Question

Calculate the molar solubility of Mg(OH)2 in a solution that is basic with a pH of...

Calculate the molar solubility of Mg(OH)2 in a solution that is basic with a pH of 12.68.

Ksp = [Mg2+][OH]2 = 5.6 × 10–12

Homework Answers

Answer #1

pH = 12.68

pOH = 14 - 12.68 = 1.32

[OH-] = 10^-1.32

         = 0.04786 M

Mg(OH)2   ---------------> Mg+2 +   2 OH-

                                           S           0.0478

Ksp = [Mg+2][OH-]^2

5.6 x 10^-12 = S x (0.04786)^2

S = 2.44 x 10^-9 M

molar solubiity = 2.4 x 10^-9 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the molar solubility of Mg(OH)2, Ksp is 5.6 x 10-12 for Mg(OH)2, in the...
What is the molar solubility of Mg(OH)2, Ksp is 5.6 x 10-12 for Mg(OH)2, in the following aqueous solutions? A. Calculate the molar solubility in 0.24 M NaOH: B. Calculate the solubility in 0.24 M MgSO4?
calculate the molar solubility of Fe(OH)2 in a buffer solution with PH= 9.50? For Fe(OH)2, Ksp...
calculate the molar solubility of Fe(OH)2 in a buffer solution with PH= 9.50? For Fe(OH)2, Ksp = 4.9x10 -17
A)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2...
A)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2 in pure H2O ? 2.41×10−4 M B)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2 in 0.200 M NaOH ? Ksp , of 5.61×10−11 D) What is the pH change of a 0.300 M solution of citric acid (pKa=4.77 ) if citrate is added to a concentration of 0.140 M with no change in volume?
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 8.0 (b) pH 11.0 (c) pH 13.6 HopHelpCh17N6
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 7.4 ______________M (b) pH 10.8 ______________M (c) pH 13.3 ______________M
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 7.7 M (b) pH 11.0 M (c) pH 13.7 M
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 8.2 M (b) pH 10.8 M (c) pH 12.3 M
Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used...
Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.180 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH. What is the pH change of a 0.200 M...
Please answer both parts. Thanks! Part A) Mg(OH)2 is a sparingly soluble salt with a solubility...
Please answer both parts. Thanks! Part A) Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.180 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH. Part B)...
Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is...
Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.150 mol L−1 NaOH solution.