Deck 18: Solubility and Complex-Ion Equilibria

Question 1

The solubility of CaF2 is 0.00021 mole per liter. What is the solubility product constant for CaF2?

A) 7.3 × 10-12
B) 3.7 × 10-11
C) 8.5 × 10-8
D) 4.4 × 10-8
E) 1.9 × 10-11

Answer 1

3.7 × 10-11

Question 2

The solubility of copper(II) iodate Cu(IO3)2 is reported as 0.12 g per 100 mL. What is the solubility product constant for this salt?

A) 9.8 × 10-8
B) 8.6 × 10-7
C) 7.3 × 10-6
D) 6.4 × 10-5
E) 1.2 × 10-4

Answer 2

9.8 × 10-8

Question 3

The solubility of cerium iodate, Ce(IO3)3, molar mass = 664.83 g/mol, in pure water is 124 mg per 100 mL of water. Calculate the solubility product constant for cerium iodate.

A) 4.9 × 10-19
B) 2.6 × 10-14
C) 8.6 × 10-15
D) 3.3 × 10-10
E) 3.5 × 10-18

Answer 3

3.3 × 10-10

Question 4

Some solid in a solution at equilibrium means the solution is saturated.

Question 5

A small amount of solid calcium hydroxide is shaken vigorously in a test tube almost full of water until no further change occurs and most of the solid settles out. The resulting solution is:

A) concentrated and saturated
B) dilute and saturated
C) dilute and unsaturated
D) dilute and supersaturated
E) concentrated and supersaturated

Question 6

A solute's molar solubility and its molarity are not the same in a saturated aqueous solution.

Question 7

The pH of a solution may affect solubility only if the salt contains the OH- ion.

Question 8

Qualitative cation analysis has been replaced in recent years by instrumental analysis.

Question 9

Fractional precipitation is a method to precipitate only part of the concentration of an ion.

Question 10

The solubility product constant of Li3PO4 is 3.2 × 10-9. What is the molar solubility of Li3PO4 in water?

A) 3.3 × 10-3 M
B) 9.3 × 10-4 M
C) 7.5 × 10-3 M
D) 1.5 × 10-3 M
E) 5.7 × 10-5 M

Question 11

The solubility of magnesium fluoride in water at 18 °C is tabulated as 0.0076 g per 100 mL. What is the solubility product for this salt?

A) 7.6 × 10-6
B) 6.8 × 10-7
C) 8.0 × 10-8
D) 7.3 × 10-9
E) 3.8 × 10-10

Question 12

A saturated solution of silver iodide has a concentration of 9.1 × 10-9 M. What is the Ksp of this compound?

A) 9.1 × 10-18
B) 9.1 × 10-3
C) 9.12 × 10-3
D) (2 × 9.2 × 10-3)2
E) (9.1 × 10-9)2

Question 13

If Qsp is larger than Ksp, precipitation should occur.

Question 14

A saturated solution of magnesium fluoride has a concentration of 1.17 × 10-3 M. For this compound, Ksp =

A) 1.17 × 10-3
B) (1.17 × 10-3)2
C) 4(1.17 × 10-3)3
D) (1.17 × 10-3)3
E) 3(1.17 × 10-3)3

Question 15

Ion pairs as a limitation to Ksp are more likely to be a problem with NaCl than with MgSO4.

Question 16

The molar solubility of SrSO4 (Ksp = 7.6 × 10-7) is:

A) 2.8 × 10-5 M
B) 7.6 × 10-7 M
C) 8.7 × 10-8 M
D) 8.7 × 10-4 M
E) 9.1 × 10-3 M

Question 17

What is the molar solubility of barium carbonate in pure water? (Ksp = 5.1 × 10-9)

A) 5.1 × 10-9 M
B) 7.1 × 10-5 M
C) 1.1 × 10-3
D) 1.7 × 10-3
E) 2.6 × 10-17

Question 18

The diverse ion effect is also called the salt effect.

Question 19

The solubility of a salt MX2 with a molar mass of 114 g/mole is 3.42 g/liter. Calculate the Ksp.

A) 2.70 × 10-5
B) 1.08 × 10-4
C) 9.00 × 10-4
D) 2.25 × 10-4
E) 6.75 × 10-8

Question 20

The common ion effect is a case of Hess's law.

Question 21

The solubility product constant of silver sulfate is 1.6 × 10-5. What is the molar solubility of this compound?

A) 1.6 × 10-5
B) (16/2)1/2 × 10-2
C) (16/4)1/3 × 10-2
D) (16)1/2 × 10-3
E) (16/4)2/3 × 10-2

Question 22

Which of the following reduces the solubility of calcium fluoride?

A) presence of "uncommon ions" such as Na+ and Cl-
B) formation of the ion-pair CaF+
C) formation of the complex ion CaF42-
D) decreasing the pH
E) cooling the solution

Question 23

Which of the following should dissolve the smallest amount of silver sulfide per liter, assuming no complex formation?

A) 0.1 M HNO3
B) 0.1 M Na2S
C) 0.1 M AgNO3
D) 0.10 M NaNO3
E) pure water

Question 24

The Ksp of AgCl is 1.7 × 10-10. How many moles of MnCl2 can be dissolved in one liter of a solution in which [AgNO3] = 3.4 × 10-4 M before a precipitate appears?

A) 5.0 × 10-7 mol
B) 5.8 × 10-14 mol
C) 2.4 × 10-7 mol
D) 2.0 × 106 mol
E) 2.5 × 10-7 mol

Question 25

The solubility product constant of silver bromide is 5.0 × 10-13. What is the molar solubility of this compound?

A) 5.0 × 10-13
B) (50)1/2 × 10-6
C) (50)1/2 × 10-7
D) (5.0/2)1/2 × 10-7
E) (5.0 × 10-13)2

Question 26

Which of the following is least soluble?

A) NiS (Ksp = 8 × 10-37)
B) MnS (Ksp = 8 × 10-16)
C) PtS (Ksp = 8 × 10-73)
D) FeS (Ksp = 4 × 10-19)
E) Hg2Cl2 (Ksp = 1.3 × 10-18)

Question 27

The solubility product constant for iron(III) hydroxide at 22 °C is 6.0 × 10-38. What mass of this compound will dissolve in 100 mL of 0.20 M sodium hydroxide, assuming no complex formation?

A) 6 × 10-39 g
B) 7 × 10-37 g
C) 8 × 10-35 g
D) 9 × 10-33 g
E) 1 × 10-30 g

Question 28

The solubility of a salt MX2 with a molar mass of 170 g/mol is 12.7 g/liter. Calculate the Ksp.

A) 4.17 × 10-4
B) 5.58 × 10-3
C) 9.59 × 103
D) 2.23 × 10-2
E) 1.67 × 10-3

Question 29

Fe(OH)3 is most soluble in which solution?

A) 0.2 M HCl
B) 0.1 M KOH
C) pure water
D) 0.1 M FeCl3
E) 0.2 M CaCl2

Question 30

The solubility product constant of M2CrO4(s) is 7.11 × 10-15. How many moles of M2CrO4(s) will dissolve in 744 mL of solution in which [CrO42-] = 0.056 M?

A) 2.7 × 10-7 mol
B) 1.7 × 10-7 mol
C) 1.2 × 10-5 mol
D) 9.0 × 10-5 mol
E) 3.6 ⊥ 10-7 mol

Question 31

Which of the following has the largest molar solubility?

A) BaSO4, Ksp = 1.1 × 10-10
B) AgCl, Ksp = 1.6 × 10-10
C) Mg(OH)2, Ksp = 2 × 10-11
D) Cr(OH)2, Ksp = 6.3 × 10-11
E) Fe(OH)3, Ksp = 4 × 10-38

Question 32

Predict the molar solubility of the following salt in a solution that contains the given concentration of one of its ions: BaSO4; [SO42-] = 4.3 × 10-5 M; Ksp = 1.1 × 10-10

A) 4.7 × 10-15 M
B) 6.9 × 10-8 M
C) 8.0 × 10-4 M
D) 2.6 × 10-6 M
E) 1.6 × 10-3 M

Question 33

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10-6 calcium carbonate 2.8 × 10-9
Calcium fluoride 5.3 × 10-9
Magnesium fluoride 3.7 × 10-8
Silver carbonate 8.5 × 10-12

A) 2 × 10-5 M Ag+ + 2 × 10-5 M CO32-
B) 2 × 10-5 M Ca2+ + 2 × 10-5 M CO32-
C) 2 × 10-4 M Ca2+ + 2 × 10-2 M F-
D) 2 × 10-5 M Mg2+ + 2 × 10-6 M F-
E) 2 × 10-3 M Ba2+ + 2 × 10-3 M F-

Question 34

Which of the following is most soluble?

A) CuS (Ksp = 8 × 10-37)
B) Bi2S3 (Ksp = 1 × 10-70)
C) Ag2S (Ksp = 6 × 10-51)
D) MnS (Ksp = 7 × 10-16)
E) PbS (Ksp = 3 × 10-28)

Question 35

Which of the following soil additives would best reduce the concentration of dissolved Fe3+ in ground water?

A) lime [Ca(OH)2]
B) saltpeter [KNO3]
C) ferric chloride [FeCl3]
D) ammonium nitrate
E) ammonium sulfate

Question 36

A saturated solution of silver chromate has a concentration of 7.4 × 10-5 M. What is the Ksp of this compound?

A) (7.4 × 10-5)2
B) (7.4 × 10-5)3
C) 3(7.4 × 10-5)3
D) 7.4 × 10-5
E) 4(7.4 × 10-5)3

Question 37

Which of the following salts, each of which has a solubility product equal to 1.0 × 10-6, has the greatest molar solubility?

A) MX
B) MX2
C) MX3
D) M2X

Question 38

Predict the molar solubility of the following salt in a solution that contains the given concentration of one of its ions: AgI; [I-] = 7.2 × 10-6 M; Ksp = 8.5 × 10-17

A) 2.4 × 10-11
B) 9.2 × 10-9
C) 1.7 × 10-6
D) 2.7 × 10-4
E) 1.2 × 10-11

Question 39

When solid silver chloride is shaken with a 0.1 molar solution of potassium iodide, most of the silver chloride is converted to silver iodide. This transformation takes place because:

A) silver iodide is less soluble than silver chloride
B) I- is a better reducing agent than Cl-
C) I- has a larger radius than Cl-
D) the Ksp of AgI is larger than the Ksp of AgCl
E) potassium chloride precipitates

Question 40

What is the molar solubility of PbI2 (Ksp = 7.1 × 10-9) in 0.10 M Pb(NO3)2?

A) 1.3 × 10-4 M
B) 2.6 × 10-3 M
C) 7.1 × 10-8 M
D) 2.7 × 10-4 M
E) 2.7 × 10-5 M

Question 41

When 100 mL each of 2.0 × 10-6 M Ag+ and 2.0 × 10-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10-13.

A) 7.1 × 10-7, no
B) 5.0 × 10-10, yes
C) 1.0 × 10-3, no
D) 5.0 × 10-13, yes
E) 2.5 × 10-10, yes

Question 42

What is the free Ag+ concentration of 0.020 M Ag+ solution mixed with an equal volume of 2.0 M NH3? Kf for [Ag(NH3)2]+ is 1.6 × 107.

A) 1.3 × 10-10
B) 2.0 × 10-14
C) 6.3 × 10-8
D) 6.5 × 10-10
E) 3.1 × 10-10

Question 43

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10-6 calcium carbonate 2.8 × 10-9
Calcium fluoride 5.3 × 10-9
Magnesium fluoride 3.7 × 10-9
Silver carbonate 8.5 × 10-12

A) 2 × 10-5 M Ag+ + 2 × 10-5 M CO32-
B) 2 × 10-4 M Ca2+ + 2 × 10-4 M CO32-
C) 2 × 10-5 M Ca2+ + 2 × 10-3 M F-
D) 2 × 10-5 M Mg2+ + 2 × 10-6 M F-
E) 2 × 10-3 M Ba2+ + 2 × 10-3 M F-

Question 44

If iron(III) acetate is added to be 1 × 10-10 M in a solution that is 0.10 M NH3, what is Qsp and will Fe(OH)3 precipitate? The Ksp of Fe(OH)3 is 4 × 10-38 and Kb for NH3 is 1.8 × 10-5.

A) 1.3 × 10-13, yes
B) 1.7 × 10-16, yes
C) 1.7 × 10-16, no
D) 2.4 × 10-19, yes
E) 2.4 × 10-19, no

Question 45

In which of the following one molar solutions would you expect cadmium sulfide, CdS, to be the most soluble?

A) NaCl
B) HCl
C) NaOH
D) C2H5OH
E) KOH

Question 46

When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaF2 is 5.3 × 10-9.

A) 5.6 × 10-4, no
B) 1.7 × 10-8, yes
C) 4.3 × 10-7, no
D) 1.7 × 10-6, yes
E) 5.4 × 10-5, no

Question 47

What is the approximate concentration of free Fe3+ ion in a solution prepared by mixing equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions? [The net formation constant for FeF5(H2O)2- is 2.0 × 1015.]

A) 2.8 × 10-23 M
B) 6.7 × 10-21 M
C) 6.9 × 10-19 M
D) 4.0 × 10-15 M
E) 8.9 × 10-10 M

Question 48

To a saturated solution of barium carbonate is added just enough sodium sulfate to achieve a maximum sulfate concentration without precipitation of barium sulfate. If no complexes form and the "salt effect" is negligible, what is the concentration of the sulfate ion in this solution? [Ksp for barium carbonate is 1.6 × 10-9; Ksp for barium sulfate is 7.9 × 10-11]

A) 2.8 × 10-5 M
B) 6.7 × 10-6 M
C) 2.0 × 10-6 M
D) 4.0 × 10-5 M
E) 8.9 × 10-5 M

Question 49

Consider an aqueous solution which is 0.020 M in Pb2+ and 0.20 M in Ag+. Concentrated potassium iodide solution (so that volume changes may be neglected) is added gradually with good stirring to this solution. Eventually the iodide ion concentration should increase enough to cause precipitation of the second ion. What will be the concentration of the ion that precipitates first when the second ion just begins to precipitate?

A) 2.0 × 10-17 M
B) 1.2 × 10-8 M
C) 5.0 × 10-20 M
D) 1.4 × 10-13 M
E) 1.2 × 10-5 M

Question 50

If chromium(III) chloride is added to be 1 × 10-12 M in a solution that is 0.10 M NH3, what is Qsp and will Cr(OH)3 precipitate? The Ksp of Cr(OH)3 is 6.3 × 10-31 and Kb for NH3 is 1.8 × 10-5.

A) 1.0 × 10-16, yes
B) 2.4 × 10-23, no
C) 2.2 × 10-19, no
D) 2.2 × 10-19, yes
E) 2.4 × 10-21, yes

Question 51

The solubility product constant of Mg(OH)2 is 9.0 × 10-12. If a solution is 0.010 M with respect to Mg2+ ion, the amount of [OH-] required to start the precipitation of Mg(OH)2 is:

A) 1.5 × 10-7
B) 3.0 × 10-5 M
C) 3.0 × 10-7 M
D) 9.0 × 10-10
E) 1.5 × 10-5 M

Question 52

When 100 mL each of 2.0 × 10-4 M Ag+ and 2.0 × 10-1 M CO32- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of Ag2CO3 is 8.5 × 10-12.

A) 4.2 × 10-8, yes
B) 2.0 × 10-4, no
C) 9.2 × 10-6, no
D) 1.0 × 10-3, no
E) 8.5 × 10-9, yes

Question 53

When 100 mL each of 2.0 × 10-5 M Ca2+ and 2.0 × 10-3 M CO32- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaCO3 is 2.8 × 10-9.

A) 2.8 × 10-6, no
B) 1.0 × 10-3, no
C) 6.9 × 10-5, no
D) 2.8 × 10-3, no
E) 2.8 × 10-6, yes

Question 54

What is the concentration of free Zn2+ if 0.020 M Zn2+ solution is mixed with an equal volume of 2.0 M NH3? Kf for [Zn(NH3)4]2+ is 4.1 × 108.

A) 2.5 × 10-11
B) 2.9 × 10-11
C) 1.7 × 10-10
D) 9.6 × 10-11
E) 2.4 × 10-9

Question 55

A homeowner in Boston becomes concerned that there may be appreciable amounts of lead in her drinking water due to 150-year old water pipes in her house. Consequently, she takes a sample of her drinking water in to be analyzed. The laboratory technician, who is new on the job, has been told to analyze by precipitating the lead ion as the iodide (Ksp = 7.1 × 10-9 for PbI2) by slowly adding small portions of 1.00 M NaI solution. If we assume that the concentration of lead in the solution is 1.00 mg/liter or approximately 4.8 × 10-6 M (this would be 1.0 part per million) is it possible to detect the lead in the drinking water by adding a total of no more than 10.0 mL of NaI solution to a 100 mL sample of drinking water? You must of course consider dilution effects. What is Q?

A) yes, Q = 4.0 × 10-7
B) yes, Q = 3.6 × 10-8
C) no, Q = 1.6 × 10-13
D) no, Q = 3.6 × 10-8
E) no, Q = 4.0 × 10-7

Question 56

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10-6 calcium carbonate 2.8 × 10-9
Calcium fluoride 5.3 × 10-9
Magnesium fluoride 3.7 × 10-8
Silver carbonate 8.5 × 10-12

A) 2 × 10-5 M Ag+ + 2 × 10-5 M CO32-
B) 2 × 10-5 M Ca2+ + 2 × 10-5 M CO32-
C) 2 × 10-5 M Ca2+ + 2 × 10-3 M F-
D) 2 × 10-2 M Mg2+ + 2 × 10-3 M F-
E) 2 × 10-3 M Ba2+ + 2 × 10-3 M F-

Question 57

A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and [Zn2+] = 2.0 × 10-7 M. Sodium oxalate is slowly added so that [C2O42-] increases. Salt BaC2O4 ZnC2O4 Ag2C2O4
Ksp 1.5 × 10-8 1.35 × 10-9 1.1 × 10-11
What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

A) 1.3 × 10-6
B) 2.2 × 10-6
C) 5.0 × 10-5
D) 1.35 × 10-9
E) 1.1 × 10-11

Question 58

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca2+, Cd2+, and Cu2+. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide
Ksp: 4.0 × 10-6 2.0 × 10-14 1.8 × 10-19

A) only Ca(OH)2
B) only Cd(OH)2
C) only Cu(OH)2
D) only Cd(OH)2 and Cu(OH)2
E) Ca(OH)2, Cd(OH)2, and Cu(OH)2

Question 59

In which of the following solutions will the concentration of dissolved silver species be the highest if solid AgNO3 is stirred with 1.00 L of solution?

A) 1.00 M NH3(aq)
B) 1.00 M NaOH
C) 1.00 M Na2SO4(aq)
D) 1.00 M NaCl(aq)
E) 1.00 M NaC2H3O2(aq)

Question 60

What is the free Cu2+ concentration if 0.020 M Cu2+ solution is mixed with an equal volume of 4.0 M NH3? Kf for [Cu(NH3)4]2+ is 1.1 × 1013.

A) 5.7 × 10-15
B) 2.8 × 10-16
C) 6.2 × 10-17
D) 4.5 × 10-15
E) 1.7 × 10-16

Question 61

Write the solubility product constant expression for the following salt: Na2CO3.

A) [Na+][CO32-]
B) [Na+][CO32-]2
C) [Na+]2[CO32-]2
D) [Na+]2[CO32-]
E) 4[Na+]2[CO32-]

Question 62

Choose the compound that is most soluble in water.

A) K2S
B) HgS
C) ZnS
D) SnS
E) PbS

Question 63

At a temperature for which the solubility product constant of calcium carbonate is 4.7 × 10-9, what mass of the salt will dissolve in 100 mL of water?

A) 0.69 mg
B) 0.94 mg
C) 1.2 mg
D) 2.4 mg
E) 4.7 mg

Question 64

Equal volumes of 0.020 M Ag+ solution and 2.0 M NH3 solution are mixed. Kf for [Ag(NH3)2]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10-22.

A) no, Q = 6.3 × 10-9
B) no, Q = 1.9 × 10-29
C) yes, Q = 6.5 × 10-9
D) yes, Q = 4.2 × 10-20
E) no, Q = 2.6 × 10-29

Question 65

The solubility product constant of PbI2 is 7.1 × 10-9. How many moles of PbI2 will precipitate if 250 ml of a 0.200 M solution of NaI are added to 150 ml of 0.100 M solution of Pb(NO3)2? You may neglect hydrolysis.

A) 0.050 mol
B) 1.3 × 10-5 mol
C) 0.015 mol
D) 5.6 × 10-3 mol
E) 0.040 mol

Question 66

What is the concentration of Ca2+ in ppm (mg/L) in cave water saturated with calcite (calcium carbonate, Ksp = 4.7 × 10-9)?

A) 7.5
B) 6.9
C) 5.0
D) 3.8
E) 2.7

Question 67

What is the composition of the precipitate formed when H2S gas is bubbled through 1.0 litre of a solution of 0.010 M Zn2+, 0.010 M Pb2+, and 0.010 M Mn2+, buffered at pH 2.0, until 0.10 mol of H2S has been added? [Ksp values are: ZnS: 1.6 × 10-23; MnS: 7.0 × 10-16; PbS: 7.0 × 10-29. For H2S, Ka1 = 1.0 × 10-7; Ka2 = 1.3 × 10-13.

A) only ZnS
B) only MnS
C) only PbS
D) only MnS and PbS
E) only ZnS and PbS

Question 68

What molar concentration of silver ion could exist in a solution in which the concentration of CrO42- is 1.0 × 10-4 M? (Ksp of Ag2CrO4 = 1.1 × 10-12)

A) 9.0 × 10-8 M
B) 4.5 × 10-3 M
C) 1.0 × 10-4 M
D) 2.1 × 10-4 M
E) 7.5 × 10-5 M

Question 69

Write the solubility product constant expression for the following salt: Ag2SO4.

A) [Ag+][SO42-]
B) [Ag+]2[SO42-]
C) 4[Ag+]2[SO42-]
D) [Ag+][SO42-]2
E) [Ag+]2[SO42-]2

Question 70

Write the solubility product constant for KAl(SO4)2(s)?

A) ([K+] × [Al3+] × 2[SO42-]/[KAl(SO4)2])
B) ([K+] × [Al3+] × [SO42-]/[KAl(SO4)2])
C) ([K+] × [Al3+] × [SO42-])
D) ([K+] × [Al3+] × [SO42-]2)
E) none of these

Question 71

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag+(aq)? (Ksp for AgX(s) = 5.2 × 10-17; Kf for Ag(CN)2- = 5.6 × 1018)

A) 3.1 × 10-3 M
B) 9.4 × 10-6 M
C) 1.8 × 10-10 M
D) 1.2 × 10-3 M
E) 9.6 × 10-3 M

Question 72

Write the solubility product constant expression for the following salt: Ca3(PO4)2.

A) [Ca2+][PO43-]
B) [Ca2+]2[PO43-]3
C) [Ca2+]3[PO43-]2
D) [Ca2+]2[PO43-]
E) [Ca2+][PO43-]2

Question 73

Equal volumes of a 0.020 M Zn2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3)4]2+ is 4.1 × 108. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10-8

A) yes, Q = 11
B) yes, Q = 2.9 × 10-12
C) no, Q = 2.9 × 10-12
D) yes, Q = 2.4 × 10-9
E) no, Q = 2.4 × 10-9

Question 74

Write the solubility product constant expression for the following salt: Ca(OH)2.

A) [Ca2+][OH-]
B) [Ca2+]2[OH-]
C) [Ca2+]3[OH-]
D) [Ca2+]2[OH-]2
E) [Ca2+][OH-]2

Question 75

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10-25
TlBr 3.4 × 10-6
AgCl 1.8 × 10-10
FeS 6 × 10-19
CuI 1.1 × 10-12

A) ZnS
B) TlBr
C) AgCl
D) FeS
E) CuI

Question 76

When 200 mL of 0.10 M BaCl2 is added to 100 mL of 0.30 M Na2SO4, the number of moles of BaSO4 (solubility product = 1.1 × 10-10) precipitated is ________.

A) 0.020 mol
B) 0.010 mol
C) 0.20 mol
D) 0.030 mol
E) 0.10 mol

Question 77

Write the solubility product constant expression for the following salt: PbC2O4.

A) [Pb2+][C2O42-]
B) [Pb2+]2[C2O42-]
C) [Pb2+]2[C2O42-]2
D) [Pb2+][C2O42-]2
E) 4[Pb2+][C2O42-]

Question 78

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

A) Ksp = 9[Ag+]3
B) Ksp = 27[Ag+]4
C) Ksp = [Ag+]1/3
D) Ksp = 0.125[Ag+]
E) Ksp = 0.333[Ag+]4

Question 79

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

A) (Ksp/125)1/6
B) (Ksp/108)1/5
C) (Ksp/27)1/4
D) (Ksp/4)1/3
E) (Ksp)1/2

Question 80

Write the solubility product constant expression for the following salt: CoS.

A) [Co2+]2[S2-]2
B) [Co2+]2[S2-]
C) [Co2+][S2-]
D) [Co2+][S2-]2
E) [Co2+]1/2[S2-]