What is the molar solubility of mg(oh)2 in a basic solution with a ph of 12.50? ksp for mg(oh)2 is 5.6 × 10-12. what is the molar solubility of mg(oh)2 in a basic solution with a ph of 12.50? ksp for mg(oh)2 is 5.6 × 10-12. 1.1 × 10-4 m 5.6 × 10-9 m 2.4 × 10-6 m 1.8 × 10-10 m

Explanation:

will form its respective ions in the solution as:

Consider the ICE take for as:

                                     Mg(OH)₂         ⇄        Mg²⁺ + 2OH⁻

At t =equilibrium                                              S            2S            

Where, S is the molar solubility

The expression for Solubility product of is:

Given that:

pH = 12.50

Also, pH + pOH = 14  

So, pOH = 14 - 12.50 = 1.5

So, Total [OH⁻ ] = S + 0.03162

So,

Since, S is very small, So, S + 0.03162 ≅ 0.03162

Thus,

The molar solubility of in a basic solution with a pH of 12.50 is:-

the objects have the same charge.