Calculate Kb of Mg(OH)2 . It has a pH of 9.65 and the concentration is 0.10M
Mg(OH)2+ H2O----> Mg2++ 2OH-
Calculate Kb of Mg(OH)2 . It has a pH of 9.65 and the concentration is 0.10M...
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
In a saturated solution that is in contact with solid Mg(OH)2, the concentration of Mg2+ is 1.12×10–4 M. What is the solubility product for Mg(OH)2? Mg(OH)2(s)⇌Mg2+(aq)+2OH−(aq) Your answer should include three significant figures.
How should the solid compound Mg(OH)2 be represented in a net ionic equation? Mg(s) + (OH)2(s) Mg(OH)2(s) Mg2+(s) + (OH-)2(s) Mg2+(aq) + 2OH- (aq) Mg2+(s) + 2OH-(s)
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
If 0.10M solution of a weak base has a pH of 8.90, find the Kb for the base.
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate the equilibrium hydroxide ion concentration in a 0.95 M solution of the base. [OH-] = What are the pH and pOH of the solution?
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)
Determine Ka and Kb for 0.10M NH3 with a pH of 11.12.
. Given the reaction Mn2+ + 2OH- = Mn(OH)2 (s), calculate the pH required to decrease the manganese concentration (in the form of Mn2+) in a water supply to 0.03 mg/L. Note that the solubility product Ksp = 8×10-14.
If the concentration of Mg2+ ion in seawater is 1.21x103 mg/L, what OH- concentration is required to precipitate Mg(OH)2 ? Ksp(Mg(OH)2)=5.6x10-12 -OH concentration must be greater than _____ M.