Q: If the molar solubility of $$BaSO_4 is$$ $$1.1 \times 10$$^{-5}$$ M, what is the K$$_{sp}$$ for $$BaSO_4$$?

$$K_{sp} = (1.1 \times 10$$^{-5}$$)^2$

Question 1

Which of the following correctly describes the process shown in the diagram for determining the solubility product constant ($$K_{sp}) of a $$compound?

Accepted Answer

Calculate the molar solubility (mol/L) from the solubility (g/L), then determine the molar concentration of ions at equilibrium, and finally compute $$K_{sp} as $$the product of ion concentrations.

Question 2

If the solubility of a compound is given in grams per liter (g/L), what is the first step in calculating its $$K_{sp}$$?

Accepted Answer

Divide the solubility by the molar mass to obtain molar solubility (mol/L).

Question 3

After determining the molar solubility of a compound, what must be done before calculating $$K_{sp}$$?

Accepted Answer

Calculate the equilibrium concentrations of each ion based on the stoichiometry of the dissolution reaction.

Question 4

Which equation represents the solubility product constant ($$K_{sp}) $$for a salt $$MX_2$$ that dissociates as $$MX_2(s$$) \rightleftharpoons $$M^{2+}(aq) + 2X^-(aq$$)$$?

Accepted Answer

$$K_{sp} = [M$$^{2+}$$][X^-]^2$$

Question 5

A student finds the solubility of $$Ag_2CrO_4 to be$$ $$6.7 	imes 10$$^{-5}$$ M. What is the correct expression for K$$_{sp}$$ for Ag_2$$CrO_4$$?

Accepted Answer

$$K_{sp} = [Ag^+]^2 [$$CrO_4$$^{2-}]$$

Question 6

If the molar solubility of $$BaSO_4 is$$ $$1.1 	imes 10$$^{-5}$$ M, what is the K$$_{sp}$$ for $$BaSO_4$$?

Accepted Answer

$$K_{sp} = (1.1 	imes 10$$^{-5}$$)^2$

Question 7

Which step is necessary to convert the solubility of a compound (g/L) to its $$K_{sp}$$?

Accepted Answer

Convert grams per liter to moles per liter using the molar mass.

Question 8

Why is the concentration of a pure solid not included in the $$K_{sp}$$ expression?

Accepted Answer

Because its concentration is constant and does not affect the equilibrium.

Question 9

A compound has a solubility of 0.5 g/L and a molar mass of 100 g/mol. What is its molar solubility?

Accepted Answer

$$0.005$$ mol/L$

Question 10

In the process shown in the diagram, what is the final step before calculating $$K_{sp}$$?

Accepted Answer

Determine the molar concentration of ions at equilibrium.

Solubility Product Principle and Applications

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