Multiple Choice Questions
Solubility:

   
 1 Silver chloride is difficultly soluble. Calculate the equilibrium concentration of silver ion ([Ag+1]) in a saturated silver chloride solution.
Ksp AgCl = 1.6x10-10

2.2x10-3 M
5.2x10-4 M
6.7x10-6 M
1.8x10-10 M
1.3x10-5 M

 2 Calculate the molar solubility of silver chloride in a 0.20 M sodium chloride solution.
Ksp AgCl = 1.6x10-10

3.0x10-5 M
6.0x10-6 M
3.6x10-11 M
9.0x10-10 M
1.3x10-5 M

 3 Silver carbonate would be most soluble in a solution of:

Na2CO3
HNO3
AgNO3
AgCl 
K2CO3

 4 A solution contains 0.15 M Cl- and 0.15 M CO3-2. Silver ion is slowly added. Assuming no dilution of the solution, which of the following statements is true:
Ksp AgCl = 1.6x10-10;    Ksp Ag2CO3 = 8.2x10-12

AgCl precipitate first at a silver ion concentration of 1.2x10-9 M. 
AgCl precipitate first at a silver ion concentration of 3.5x10-5 M. 
Ag2CO3 precipitate first at a silver ion concentration of 3.7x10-6 M. 
Ag2CO3 precipitates first at a silver ion concentration of 5.4x10-11 M. 
No precipitate forms.

 5 5.0 mL of 0.022 M lead nitrate solution is combined with 5.0 mL of 0.022 M sodium chloride solution. Which of the following statements is TRUE:
Ksp PbCl2 = 1.6x10-5

NaNO3 precipitates. 
PbCl2 precipitates. 
NaCl precipitates. 
Pb(NO3)2 precipitates. 
No precipitate forms.

 6  The molar solubility of barium sulfate is 1.05x10-5 M in pure water. The Ksp for BaSO4 is:

1.1x10-10
4.4x10-10
1.05x10-5
3.2x10-3
5.0x10-9

 7 The molar solubility of silver chloride in water is 1.3x10-5 M. The solubility product constant (Ksp) for AgCl is _____.

3.6x10-3
1.3x10-5
4.2x10-7
1.7x10-10
3.4x10-10

 8 The molar solubility of barium sulfate in 0.10 M sodium sulfate is _____ M.
Ksp BaSO4 = 1.1 x 10-10

0.10 
1.0 x 10-5
5.5 x 10-11
1.1 x 10-11
1.1 x 10-9

 9 The solubility of calcium sulfate in water is 4.9x10-3 M at a given temperature. Calculate the value of Ksp for calcium sulfate at this temperature.

2.4x10-5
9.8x10-3
4.9x10-3
4.8x10-5
2.4x10-3

 10 Ksp for Ag2CO3 is 8.2x10-12 at 25° C. What is the solubility in moles/liter of silver carbonate in water at this temperature?

2.9x10-6
1.3x10-4
2.0x10-4
5.0x10-5
8.2x10-12

 11  A sample of 20.0 ml of 0.10 M Ba(NO3)2 is added to 20.0 ml of 0.10 M Na2CO3. Will BaCO3 precipitate? 
Ksp for BaCO3 is 5.1x10-9

yesnomaybe

 12 Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+. Which compound will begin to precipitate first? What concentration of I- is needed to initiate this precipitation? 
Ksp (CuI) = 5.1x10-12; Ksp (AgI) = 8.3x10-17

AgI; 8.3x10-17
CuI; 5.1x10-12
CuI; 5.1x10-10
AgI; 8.3x10-15
AgI; 9.1x10-9

 13 What is the [Sr2+] in a saturated solution of SrCrO4 (s) in pure water.
Ksp for SrCrO4 is 3.6x10-5

2.2x10-4
1.0x10-5
2.0x10-5
2.0x10-6
4.0x10-9

 14 What is the solubility of CaF2 in mol/L in 0.10M Ca(NO3)2
Ksp for CaF2 = 4.0x10-11.

2.2x10-4
1.0x10-5
2.0x10-5
2.0x10-6
4.0x10-9

 15 If solid NaCl is added to an aqueous solution which is 0.020 M in BOTH Pb(NO3)2 and AgNO3 until the [Cl-] is 0.020 M, what will happen? Assume no volume change. 
Ksp for PbCl2 is 1.6x10-5 and Ksp for AgCl is 1.6x10-10.

A precipitate of PbCl2 but not of AgCl will form. 
A precipitate of AgCl but not of PbCl2 will form. 
Precipitates of both AgCl and PbCl2 will form. 
No precipitate will form.
A precipitate of NaNO3 will form.

 16 The molar solubility of barium sulfate in 0.50 M sodium sulfate is _____ M. 
Ksp (BaSO4) = 1.1 x 10-10

5.5x10-11
4.4x10-10
1.1x10-10
1.8x10-9
2.2x10-10

 17 Solid sodium chloride is added to a solution containing 0.62 M Pb(NO3)2 and 0.54 M AgNO3. Which solid precipitates first?
Ksp  PbCl2 = 1.6x10-5 ;     Ksp for AgCl is 1.6x10-10.
 

NaNO3
AgCl 
PbCl2
AgNO3
no precipitate forms 

 18 If the concentration of chloride ion in the solution in problem 17 is 0.011 M, the concentration of Ag+ is _____ M.

54 
0.0 
1.76x10-12
2.0x10-6
1.45x10-8

 19 Calculate the molar solubility of silver chloride in 0.15 M sodium chloride. 
Ksp of silver chloride = 1.6x10-10.

1.6x10-10
1.3x10-5
1.1x10-9
1.3x10-10
1.6x10-4

 20 Calcium ion is slowly added to a solution which is 0.10 M in F- and 1.0x10-3 M in CO3-2. What precipitate will form first and at what concentration of calcium ion? 
Ksp of CaF2 = 2.7x10-11 and the Ksp of CaCO3 is 2.8x10-9.

CaCO3   2.8x 10-6
CaF2   2.8x 10-6
CaCO3   2.7x 10-9
CaF2   2.7x10-10
no precipitate will form 

 21 Calculate the Molar solubility of PbCl2 in 0.30 M NaCl aqueous solution. 
(Ksp of PbCl2=1.6x10-5)

1.6x10-2
5.3x10-5
1.8x10-4
4.4x10-5
4.0x10-3

 22 An aqueous solution is 0.10 M in CrO42-. If Ag+ ions are added slowly (assuming no dilution of the solution) what will be the equilibrium concentration of Ag+ when Ag2CrO4 first begins to precipitate? 
Ksp of Ag2CrO4 = 2.4x10-12

8.4x10-5 
4.9x10-6
2.5x10-6
2.4x10-11
2.4x10-12

 23 Calculate the molar solubility of BaF2 in a 0.20 M aqueous solution of KF. 
(Ksp of BaF2 = 1.7x10-6)

1.6x10-2
8.5x10-6
4.2x10-5
1.1x10-5
1.7x10-6

 24 Hydrogen Sulfide (H2S) is added to a 0.10 M aqueous solution of Cu2+ until the equilibrium concentration of S2- becomes 4.0x10-23 M. Determine the molar concentration of Cu2+
(Ksp of CuS = 6.3x10-36)

1.6x10-13
4.0x10-23
2.5x10-18
6.3x10-35
0.10