Consider the dissolution of ab(s): ab(s)⇌a+(aq)+b−(aq)le châtelier's principle tells us that an increase in either [a+] or [b−] will shift this equilibrium to the left, reducing the solubility of ab. in other words, ab is more soluble in pure water than in a solution that already contains a+ or b− ions. this is an example of the common-ion effect. the generic metal hydroxide m(oh)2 has ksp = 1.05×10−18. (note: in this particular problem, because of the magnitude of the ksp and the stoichiometry of the compound, the contribution of oh− from water can be ignored. however, this may not always be the case.)what is the solubility of m(oh)2 in pure water?