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?

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.