The ksp of magnesium hydroxide, mg(oh)2, is 1.2 x 10-11, so setting 4s3 = ksp, results in s = 1.4 x 10-4. this leads to an [oh-] = 2.8 x 10-4 (i. e., a poh=3.55), thus a ph of 10.45. given the aforementioned information and resulting calculations, comment on the solubility of mg(oh)2 at ph values: 1) less than 10.45 and, 2) greater than 10.45

1) less than 10.45 : Increase the solubility

2) greater than 10.45: decrease the solubility

Explanation:

The dissolution equation for magnesium hydroxide is:

Thus there is formation of hydroxide ion during dissollution of magnesium hydroxide.

If the pH value increases from 10.45 to higher value, it means we are decreasing the concentration of [H⁺] or increasing the concentration of [OH⁻]

Increasing the concentration of [OH⁻] will shift the equilibrium towards reactant side. Thus it will decrease the solubility of magnesium hydroxide.

If the pH value decreases from 10.45 to lower value, it means we are increasing the concentration of [H⁺] or decreasing the concentration of [OH⁻]

decreasing the concentration of [OH⁻] will shift the equilibrium towards product side. Thus it will increase the solubility of magnesium hydroxide.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

it is a solid

explanation: