The Ksp of Mg(OH)2 is 9.0 x 10‐12. If a solution is 0.045M with respect to...
The solubility product constant of Mg(OH)2 is 9.0 × 10-12. If a solution is 0.010 M with respect to Mg2+ ion, the amount of [OH-] required to start the precipitation of Mg(OH)2 is? : 3.0 × 10-5 M 3.0 × 10-7 M 1.5 × 10-5 M 9.0 × 10-10 1.5 × 10-7
What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.
Mg(OH)2 has a Ksp=5.61x10-12. Determine the pH of a saturated solution of Mg(OH)2. (Magnesium hydroxide is a solid.) (10 points)
Calculate the molar solubility of Mg(OH)2 in a solution that is basic with a pH of 12.62. Ksp = [Mg2+][OH–]2 = 5.6 × 10–12
Question 12 of 12 What is the solubility of Mg(OH)2 at a pH of 11.70? (Ksp Mg(OH)2 is 1.6 * 10-13) | 4 5 6 c X 100
What is Ksp for the following equilibrium if Mg(OH)2 has a molar solubility of 1.1×10−4 M? Mg(OH)2(s)↽−−⇀Mg2+(aq)+2OH−(aq)
7. If the initial pH of a solution is 12.00 and you add Mg(OH)2 to that solution, what is the molar solubility given that the Ksp for Mg(OH)2 is 5.6 x 10-12
An acidic solution is 0.01 M in Mg2+, Cu2+, and Fe2+. The pH of the solution is adjusted by adding NaOH. What is the maximum pH that removes only the Cu2+? Mg(OH)2(s) ↔ Mg2+(aq) + 2OH–(aq) Ksp = 6.3 x 10–10 Fe(OH)2(s) ↔ Fe2+(aq) + 2OH–(aq) Ksp = 4.1 x 10–15 Cu(OH)2(s) ↔ Cu2+(aq) + 2OH–(aq) Ksp = 2.2 x 10–20
Table 1. The results of adding solid Mg(OH)2 to 10.0L of water. Total amount of Mg(OH)2 added (g) Total amount of Mg(OH)2 added (mol) [Mg2+] in solution (M) [OH-] in solution (M) Mass of Mg(OH)2 that does NOT dissolve (g) 0.00963 1.65 x 10-4 1.65x 10-5 3.30 x 10-5 0 0.04815 8.26 x 10-4 8.26 x 10-5 1.65 x 10-4 0 0.09590 1.64 x 10-3 1.64 x 10-4 3.29 x 10-4 0 0.09630 1.65 x 10-3 1.65 x 10-4 3.30...
The Ksp of Ca(OH)2 is 6.5 x 10-6. Will a precipitate form if the pH of a 0.085 M CaCl2 solution is adjusted to 8.8?