# Worksheet: Concentrations from Solubility Products

In this worksheet, we will practice using the solubility product of an ionic material to find the concentrations of dissolved ions.

Q1:

The dissolution of tribasic calcium phosphate is represented by the following equation. If this process changes by an amount , what is the change in ?

• A
• B
• C
• D
• E

Q2:

The dissolution of magnesium phosphate is represented by the following equation. If this process changes by an amount , what is the change in ?

• A
• B
• C
• D
• E

Q3:

The dissolution of magnesium hydroxide is represented by the following equation. If this process changes by an amount , what is the change in ?

• A
• B
• C
• D
• E

Q4:

The dissolution of calcium carbonate is represented by the following equation. If this process changes by an amount , what is the change in ?

• A
• B
• C
• D
• E

Q5:

The dissolution of silver(I) iodide is represented by the following equation. If this process changes by an amount , what is the change in ?

• A
• B
• C
• D
• E

Q6:

A 1.00 L solution is prepared by dissolving 1.00 g of and 10.0 g of in water. and ions react to form ions, with a stability constant of . Calculate the concentration of ions in the solution at equilibrium.

• A M
• B M
• C M
• D M
• E M

Q7:

In an aqueous ammonia solution, molecules react with ions to form ions. The stability constant of is . If the concentration of ions in a solution is initially 0.10 M, what is the concentration of ions at equilibrium?

• A M
• B M
• C M
• D M
• E M

Q8:

The first step in the preparation of magnesium metal is the precipitation of from sea water by the addition of . The concentration of in sea water is M and the solubility product of is . Calculate to 2 decimal places the pH at which the addition of causes to decrease to M.

Q9:

Clothing may be stained during washing if the water has a ion concentration of 0.1 mg/L ( M), but the amount of in the water can be reduced by adding a base. The base lowers the maximum value of [] by precipitating excess manganese ions as the hydroxide, . The solubility product of , , is . Calculate to 1 decimal place the pH required to prevent [] from exceeding M.

Q10:

The solubility product of at is . If a solution contains 0.0020 mol of per liter, what concentration of ion must be reached by adding solid before begins to precipitate? Neglect any increase in volume upon adding the solid silver nitrate.

• A M
• B M
• C M
• D M
• E M

Q11:

A solution contains and ions at equal concentrations of 0.050 M. Silver(I) nitrate is added to the solution until precipitation takes place. The solubility product is for and for .

At what value of does precipitation begin?

• A M
• B M
• C M
• D M
• E M

To 3 significant figures, what molar percentage of the initial precipitate is ?

• A
• B
• C
• D
• E

Q12:

A solution contains 0.0010 mol is and 0.10 mol for . is gradually added to this solution. Which forms first, solid or solid ? is for , and for .

• AOnly solid precipitates.
• BSolid
• DSolid and solid precipitate at the same value of
• ESolid

Q13:

Blood will not clot if calcium ions are removed from its plasma. Some blood collection tubes contain salts of the oxalate ion, , for this purpose. At sufficiently high concentrations, the calcium and oxalate ions form solid . The concentration of in a sample of blood serum is M. What concentration of ions must be established before begins to precipitate? Consider

• A M
• B M
• C M
• D M
• E M

Q14:

Consider the following equilibrium.

A suspension contains solid in equilibrium with a saturated solution of and ions. The concentration of ions in the solution is M. What is the solubility product of ?

• A
• B
• C
• D
• E

Q15:

Fluorite, , is a slightly soluble solid that dissolves according to the following equation. The concentration of in a saturated solution of is M. What is the solubility product of fluorite?

• A
• B
• C
• D
• E

Q16:

The iodate ion concentration of a saturated solution of was found to be mol/L. What is the of ?

• A
• B
• C
• D
• E

Q17:

The of copper(II) iodate () is . Calculate the concentration of iodate ions in a saturated solution of copper(II) iodate.

• A M
• B M
• C M
• D M
• E M

Q18:

The acid dissociation constant, , of is and the solubility product, , of is . To 2 significant figures, what mass of must be added to 1.00 L of 0.010 M to initiate the precipitation of ?

• A g
• B g
• C g
• D g
• E g

Q19:

Which of the following compounds, when dissolved in a 0.01 M solution of , has a solubility greater than in pure water?

• A
• B
• C
• D
• E

Q20:

If solid was added to 0.01 M aqueous solutions of the following compounds, which of them will decrease the solubility of ions?

• A
• B
• C
• D
• E

Q21:

In a solution buffered at a pH of 11.45 in contact with solid , what is at equilibrium? The of is and the self-ionization constant of water, , is .

• A M
• B M
• C M
• D M
• E M

Q22:

An unbuffered solution initially at a pH of 12.700 is brought into contact with solid . What is at equilibrium? The of is .

• A M
• B M
• C M
• D M
• E M