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QUESTION

# Quest (1) determine the ksp for magnesium hydroxide Mg(OH)2 where the molar solubility of Mg(OH)2 is 1.4X10^-4 M? quest (2) the Ksp for Zn(OH)2 is 5.0x10^-17 .determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5?

Question 1: K_(sp)= 1.1 xx10^(-11)

Question 2: s= 4.9 xx10^(-12)M

Quest (1) determine the for magnesium hydroxide Mg(OH)_2 where the molar solubility of Mg(OH)_2 is 1.4xx10^(-4) M?

We will use ICE table to solve this question.

The dissolution of Mg(OH)_2 can be written as follows:

" " " " " " " " " " " Mg(OH)_2(s) -> Mg^(2+)(aq) + 2OH^(-)(aq) " " " " " "  Initial:  " " " " " " " " " " " " 0 M " " " " " " 0M " " " " "  Change:  - sM " " " " " " " " " +sM " " " " " +2s M " " "  Equilibrium:  " " " " " " " " " " " " s M " " " " " " " " " 2s M

The expression of K_(sp) can be written as follows:

K_(sp) = [Mg^(2+)(aq)] *[OH^(-)(aq)]^2

 => K_(sp) = s*(2s)^2 = 4s^3= 4xx(1.4xx10^-4)^3

=> K_(sp)= 1.1 xx10^(-11)

Quest (2) The K_(sp) for Zn(OH)_2 is 5.0xx10^(-17) . Determine the molar solubility of Zn(OH)_2 in a buffer solution with a pH " of " 11.5?

We will use ICE table to solve this question.

pH = 11.5 => [H^+] = 10^(-11.5)

=> [OH^-] =10^(-2.5) = 3.2xx10^(-3) M

The dissolution of Zn(OH)_2 can be written as follows:

" " " " " " " " " " " Zn(OH)_2(s) -> Zn^(2+)(aq) + 2OH^(-)(aq) " " " " " "  Initial:  " " " " " " " " " " " " 0 M " " " " " 3.2xx10^(-3) M " " " " "  Change:  - sM " " " " " " "" +sM " " " " " +2s M " " "  Equilibrium:  " " " " " " " " " " " " s M " " " " " (3.2xx10^(-3) + 2s) M

The expression of K_(sp) can be written as follows:

K_(sp) = [Zn^(2+)(aq)] *[OH^(-)(aq)]^2

5.0xx10^(-17) =s *(3.2xx10^(-3) + 2s)^2

Solve for s=4.9xx10^(-12)M

Here is a video that explains the solving of Q2 (start at minute 5:14):