). The formation constant of [M(CN)2] is 5.30 times 1018, where M is a generic metal. A 0.160-mole quantity of M(NC>3) is added to a liter of 0.710 M NaCN solution. What is the concentration of M + ions at equilibrium?
assuming M to be Mg
I will do the solubility for Mg(OH)2 where the pH is l0, and perhaps you can do the others the same way.
Ksp =2 x l0^-16th = (Mg++)(OH)^2 Mg(OH)2(s) at equilib Mg++(aq) + 2 OH-(aq)
If the pH is l0 then the pOH is 4 because pH + pOH = 14
and if the pOH is 4, then the (OH-) concentration = antilog(-pOH)
antilog (-4) = l x l0^-4
Ksp 2 x l0^-16 = (Mg++)(l x l0^-4)^2
(Mg++) = 2 x l0^-16 over 1 x l0^-8 = 2 x l0^-8 Moles per liter solubility
Mg(OH)2 when pH is l0
