Question

What is the solubility of mg(oh)₂ at a ph of 12.70? (ksp mg(oh)₂ is 1.6 × 10⁻¹³)

Answer 1

Based on the calculations, the solubility of mg(oh)₂ at a pH of 12.70 is equal to 3.4 × 10⁻⁵ M.

Given the following data:

• Ksp of mg(oh)₂ = 1.6 × 10⁻¹³

• pH = 12.70

What is pH?

pH is an abbreviation for the power of hydrogen ions and it can be defined as a measure of the molar concentration of hydrogen ions that are present in a given solution. Thus, the power of hydrogen ions (pH) is generally used to identify or specify the acidity, neutrality, or basicity of any chemical solution.

First of al, we would write the properly balanced chemical equation for this chemical reaction:

                          $Mg(OH)_2(s)\rightleftharpoons Mg^{2+} (aq)+ 2OH^{-}(aq)$

Mathematically, the Ksp for the above chemical reaction is given by:

Ksp = [Mg²⁺][OH⁻]²

Ksp = [x][2x]²

1.6 × 10⁻¹³ = 4x³

x = ∛4 × 10⁻¹⁴

x = 3.4 × 10⁻⁵ M.

Read more on solubility here: brainly.com/question/3006391