Free Printable Solubility

1.

Which compound is "insoluble" according to the solubility rules?

a)

Na₂SO₄

b)

NaCl

c)

Fe(NO₃)₂

d)

Ca₃(PO₄)₂

2.

Write an equilibrium expression for the dissolution of Ca₃(PO₄)₂

a)

K_sp = [Ca²⁺]³[PO₄^3-]²

b)

K_sp = [Ca²⁺]²[PO₄^3-]³

c)

K_sp = [Ca²⁺][PO₄^3-]

d)

$Ksp=\frac{[Ca^{2+}]^3[PO_4^{3-}]^2}{\left[Ca_3\left(PO_4\right)_2\right]}$

3.

The K_sp of Pb₃(AsO₄)₂ = 4.0 x 10^-36. What is the molar solubility of this compound?

a)

3.7 x 10^-38

b)

3.3 x 10^-8

c)

4.0 x 10^-36

d)

5.8 x 10^-8

4.

The solubility of cobalt(III) sulfide, (Co₂S₃) is 7.52 x 10^-26M. What is the K_sp?

a)

7.52 x 10^-26 M

b)

1.44 x 10^-125 M

c)

2.6 x 10^-124 M

d)

8.75 x 10^-8 M

5.

The K_sp of silver phosphate, Ag₃PO₄ is 2.6 x 10^-18. What is the molar solubility?

a)

9.53 x 10^-7 M

b)

3.05 x 10^-5 M

c)

1.76 x 10^-5 M

d)

4.58 x 10^-7 M

6.

The K_sp of magnesium carbonate, MgCO₃ is 3.5 x 10^-8. What is the molar solubility of this compound in a 0.237 L solution that already contains 0.173 mol of Mg²⁺?

a)

4.79 x 10^-8 M

b)

8.30 x 10^-9 M

c)

0.487 M

d)

1.48 x 10^-7 M

7.

What's the net ionic equation for the dissolution of Ca₃(PO₄)₂in water?

a)

$Ca_3\left(PO_4\right)_2\ \left(s\right)\ \leftrightarrow\ 3\ Ca^{2+}\ \left(aq\right)\ +\ 2\ PO_4^{3-}\ \left(aq\right)$

b)

$Ca_3\left(PO_4\right)_2\ \left(s\right)\ +\ 6H_2O\ \left(l\right)\ \leftrightarrow\ 3\ Ca\left(OH\right)_2\ \left(aq\right)\ +\ 2\ H_3PO_4^{ }\ \left(aq\right)$

c)

$Ca_3\left(PO_4\right)_2\ \left(s\right)\ \leftrightarrow\ 3\ Ca\ \left(s\right)\ +\ 2\ PO_4^{ }\ \left(l\right)$

d)

$Ca_3\left(PO_4\right)_2\ \left(s\right)\ +\ H_2O\ \left(l\right)\ \leftrightarrow\ 3\ Ca\ \left(aq\right)\ +\ 2\ PO_4\ \left(aq\right)$

8.

Landonium sorenside, L₂So is a sparingly soluble solid with K_sp = 6.9. You prepare a solution with [L⁺] = 3.0 M and [So^2-] = 1.0 M. Does a precipitate form? Why?

a)

No because Q > K_sp

b)

No because Q < K_sp

c)

Yes because Q > K_sp

d)

Yes because Q < K_sp

9.

An aqueous solution at room temperature is 0.5 M in both Pb²⁺ and Ca²⁺ ions. You want to separate these two ions by selective precipitation using chloride. What percentage of the first ion has been precipitated when the second ion begins precipitating? (PbCl₂; K_sp = 1.6 x 10^-5) and (CaCl₂; K_sp = 3.2 x 10^-11)

a)

100.%

b)

0.0002%

c)

99.96%

d)

0.04%

10.

Which compound has a higher molar solubility? PbCO₃ (K_sp = 7.4 x 10^-14) or BaCO₃ (K_sp = 2.0 x 10^-9).

a)

BaCO₃

b)

PbCO₃

c)

Can't say for sure

11.

Which compound has the highest molar solubility? AgCl (K_sp = 1.8 x 10^-10) or LaF₃ (K_sp = 2.0 x 10^-9) or CaF₂ (K_sp = 3.2 x 10^-11).

a)

AgCl

b)

LaF₃

c)

Can't say for sure

d)

CaF₂

12.

What is the pH of a saturated solution of Al(OH)₃ (K_sp = 1.8 x 10^-5)?

a)

0.09

b)

1.07

c)

12.93

d)

13.10

13.

What concentration of Cu²⁺ is necessary to precipitate Cu(OH)₂ (2.2 x 10^-20) in a solution with a pH of 8.5?

a)

3.92 x 10^-4M

b)

2.58 x 10^-5M

c)

6.96 x 10^-15M

d)

2.2 x 10^-9M

14.

A 300. mL solution of 0.013 M Pb(NO₃)₂ and 400. mL solution of 0.56 M NaCl are combined to form a precipitate. What is the equilibrium concentration of chloride ion after the precipitate forms? (PbCl₂; K_sp = 1.57 x 10^-5)

a)

0.096

b)

0.0054 M

c)

0.31 M

d)

0.54 M

Solubility

Total questions: 14

Worksheet time: 21mins

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