Answer:
[tex]Ksp=2.00x10^{-8}[/tex]
Explanation:
Hello!
In this case, since the pH of the given metal is 10.15, we can compute the pOH as shown below:
[tex]pOH=14-pH=14-10.15=3.85[/tex]
Now, we compute the concentration of hydroxyl ions in solution:
[tex][OH^-]=10^{-pOH}=10^{-3.95}=1.41x10^{-4}M[/tex]
Now, since this hydroxide has the form MOH, we infer the concentration of OH- equals the concentration of M^+ at equilibrium, assuming the following ionization reaction:
[tex]MOH(s)\rightarrow M^+(aq)+OH^-(aq)[/tex]
Whose equilibrium expression is:
[tex]Ksp=[M^+][OH^-][/tex]
Therefore, the Ksp for the saturated solution turns out:
[tex]Ksp=1.41x10^{-4}*1.41x10^{-4}\\\\Ksp=2.00x10^{-8}[/tex]
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