The reaction by which it goes into solution is: Mg(OH)2(s) <-----> Mg2+(aq) + 2 OH−(aq) a. Formulate the expression for the equilibrium constant, Ksp, for the above reaction. b. It is possible to dissolve significant amounts of Mg(OH)2 in solutions in which the concentration of either Mg2+ or OH− is very, very small. Explain, using Ksp, why this is the case. c. Explain why Mg(OH)2 might have very appreciable solubility in 1 M HCl.
The reaction by which it goes into solution is: Mg(OH)2(s) <-----> Mg2+(aq) + 2 OH−(aq) a. Formulate the expression for the equilibrium constant, Ksp, for the above reaction. b. It is possible to dissolve significant amounts of Mg(OH)2 in solutions in which the concentration of either Mg2+ or OH− is very, very small. Explain, using Ksp, why this is the case. c. Explain why Mg(OH)2 might have very appreciable solubility in 1 M HCl.
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Magnesium hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is:
Mg(OH)2(s) <-----> Mg2+(aq) + 2 OH−(aq)
a. Formulate the expression for the equilibrium constant, Ksp, for the above reaction.
b. It is possible to dissolve significant amounts of Mg(OH)2 in solutions in which the concentration of either Mg2+ or OH− is very, very small. Explain, using Ksp, why this is the case.
c. Explain why Mg(OH)2 might have very appreciable solubility in 1 M HCl.
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