Using only K_sp from the equilibria of alkaline earth metal hydroxides table, ca

Question

Using only K_sp from the equilibria of alkaline earth metal hydroxides table, calculate how many moles of Mg(OH)_2 will dissolve in 100. mL of water. How will the solubility calculated in part (a) be affected by the K_1 reaction in this table? (Select all that apply.) The solubility of Mg(OH)_2 will be less than we would expect just on the basis of K_sp. The dissolution reaction will be drawn to the right. The solubility of Mg(OH)_2 will be greater than we would expect just on the basis of K_sp. The dissolution reaction will be drawn to the left.

Explanation / Answer

Ksp of Mg (OH)2=1.8 x 10-11

4S3 = 1.8 x 10^-11

S =3( 1.8 x 10^-11 /4) =0.00017 M

0.00017 moles/ L

so in 100 ml = 0.000017 moles= 1.7x10^-5 moles

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