Deck 17: Acid-Base Equilibria and Solubility Equilibria

Question 1

What is the pH of a solution prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl?
[K_a(HOCl)= 3.2 × 10^-8]

A)4.10
B)7.00
C)7.19
D)7.49
E)7.80

Answer 1

7.19

Question 2

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C₆H₅CO₂H)and 0.15 M sodium benzoate (C₆H₅COONa).(K_a = 6.5 × 10^-5 for benzoic acid)

A)3.97
B)4.83
C)4.19
D)3.40
E)4.41

Answer 2

3.97

Question 3

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH)and 0.20 M sodium acetate (CH₃COONa).What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution?
[K_a(CH₃COOH)= 1.8 × 10^-5]

A)4.65
B)4.71
C)4.56
D)4.84
E)5.07

Answer 3

4.71

Question 4

Which pair of substances could form a buffered aqueous solution?

A)HCl,NaCl
B)HNO₃,NaNO₃
C)H₃PO₄,Na H₂PO₄
D)H SO₄,CH₃COOH
E)NH₃,NaOH

Question 5

What is the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO)and 0.80 mole of sodium cyanate (NaCNO)in enough water to make 1.0 liter of solution? [K_a(HCNO)= 2.0 × 10^-4]

A)0.97
B)3.10
C)4.40
D)3.70
E)4.30

Question 6

What is the name is used to describe the situation when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium which shifts the equilibrium?

A)Shift ion
B)Shift reagent
C)Equilibrium ion
D)Common ion effect
E)Ion adduct

Question 7

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)and 1.0 mole of cyanic acid (HCNO)in enough water to make 1.0 liter of solution. [K_a(HCNO)= 2.0 × 10^-4]

A)0.00
B)3.00
C)3.70
D)4.40
E)5.00

Question 8

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H⁺(aq)+ HCOO^-(aq)

A)There is no change in the equilibrium.
B)The equilibrium shifts to the right.
C)More information is needed to answer the question.
D)The equilibrium shifts to the left.
E)The pH decreases.

Question 9

Which pair of substances is capable of forming a buffer in aqueous solution?

A)H₃PO₄,Na₃PO₃
B)HNO₃,NaNO₃
C)HCl,NaCl
D)H₂CO₃,NaNO₂
E)CH₃COOH,CH₃COONa

Question 10

Which may be used to prepare a buffer having a pH of 8.8? K_a = 7 × 10^-3 for H₃PO₄; 8 × 10^-8 for H₂PO₄^-; 5 × 10^-13 for HP O₄^2-

A)NaH₂PO₄ only
B)NaH₂PO₄ and Na₂HPO₄
C)Na₃PO₄ and Na₂HPO₄
D)NaHPO₄ and H₃PO₄
E)H₃PO₄ and Na₃PO₄

Question 11

What is the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl? [K_a(HOCl)= 3.2 × 10^-8]

A)0.39
B)3.94
C)6.58
D)7.49
E)8.40

Question 12

What molar ratio of CH₃COOH to CH₃COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [K_a(CH₃COOH)= 1.8 × 10^-5]

A)0.18
B)0.84
C)1.2
D)5.6
E)0.10

Question 13

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH₃COOH)and 0.30 M sodium acetate (CH₃COONa).What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a(CH₃COOH)= 1.8 × 10^-5]

A)4.41
B)4.74
C)4.56
D)4.92
E)5.07

Question 14

Which of the following acids is the best acid to prepare a buffer with the highest pH?

A)C₅H₅O₅COOH,K_a = 4.0 × 10^-6
B)HOC₆H₄OCOOH,K_a = 1.0 × 10^-3
C)HBrO,K_a = 2.3 × 10^-9
D)C₆H₄(COOH)₂,K_a = 2.9 × 10^-4
E)CH₃COOH,K_a = 1.8 × 10^-5

Question 15

When the concentration of the conjugate base of a weak acid is less than the concentration of the weak acid in a buffer solution,the pH of the solution is

A)less than the pK_a.
B)greater than the pK_a.
C)always acidic.
D)always basic.
E)equal to the pK_a.

Question 16

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺ (aq)+ CH₃COO^- (aq)

A)The equilibrium shifts to the right.
B)There is an increase in percent ionization of acetic acid.
C)Less of hydrogen ion is consumed.
D)There is an increased concentration of acetate ions.
E)Less of the acetate ion is consumed.

Question 17

Which pair of substances cannot form a buffered aqueous solution?

A)HCN and KCN
B)NH₃ and (NH₄)₂SO₄
C)HNO₃ and NaNO₃
D)HF and NaF
E)HNO₂ and NaNO₂

Question 18

What is the effect on equilibrium when sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺(aq)+ CH₃COO^-(aq)

A)There is no change in the equilibrium.
B)The equilibrium shifts to the right.
C)More information is needed to answer the question.
D)The equilibrium shifts to the left.
E)The pH decreases.

Question 19

Which results in a buffered solution?

A)A solution containing a strong acid and its conjugate base
B)A solution containing a strong base and its conjugate acid
C)A solution containing a catalyst
D)A solution containing two organic liquids
E)A solution containing a weak acid and its conjugate base

Question 20

What is the Henderson-Hasselbach equation?

A)
B)
C)
D)
E)

Question 21

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆ (ascorbic acid)and 0.75 M NaHC₆H₆O₆ (sodium ascorbate)?
[K_a (H₂C₆H₆O₆)= 6.8 × 10^-5]

A)3.76
B)3.99
C)4.34
D)4.57
E)5.66

Question 22

Which of the following is correct for the equivalence point in an acid-base titration?

A)The pH is at its highest value for any reaction.
B)The amounts of acid and base combined are in a stoichiometric ratio at the equivalence point in an acid-base titration.
C)The pH is 7.0.
D)The pH is equal to the pK_a of the weak acid.
E)The pH is equal to the pK_b of the weak base.

Question 23

A 50.00-mL solution of 0.10 M HNO₂ is titrated with a 0.10 M KOH solution.After 25.00 mL of the KOH solution is added,what is the pH in the titration flask?
[K_a(HNO₂)= 4.5 × 10^-4]

A)2.17
B)3.35
C)2.41
D)1.48
E)7.00

Question 24

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO.What is the pH of this buffer? [K_a (HCOOH)= 1.7 × 10^-4]

A)2.87
B)3.72
C)3.82
D)3.95
E)4.66

Question 25

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

A)0.025 mol HCl
B)0.063 mol HCl
C)0.082 mol HCl
D)0.50 mol HCl
E)1.0 mol HCl

Question 26

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH.What is the pH of this buffer? [K_a(CH₃COOH)= 1.8 × 10^-5]

A)4.57
B)4.52
C)4.87
D)4.92
E)4.97

Question 27

Which best describes the pH at the equivalence point of a titration of a weak acid with a strong base?

A)Less than zero
B)Between 0 and 7
C)Close to 7.0
D)Between 7 and 14
E)Greater than 14

Question 28

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 M NH₄Cl? K_b = 1.8 × 10^-5

A)1.1 × 10^-5 M
B)3.0 × 10^-6 M
C)3.3 × 10^-9 M
D)5.6 × 10^-10 M
E)9.3 × 10^-10 M

Question 29

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

A)1.0
B)6.0
C)7.0
D)8.0
E)13.0

Question 30

A 20.0-mL sample of 0.25 M HNO₃ is titrated with 0.15 M NaOH.What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

A)2.00
B)1.60
C)1.05
D)1.00
E)0.00

Question 31

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74.What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

A)4.77
B)4.71
C)4.68
D)4.62
E)1.70.

Question 32

What is the pH of a buffer that consists of 0.20 M Na H₂PO₄ and 0.40 M Na₂HPO₄? [K_a(Na H₂PO₄)= 6.2 × 10^-8]

A)6.51
B)6.91
C)7.51
D)7.90
E)8.13

Question 33

Which is the best acid to prepare a buffer with the lowest pH?

A)C₅H₅O₅COOH,K_a = 4.0 × 10^-6
B)HOC₆H₄OCOOH,K_a = 1.0 × 10^-3
C)HBrO,K_a = 2.3 × 10^-9
D)C₆H₄(COOH)₂,K_a = 2.9 × 10^-4
E)CH₃COOH,K_a = 1.8 × 10^-5

Question 34

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH.What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

A)0.85
B)2.96
C)2.85
D)1.49
E)3.81

Question 35

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH.What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

A)1.00
B)3.13
C)10.87
D)11.05
E)13.14

Question 36

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? [K_a(CH₃COOH)= 1.8 × 10^-5]

A)3.43
B)4.64
C)4.85
D)4.74
E)6.06

Question 37

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [K_a(HCOOH)= 1.7 × 10^-4]

A)1.1 × 10^-4 M
B)2.6 × 10^-4 M
C)4.3 × 10^-4 M
D)6.7 × 10^-5 M
E)1.7 × 10^-4 M

Question 38

Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

A)Less than zero
B)Between 0 and 7
C)Close to 7.0
D)Between 7 and 14
E)Greater than 14

Question 39

Which is the best choice for preparing a buffer with a pH of 3.5?

A)C₅H₅O₅COOH,K_a = 4.0 × 10^-6
B)HOC₆H₄OCOOH,K_a = 1.0 × 10^-3
C)HBrO,K_a = 2.3 × 10^-9
D)C₆H₄(COOH)₂,K_a = 2.9 × 10^-4
E)CH₃COOH,K_a = 1.8 ×10^-5

Question 40

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

A)14.0
B)7.0
C)3.5
D)1.0
E)0.0

Question 41

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M)with a strong base of the same concentration?

A)
B)
C)
D)
E)

Question 42

When a strong acid is titrated with a strong base,the pH at the equivalence point

A)is greater than 7.0.
B)is equal to 7.0.
C)is between 3.5 and 7.0.
D)is equal to the p K_a of the acid.
E)is equal to 3.5.

Question 43

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl.What is the pH of the solution after 23.0 mL of HCl have been added to the base?

A)1.26
B)1.67
C)12.33
D)12.74
E)13.03

Question 44

When a weak acid is titrated with a strong base,the pH at the equivalence point

A)is greater than 7.0.
B)is equal to 7.0.
C)is less than 7.0.
D)is equal to the pK_a of the acid.
E)is equal to the pK_b of the conjugate base.

Question 45

For PbCl₂ (K_sp = 2.4 × 10^-4),will a precipitate of PbCl₂ form when 0.10 L of 3.0 × 10^-2M Pb(NO₃)₂ is added to 400 mL of 9.0 × 10^-2M NaCl?

A)Yes,because Q > K_sp.
B)No,because Q < K_sp.
C)No,because Q = K_sp.
D)Yes,because Q < K_sp.

Question 46

When a weak acid is titrated with a weak base,the pH at the equivalence point

A)is greater than 7.0.
B)is equal to 7.0.
C)is less than 7.0.
D)is determined by the magnitudes of K_a and K_b.
E)depends on the pK_a of the indicator.

Question 47

Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

A)green
B)red
C)blue
D)yellow
E)violet

Question 48

40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.After 20.0 mL of the base solution has been added,the pH in the titration flask is 5.10.What was the concentration of the original acetic acid solution? (K_a(CH₃COOH)= 1.8 × 10^-5)

A)0.11 M
B)0.022 M
C)0.072 M
D)0.050 M
E)0.015 M

Question 49

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [Kb(NH₃)= 1.8 × 10^-5]

A)2.87
B)4.98
C)5.13
D)7.00
E)11.13

Question 50

A 25.0-mL sample of 0.10 M C₂H₅NH₂ (ethylamine)is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? [K_b(C₂H₅NH₂)= 6.5 × 10^-4]

A)11.08
B)10.74
C)10.81
D)10.55
E)10.49

Question 51

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH.The following data were collected during the titration.Determine to K_a for HClO. mL NaOH added
5)00
10)00
15)00
20)00
PH
6)98
7)46
7)93
10)31

A)1.1 × 10^-7
B)3.5 × 10^-8
C)1.2 × 10^-8
D)4.9 × 10^-11
E)None of the answers is correct.

Question 52

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH.What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [K_a(CH₃CH₂COOH)= 1.3 × 10^-5]

A)5.75
B)4.94
C)4.83
D)4.02
E)3.95

Question 53

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 × 10^-10)solution.

A)5.15
B)8.71
C)5.85
D)9.91
E)13.0

Question 54

A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl.What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [K_b(NH₃)= 1.8 × 10^-5]

A)10.26
B)9.30
C)9.21
D)8.30
E)8.21

Question 55

Which is included in the K_sp expression? I.Concentration of cation
II)Concentration of anion
III)Concentration of solid

A)I only
B)II only
C)III only
D)I and II
E)I,II and III

Question 56

Which of the following is correct?

A)Solubility is the concentration of unsaturated ions in solution.
B)K_sp is the same as the solubility.
C)K_sp is an equilibrium constant and solubility is the concentration of a saturated solution.
D)K_sp is the solubility product constant for a precipitate.
E)Solubility = K_w × K_sp.

Question 57

When a strong acid is titrated with a weak base,the pH at the equivalence point

A)is greater than 7.0.
B)is equal to 7.0.
C)is less than 7.0.
D)is equal to the pK_a of the conjugate acid.
E)is equal to the pK_b of the base.

Question 58

The indicator propyl red has K_a = 3.3 × 10^-6.What would be the approximate pH range over which it would change color?

A)3.5 - 5.5
B)4.5 - 6.5
C)5.5 - 7.5
D)6.5 - 8.5
E)7.5 - 9.5

Question 59

Which indicator would be the best to use if 0.050 M benzoic acid (K_a = 6.6 × 10^-5)is titrated with 0.050 M NaOH?

A)bromphenol blue,pH range: 3.0 - 4.5
B)bromcresol green,pH range: 3.8 - 5.4
C)alizarin,pH range: 5.7 - 7.2
D)phenol red,pH range: 6.9 - 8.5

Question 60

The solubility of lead(II)iodide is 0.064 g/100 mL at 20°C.What is the solubility product for lead(II)iodide?

A)1.1 × 10^-8
B)2.7 × 10^-9
C)1.1 × 10^-11
D)2.7 × 10^-12
E)1.1 × 10^-3

Question 61

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO₃)₂.Which statement is correct? [K_sp(Ca(OH)₂)= 6.5 × 10^-6]

A)Calcium hydroxide precipitates until the solution is saturated.
B)The solution is unsaturated and no precipitate forms.
C)The concentration of calcium ions is reduced by the addition of the hydroxide ions.
D)Potassium nitrate precipitates until the solution is saturated.
E)The presence of KOH will raise the solubility of Ca(NO₃)₂.

Question 62

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

A)1.8 × 10^-4
B)3.6 × 10^-4
C)1.3 × 10^-7
D)3.2 × 10^-8
E)2.8 × 10^-14

Question 63

mL of 0.150 M KI? [K_sp(PbI₂)=1.4 × 10^-8]

A)2.2 × 10^-2 M
B)1.5 × 10^-7 M
C)6.2 × 10^-7 M
D)9.3 × 10^-8 M
E)1.4 × 10^-8 M

Question 64

The solubility of lead(II)chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?

A)4.9 × 10^-2
B)1.7 × 10^-5
C)8.5 × 10^-6
D)4.2 × 10^-6
E)2.6 × 10^-4

Question 65

Calculate the solubility of silver oxalate,Ag₂C₂ O₄,in pure water. [K_sp(Ag₂C₂O₄)= 1.0 × 10^-11]

A)1.4 × 10^-4 M
B)8.2 × 10^-5 M
C)5.4 × 10^-5 M
D)3.2 × 10^-6 M
E)2.5 × 10^-12 M

Question 66

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10^-3 M MgCl₂ are added to 500.0 mL of 1.2 × 10^-3 M NaF?
[K_sp (MgF₂)= 6.9 × 10^-9]

A)Yes,because Q > K_sp.
B)No,because Q < K_sp.
C)No,because Q = K_sp.
D)Yes,because Q < K_sp.
E)No,because Q > K_sp.

Question 67

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(P O₄)₂?

A)7.46 × 10^-11
B)2.68 × 10^-9
C)5.19 × 10^-24
D)4.80 × 10^-26
E)1.20 × 10^-26

Question 68

Will a precipitate (ppt)form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

A)Yes,the ppt is AgNO₃(s).
B)Yes,the ppt is AgBr(s).
C)Yes,the ppt is NaBr(s).
D)Yes,the ppt is NaNO₃(s).
E)No,a precipitate will not form.

Question 69

Calculate the solubility of zinc hydroxide,Zn(OH)₂,in 1.00 M NaOH.K_sp = 3.0 × 10^-16 for Zn(OH)₂,K_f = 3.0 × 10¹⁵ for Zn(OH)₄^2-

A)0.60 M
B)0.52 M
C)0.37 M
D)0.32 M
E)0.24 M

Question 70

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III)fluoride.[K_sp(CrF₃)= 6.6 × 10^-11]

A)0.023 M
B)0.032 M
C)7.7 × 10^-8 M
D)2.9 × 10^-9 M
E)6.9 × 10^-10 M

Question 71

Which compound has the lowest solubility in pure water?

A)Ag₂C₂O₄,K_sp = 1.0 × 10^-11
B)PbCl₂,K_sp = 1.7 × 10^-5
C)FePO₄,K_sp = 1.3 × 10-22
D)Ca₃(PO₄)₂,K_sp = 1.2 × 10^-26
E)MgF₂,K_sp = 6.9 × 10^-9

Question 72

Consider the dissolution of MnS in water.[K_sp(MnS)=3.0 × 10^-14] MnS(s)+ H₂O(l) Mn²⁺(aq)+ HS^-(aq)+ OH^-(aq)
How is the solubility of manganese(II)sulfide affected by the addition of aqueous potassium hydroxide to the system?

A)The solubility will be unchanged.
B)The solubility will decrease.
C)The solubility will increase.
D)The amount of KOH added must be known before its effect can be predicted.
E)The pK_a of H₂S is needed before a reliable prediction can be made.

Question 73

Write the ion product expression for calcium phosphate,Ca₃(P O₄)₂.

A)
B)
C)
D)
E)(3 × [Ca²⁺])(2 × [P O₄^3- ]

Question 74

Will a precipitate (ppt)form when 20.0 mL of 1.1 × 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 ×10^-4M Na₂CO₃?

A)Yes,the ppt is Ba(NO₃)₂.
B)Yes,the ppt is NaNO₃.
C)Yes,the ppt is BaCO₃.
D)Yes,the ppt is Na2CO₃.
E)No,a precipitate will not form.

Question 75

The molar solubility of tin(II)iodide is 1.28 × 10^-2 mol/L.What is K_sp for this compound?

A)8.39 × 10^-6
B)1.28 × 10^-2
C)4.20 × 10^-6
D)1.64 × 10^-4
E)2.10 × 10^-6

Question 76

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃)₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

A)A precipitate of PbS forms.
B)A precipitate of NaNO₃ forms.
C)A precipitate of Na₂S forms.
D)A precipitate of Pb(NO₃)₂ forms.
E)No precipitate forms.

Question 77

Which compound has the highest solubility in pure water?

A)Ag₂C₂O₄,K_sp = 1.0 × 10^-11
B)PbCl₂,K_sp = 1.7 × 10^-5
C)CaSO₄,K_sp = 2.4 × 10^-5
D)Ca₃(PO₄)₂,K_sp = 1.2 × 10^-26
E)MgF₂,K_sp = 6.9 × 10^-9

Question 78

The molar solubility of manganese(II)carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

A)4.2 × 10^-6
B)8.4 × 10^-6
C)3.0 × 10^-16
D)1.8 × 10^-11
E)2.0 × 10^-3

Question 79

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂)= 6.9 × 10^-9] rev: 08_14_2014_QC_52437

A)1.4 × 10⁷ M
B)6.9 × 10^-9 M
C)6.9 × 10^-8 M
D)1.7 × 10^-7 M
E)6.9 × 10^-7 M

Question 80

What is the ion product expression for magnesium fluoride,MgF₂?

A)
B)
C)
D)
E)