Answer:
Ksp = 8.99x10⁻¹²
Explanation:
The solubility of Mg(OH)₂ is described with the reaction:
Mg(OH)₂(s) → Mg²⁺(aq) + 2OH⁻(aq)
The solubility product, Ksp, is:
Ksp = [Mg²⁺] [OH⁻]²
As you can see from the reaction, when 1 mole of Mg²⁺ is produced, 2 moles of OH⁻ are produced too, if [Mg²⁺] is 1.31x10⁻⁴M, [OH⁻] = 2.62x10⁻⁴M
Replacing:
Ksp = [Mg²⁺] [OH⁻]²
Ksp = [1.31x10⁻⁴M] [2.62x10⁻⁴M]²
The solubility product of the [tex]\rm Mg(OH)_2[/tex] has been [tex]\rm 8.99\;\times\;10^{-12}[/tex].
The balanced equation for the dissociation of Magnesium hydroxide has been:
[tex]\rm Mg(OH)_2\;\rightarrow\;Mg^2^+\;+\;2\;OH^-[/tex]
From the balanced chemical equation, dissociation of 1 mole magnesium hydroxide has been resulted in the 1 mole magnesium and 2 mole hydroxide ions.
Since, given magnesium concentration, [tex]\rm Mg^2^+=1.31\;\times\;10^-^4\;M[/tex]
The concentration of hydroxide ion, [tex]\rm OH^-[/tex] will be:
[tex]\rm 1\;M\;Mg^2^+=2\;M\;OH^-\\1.31\;\times\;10^-^4\;M=1.31\;\times\;10^-^4\;\times\;2\;M\;OH^-\\1.31\;\times\;10^-^4\;M=2.62\;\times\;2\;M\;OH^-\\[/tex]
The solubility product (ksp) of the reaction has been given as:
[tex]ksp=\rm [Mg^2^+]\;[OH^-]^2[/tex]
Substituting the values for ksp:
[tex]ksp\;=\rm [1.31\;\times\;10^-^4]\;[2.62\;\times\;10^-^4]^2\\\textit ksp=8.99\;\times\;10^-^1^2[/tex]
The solubility product of the reaction has been [tex]\rm 8.99\;\times\;10^{-12}[/tex].
For more information about solubility product, refer to the link:
https://brainly.com/question/1163248
