Solubility Quiz #2 Ionic Concentrations Calculations & Ionic Equations

1. A 200.0 mL solution contains 0.050 mol of Ba(NO3)2. The [NO3-] is

A. 0.050 MB. 0.10 MC. 0.25 MD. 0.50 M

2. The Ksp expression for a saturated solution of Ca3(PO4)2 is

A. Ksp = [Ca2+][PO43-]

B. Ksp = [Ca2+][PO43-]2

C. Ksp = [3Ca2+][2PO43-]

D. Ksp = [3Ca2+]3[2PO43-]2

3. In 1.5 M (NH4)2SO4 , the ion concentrations are

A. [NH4+] = 1.5 M and [SO4

2-] = 1.5 MB. [NH4

+] = 1.5 M and [SO42-] = 3.0 M

C. [NH4+] = 3.0 M and [SO4

2-] = 1.5 MD. [NH4

+] = 3.0 M and [SO42-] = 3.0 M

4. The Ksp expression for Ca3(PO4)2 is

A. Ksp = [Ca 2+ ] 3 [PO 43- ] 2

[Ca3(PO4)2]

B. Ksp = [2Ca 2+ ][3PO 43- ]

[Ca3(PO4)2]

C. Ksp = [Ca2+]3[PO43-]2

D. Ksp = [2Ca2+][3PO4

3-]

5. The solubility product expression for a saturated solution of Fe2(SO4)3 is

A. Ksp = [Fe3+]2[SO42-]3

B. Ksp = [2Fe3+][3SO42-]

C. Ksp = [Fe 3+ ] 2 [SO 42- ] 3

[Fe2(SO4)3]

D. Ksp = [2Fe 3+ ][3SO 42- ]

[Fe2(SO4)3]

6. Molecular solutions do not conduct electricity because they contain

A. molecules onlyB. cations and anionsC. molecules and anionsD. molecules and cations

7. If equal volumes of 0.2 M KBr and 0.2M FeSO4 are mixed, then

A. no precipitate will be observedB. a precipitate of FeBr2 will be observedC. a precipitate of K2SO4 will be observedD. a precipitate of both K2SO4 and FeBr2 will be observed

8. Which of the following occurs when equal volumes of 0.20 M MgS and 0.20 M ZnSO4

are mixed?

A. A precipitate does not formB. A precipitate of ZnS formsC. A precipitate of MgSO4 formsD. Precipitates of MgSO4 and ZnS form

9. In an experiment, 0.500 mol of Fe(NO3)3 is dissolved in water to produce a 2.00 L solution. The [NO3

-] in this solution is

A. 0.250 MB. 0.500 MC. 0.750 MD. 1.50 M

10. The complete ionic equation for the reaction between MgCl2(aq) and AgNO3(Aq) is

A. Ag+(aq) + Cl-

(aq) → AgCl(s)

B. 2AgNO3(aq) + MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)

C. 2Ag+(aq) + Mg2+

(aq) + 2NO3- (aq) + 2Cl-

(aq) → MgCl2(s) + 2Ag+(aq) + 2NO3

- (aq)

D. 2Ag+(aq) + 2NO3

- (aq) + Mg2+

(aq) + 2Cl-(aq) → 2AgCl(s) + Mg2+

(aq)+ 2NO3- (aq)

11. Which one of the following would form an ionic solution when dissolved in water?

A. I2

B. CH3OHC. Ca(NO3)2

D. Cl2H22O11

12. If the solubility of Pb (OH) 2 is 0.155g/L, then the concentration of each ion in a saturated solution of a Pb (OH) 2 is

A. [Pb2+] = 0.155 g/L and [OH-] = 0.155g/LB. [Pb2+] = 0.052 g/L and [OH-] = 0.103g/LC. [Pb2+] = 6.43 x 10-4 g/L and [OH-] = 1.29 x 10-3g/LD. [Pb2+] = 6.43 x 10-4 g/L and [OH-] = 6.43 x 10-4 g/L

13. The Ksp expression for calcium hydroxide is

A. Ksp = [Ca2+][OH-]2

B. Ksp = 1 . [Ca2+][OH-]2

C. Ksp = [Ca2+][2OH-]2

D. Ksp = 1 .[Ca2+][2OH-]2

14. A precipitation reaction occurs when equal volumes of 0.2 M Pb(NO3)2 and 0.2 M KI are mixed. The net ionic equation for this reaction is

A. Pb2+(aq) + 2I-

(aq) → PbI2(s)

B. PbI2(s) → Pb2+(aq) + 2I-

(aq)

C. K+(aq) + NO3

-(aq) → KNO3(s)

D. KNO3(s) → K+(aq) + NO3

-(aq)

15. When dissolved in water, which of the following procedures is an ionic solution?

A. O2

B. CH4

C. CaCL2

D. C12H22O11

16. In a 200 mL sample of 0.030 M Na3PO4, the [NA+] is

A. 0.006 MB. 0.010 MC. 0.018 MD. 0.090 M

Solubility Quiz #3 Solubility to Ksp

1. In a saturated solution of manganese (II) hydroxide, Mn(OH)2, and [Mn2+] equals 4.5 x 10-5 M. therefore, the Ksp of Mn(OH)2 is

A. 9.1 x 10-14

B. 3.6 x 10-13

C. 2.0 x 10-9

D. 4.1 x 10-9

2. The solubility of manganese (II) sulphide is 1.7 x 10-7 M at 25oC. The solubility product constant is

A. 2.9 x 10-14

B. 1.7 x 10-7

C. 3.4 x 10-7

D. 4.1 x 10-4

3. The compound Ag2S has a solubility of 1.3 x 10-4 moles per litre at 25oC. The Ksp for this compound is

A. 2.2 x 10-12

B. 8.8 x 10-12

C. 1.7 x 10-8

D. 3.4 x 10-8

4. The solubility of barium oxulate, BaC2O4, is 4.8 x 10-4 M. The value of Ksp is

A. 2.3 x 10-7

B. 4.8 x 10-4

C. 2.4 x 10-4

D. 2.2 x 10-2

5. The solubility of MnS is 4.8 x 10-7 M , at 25oC. The Ksp value is

A. 2.3 x 10-13

B. 4.8 x 10-7

C. 9.6 x 10-7

D. 6.9 x 10-4

6. At 25oC, the solubility of an unknown compound is 7.1 x 10-5 M. the compound is

A. CuIB. AgIC. CaCO3

D. CaSO4

7. The solubility of barium fluoride is 3.6 x 10-3 M. the solubility product constant is

A. 4.7 x 10-8

B. 1.9 x 10-7

C. 1.3 x 10-5

D. 2.6 x 10-5

8. At a certain temperature, the solubility of BaF2 is 7.4 x 10-3 moles per litre. The Ksp of BaF2 is

A. 1.6 x 10-6

B. 5.5 x 10-5

C. 1.1 x 10-4

D. 7.4 x 10-3

Solubility Quiz #4 Ksp to Solubility and Size of Ksp

1. Identify the most soluble sulphide

A. HgS, Ksp = 1.6 x 10-54 B. PbS, Ksp = 7.0 x 10-29 C. FeS, Ksp = 3.7 x 10-19 D. MnS, Ksp = 2.3 x 10-13

2. Saturated solutions of Na2S, CuS, SnS2, and Al2S3 are prepared at 25oC. The [S2-] will be greatest in the solution of

A. Na2SB. CuSC. SnS2

D. Al2S3

3. A solution of AgNO3 is slowly added to a mixture containing 0.10 M I-, Cl-, Br-, and IO3

-. The precipitate, which forms first, is

A. AgIB. AgClC. AgBrD. AgIO3

4. The [OH-] is measured to be 3.3 x 10-3 mol/L in a 100 mL sample of saturated solution of Al(OH)3. The solubility of Al(OH)3 is

A. 1.1 x 10-4 mol/LB. 3.3 x 10-4 mol/LC. 1.1 x 10-3 mol/LD. 3.3 x 10-3 mol/L

5. The [SO24-] in a saturated solution of PbSO4 is (Ksp = 1.1 x 10-8)

A. 1.2 x 10-16 MB. 5.5 x 10-9 MC. 1.1 x 10-8 MD. 1.0 x 10-4 M

6. The least soluble in salt water is

A. BaSB. AlCl3

C. CaSO3

D. ZnSO4

7. The solubility of AgBrO3 is

A. 2.8 x 10-9 MB. 5.3 x 10-5 MC. 1.1 x 10-4 MD. 7.3 x 10-3 M

8. At 25oC, the solubility of Mg (OH)2 is

A. 1.1 x 10-32 MB. 5.6 x 10-12 MC. 2.4 x 10-6 MD. 1.1 x 10-4 M

9. A student evaporated 200.0 mL of a saturated solution of SrCrO4 to dryness. The residue contained 1.2 x 10-3 mol SrCrO4. The solubility of SrCrO4 is

A. 1.4 x 10-6 MB. 3.6 x 10-5 MC. 2.4 x 10-4 MD. 6.0 x 10-3 M

10. The solubility of magnesium carbonate is

A. 9.3 x 10-5 MB. 3.4 x 10-6 MC. 6.8 x 10-6 MD. 6.0 x 10-3 M

11. A saturated container of NiCO3 was evaporated to dryness. A 250.0 mL sample was found to contain 1.1 x 10-2 g NiCO3. The molecular mass of NiCO3 is 118.7 g/mol. The molar solubility of NiCO3 is

A. 9.3 x 10-5 MB. 3.7 x 10-4 MC. 4.4 x 10-2 MD. 1.4 x 10-7 M

12. Which of the following is the least soluble in water at 25oC ?

A. CaSO3

B. BaSO4

C. CuSO4

D. MgSO4

13. Which of the following salts has the lowest solubility?A. copper(I) chlorideB. ammonium sulphideC. potassium hydroxideD. mercury(II) sulphate

Solubility Quiz #5 Trial Ksp

1. In an experiment, a student mixes equal volumes of 0.0020 M Pb2+ ions with 0.0040 M I- ions. The trial ion product is

A. 4.0 x 10-9 B. 3.2 x 10-8 C. 1.3 x 10-7 D. 8.0 x 10-6

2. In an experiment, 20.0 ml of 0.0060 M CaCL2 and 20.0 mL of 0.0050 M NaSO4 are mixed together. The trial ion product (trial Ksp) is

A. 7.5 x 10-6 and a precipitate will form B. 7.5 x 10-6 and a precipitate will not form C. 3.0 x 10-5 and a precipitate will form D. 3.0 x 10-5 and a precipitate will not form

3. In a saturated solution of Zn(OH)2, the [Zn2+] is

A. less than 0.10 MB. more than 10.0 MC. more than 0.10 M but less than 1.0 MD. more than 1.0M but less than 10.0 M

4. When 0.20 M Al2(SO4)3 is added to an equal volume of 0.20 M CaCl2,

A. AlCl3 precipitatesB. CaSO4 precipitatesC. AlCl3 and CaSO4 precipitateD. no precipitate forms

5. When a student mixes equal volumes of 0.20 M Na2S and 0.02 M Sr(OH)2.

A. no precipitate formsB. a precipitate of only SrS formsC. a precipitate of only NaOH formsD. precipitates of both NaOH and SrS form

6. When solutions of Pb(NO3)2 and NaCl are mixed, the trial ion product (Trial Ksp) is 9.8 x 10-6. Which of the following statements is true?

A. A precipitate forms because Ksp > 9.8 x 10-6

B. A precipitate forms because Ksp < 9.8 x 10-6

C. A precipitate does not form because Ksp < 9.8 x 10-6 D. A precipitate does not form because Ksp > 9.8 x 10-6

7. When equal volumes of 0.060 M AgNO3 and 0.00090 M NaBrO3 are mixed, the trial ion product (TIP) is

A. less than Ksp and a precipitate formsB. greater than Ksp and a precipitate formsC. less than Ksp and no precipitate formsD. greater than Ksp and no precipitate forms

8. The mixture that could produce a precipitate of two compu\ounds is

A. 0.2 M HgSO4 and 0.2 M FeCl2

B. 0.2 M AgNO3 and 0.2 MgCl2

C. 0.2 M K2CO3 and 0.2 CuSO4

D. 0.2 M ZnSO4 and 0.2 Ba(OH)2

9. Which of the following has a solubility of less than 0.10 M?

A. SrSB. SrCl2

C. SrsO4

D. Sr(OH)2

10. When equal volumes of 2.0 M Pb(NO3)2 and 2.0 M KCl are mixed

A. a precipitate forms because trial ion product < Ksp B. a precipitate forms because trial ion product > Ksp

C. a precipitate does not form because trial ion product < Ksp D. a precipitate does not form because trial ion product > Ksp

Solubility Quiz #6 Separating Ions

1. During a lab on qualitative analysis, an unknown solution containing one cation was analyzed and the following data were collected:

0.2 M Anions Added to the Unknown Solution

Observation

S2- no precipitateSO2-

4 precipitateOH- precipitate

CO2-3 precipitate

Which one of the following cations is found in the unknown solution?

A. Mg2+

B. Ca2+

C. Sr2+

D. Ba2+

2. Which of the following could be used to precipitate both Mg2+ and Ca2+ from hard water?

A. Lithium sulphateB. Sodium phosphateC. Potassium sulphideD. Ammonium chloride

3. A reagent that may be used to separate Cl- from S2- by precipitation is

A. KNO3

B. AgNO3

C. Pb(NO3)2

D. Al(NO3)3

4. The precipitate formed when equal volumes of 0.2 M Sr(OH)2 and 0.2 M MgS are mixed is

A. SrsB. Mg(OH)2

C. a mixture of Mg(OH)3 and SrSD. a mixture of Sr(OH)2 and MgS

5. Which of the following ions could be used to separate Cl-(aq) from SO4

2-(aq) by

precipitation?

A. Ag+

B. Ca2+

C. NH4+

D. Pb2+

6. Which of the following ions could be added to an aqueous mixture containing Pb2+ and Ba2+ to separate the ions by precipitating one of them?

A. I-

B. NO3-

C. PO43-

D. SO42-

7. Which of the following would precipitate the CA2+ and Mh2+ found in hard water?

A. S2-

B. PO3-4

C. SO2-4

D. CH3COO-

8. A solution containing an unknown cation was added to three solutions and the following observations were recorded:

SOLUTION OBSERVATIONNaI no precipitate

Na2SO4 precipitateNaOH no precipitate

The unknown cation is

A. Pb2+

B. Sr2+

C. Ca2+

D. Ag+

9. To remove Mg2+ from a solution by precipitation, a student should add

A. NaIB. KOHC. Li2SO4

D. (NH4)2S

10. Which of the following could be used to separate Pb2+ from Ba2+ by precipitation?

A. Na2SB. NaOHC. Na2CO3

D. Na2CO4

11. A student wishes to identify an unknown cation in a solution. A precipitate does not form with the addition of SO4

2-, but does form with the addition of S2-. Which of the following is the unknown cation?

A. Ag+

B. Mg2+

C. Ca2+

D. Cu2+

12. A solution contains CO32- and OH-. Separation of these two anions by selective

precipitation is accomplished by first adding Sr(NO3)2 solution, then filtering and finally adding to the filtrate a solution of

A. HNO3

B. RbNO3

C. NH4NO3

D. Zn(NO3)2

13. A nitrate solution containing an unknown cation is added to each of the following three test tubes.

A precipitate forms in one test tube only. The unknown cation is

A. Ag+

B. Ca2+

C. Sr2+

D. NH4+

1.0 M Na2SO4 1.0 M Na2S 1.0 M NaOH

14. A solution containing a single unknown cation is added to three test tubes. the following anions were added and observations were recorded.

TEST TUBE ANION ADDED OBSERVATION1 SO4

2- precipitate2 S2- precipitate3 OH- precipitate

The solution contains

A. Sr2+

B. Ag+ or Pb2+

C. Ca2+ or Ba2+

D. K+, NH4+ or H+

Solubility Quiz #7 Common Ion Effect

1. Consider the following equilibrium: CaCO3(s) ⇄ Ca2+(aq) + CO3

2-(aq)

Which of the following reagents, when added to the equilibrium system, would cause more CaCO3 to dissolve?

A. KNO3(s)

B. CaCO3(s)

C. H2C2O4(s)

D. Na2CO3(s)

2. A solution contains a mixture of SO4

2- and S2-. Which of the following cations could be used to remove only the SO4

2- from the solution by precipitation?A. K+

B. Sr2+

C. Pb2+

D. Cu2+

3. Consider the following solubility equilibrium: MgCO3(s)⇄ Mg2+(aq) + CO3

2-(aq)

The addition of which of the following substances would decrease the solubility of MgCO3?

A. H2OB. NaClC. NaOHD. Na2CO3

4. A student could precipitate silver chloride from a saturated solution of silver chloride by adding

A. waterB. sodium iodideC. sodium nitrateD. sodium chloride

5. The greatest mass of solid SnS will dissolve in 1.0 L of

A. H2OB. 0.10 M MgSC. 0.10 M (NH4)2SD. 0.10 M Sn(NO3)2

6. Magnesium carbonate would be the most soluble in a solution of

A. MgCl2

B. NaNO3

C. Na2CO3

D. Mg(NO3)2

7. Sodium iodide is added to a saturated solution of lead (II) iodide/. The net change is

A. [I-] increases and [Pb2+] increasesB. [I-] decreases and [Pb2+] decreasesC. [I-] increases and [Pb2+] decreasesD. [I-] decreases and [Pb2+] increases

8. Consider the following equilibrium: Pbl2(s) + heat ⇄ Pb2+(aq) + 2I-

(aq)

Which of the following changes would result in more Pbl2 dissolving?

A. Adding more Pbl2B. Increasing the pressureC. Adding some Pb(NO3)2

D. Increasing the temperature

9. Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-

(aq)

Sodium chloride is added to a saturated solution of AgCl. The amount of solid AgCl will

A. increase as the equilibrium shifts to the leftB. decrease as the equilibrium shifts to the leftC. increase as the equilibrium shifts to the rightD. decrease as the equilibrium shifts to the right

10. Consider the following equilibrium: NH4Cl(s) + energy ⇄ NH+4(aq) + Cl-

(aq) Which of the following will increase the solubility of ammonium chloride?

A. Stirring the solutionB. Adding more waterC. Adding more NH4Cl(s)

D. Increasing the temperature

Solubility Quiz #8 Titrations and Max Ion Concentration

1. What is the maximum [Ag+] that can exist in 0.20 M NaBrO3?

A. 1.1 x 10-5 MB. 5.3 x 10-5 MC. 2.6 x 10-4 MD. 7.3 x 10-3 M

2. What is the maximum [Sr2+] that can exist in a solution of 0.10 M Na2SO4?

A. 3.4 x 10-7MB. 3.4 x 10-7 MC. 1.7 x 10-6 MD. 5.8 x 10-4 M

3. A student titrates a 25.00 mL sample of well water with 18.2 mL 0.100 M AgNO3 to completely precipitate the chloride ion. The [Cl-] is

A. 1.82 x 10-3 MB. 7.28 x 10-2 MC. 1.37 x 10-1 MD. 1.50 x 10-1 M

4. What is the maximum amount of sodium sulphate, Na2SO4, that will dissolve in 1.0 L of 0.10 M Pb(NO3)2 without forming a precipitate?

A. 1.8 x 10-8 MB. 1.8 x 10-7 MC. 1.3 x 10-4 MD. 1.0 x 10-1 M

5. Consider the following equilibrium: AgCl(s) ⇄ Ag+(aq) + Cl-

(aq)

When BR-(aq) is added to a saturated solution of AgCl,

A. more AgCl dissolves and its solubility product increasesB. more AgCl precipitates and its solubility product decreasesC. more AgCl dissolves and its solubility product remains constantD. more AgCl precipitates and its solubility product remains constant

6. In a saturated solution of zinc hydroxide, at 40oC, the [Zn2+] = 1.8 x 10-5 M. The Ksp of Zn(OH)2 is

A. 5.8 x 10-15

B. 2.3 x 10-14 C. 1.8 x 10-14

D. 6.5 x 10-10

7. What is the [CO2+] and [Cl-] when 0.35 mol of CoCl2 is dissolved in enough water to make 100.0 mL of solution?

A. [CO2+] = 3.5 M and [Cl-] = 3.5 MB. [CO2+] = 3.5 M and [Cl-] = 7.0 MC. [CO2+] = 0.35 M and [Cl-] = 0.35 MD. [CO2+] = 0.35 M and [Cl-] = 0.70 M

8. In which of the following would solid AgCl be most soluble?

A. 1 M HClB. 1 M MgCl2

C. 1 M AgNO3

D. 1 M NH4NO3

9. At 25oC, the maximum [Zn2+] that can exist in a 0.250 M Na2S is

A. 5.0 x 10-26

B. 2.0 x 10-25 C. 8.0 x 10-25 D. 4.5 x 10-13

10. The molar solubility of iron(II)sulphide is

A. 3.6 x 10-37 B. 3.0 x 10-19 C. 6.0 x 10-19 D. 7.7 x 10-10