Question: A hypothetical solid AB2 dissolves in water according to the following reaction. AB2(s) A+(aq) + 2B-(aq) If AB(s) and pure water reach equilibrium per the

A hypothetical solid "AB2" dissolves in water according to the following reaction.

AB2(s) A+(aq) + 2B-(aq)

If AB(s) and pure water reach equilibrium per the Ksp reaction, what will the ratio of ion concentrations [A+]/[B-] be?

If Ksp for AB2 is 4M^3 and the solubility reaction is AB2(s) A+(aq) + 2B-(aq), what is the solubility of AB2 in pure water in M units?

If Ksp for AB2 is 4M^3, what concentration of B-(aq) would you expect to find if the equilibrium process described by Ksp is reached by adding AB2 to pure water?

If the molar mass of AB2 is 100, what is the solubility of AB2 in pure water in grams per liter?

If 50g of AB2 is added to sufficient pure water to result in 1 liter of solution, what will the concentration of A+(aq) be in M units?

If 200g of AB2 is added to sufficient pure water to result in 1 liter of solution, what will the concentration of A+(aq) be in M units?

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