Deck 15: Applications of Aqueous Equilibria

Question 1

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5.
CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

A)1)8 × 10^-19
B)5)6 × 10^-10
C)1)8 × 10^-8
D)1)8 × 10⁹

Answer 1

1)8 × 10⁹

Question 2

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃)and morphine (C₁₇H₁₉NO₃)is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

A)1)3 × 10^-22
B)6)3 × 10^-23
C)7)4 × 10^-7
D)1)1 × 10⁷

Answer 2

7)4 × 10^-7

Question 3

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

A)8)95
B)9)26
C)9)56
D)11.13

Answer 3

9)56

Question 4

Which is a net ionic equation for the neutralization of a weak acid with a strong base?

A)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
B)H₃O⁺(aq)+ OH^-(aq)⇌ 2 H₂O(l)
C)HF(aq)+ NaOH(aq)⇌ H₂O(l)+ NaF(aq)
D)HF(aq)+ OH^-(aq)⇌ H₂O(l)+ F^-(aq)

Question 5

What is the approximate value of the equilibrium constant,K_n,for the neutralization of pyridine with hydrochloric acid,shown in the equation below? The K_b for pyridine is 1.8 × 10^-9.
HCl(aq)+ C₅H₅N(aq)⇌ C₅H₅NHCl(aq)

A)5)6 × 10^-10
B)5)6 × 10^-6
C)1)8 × 10⁵
D)5)6 × 10⁸

Question 6

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

A)CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)
B)HCl(aq)+ C₅H₅N(aq)⇌ C₅H₅NHCl(aq)
C)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
D)H₂SO₄(aq)+ 2 KOH(aq)⇌2 H₂O(l)+ K₂SO₄(aq)

Question 7

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

A)K_n = K_aK_bK_w
B)K_n =
C)K_n =
D)K_n =

Question 8

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

A)H₃O⁺
B)Na⁺
C)CH₃CO₂^-
D)OH^-

Question 9

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below?
HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)

A)1)0 × 10²
B)1)0 × 10⁷
C)1)0 × 10¹⁴
D)1)0 × 10²⁸

Question 10

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.050 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

A)2)87
B)4)44
C)4)74
D)5)05

Question 11

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃ solution the pH of the resulting solution will

A)become 7.
B)decrease.
C)increase.
D)remain the same.

Question 12

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is
1)8 × 10^-5.
HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

A)8)1 × 10⁵
B)1)8 × 10⁹
C)4)5 × 10¹⁰
D)8)1 × 10¹⁹

Question 13

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

A)become 7.
B)decrease.
C)increase.
D)remain the same.

Question 14

Which of these neutralization reactions has a pH = 7 when equal molar amounts of acid and base are mixed?

A)CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)
B)HCl(aq)+ C₅H₅N(aq)⇌ C₅H₅NHCl(aq)
C)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
D)HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

Question 15

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

A)H₃O⁺(aq)+ OH^-(aq)⇌ 2 H₂O(l)
B)HF(aq)+ NH₃(aq)⇌ NH₄⁺(aq)+ F^-(aq)
C)HF(aq)+ OH^-(aq)⇌ H₂O(l)+ F^-(aq)
D)H₃O⁺(aq)+ NH₃(aq)⇌ NH₄⁺(aq)+ H₂O(l)

Question 16

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

A)10.27
B)10.57
C)10.87
D)11.78

Question 17

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

A)CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)
B)HCl(aq)+ C₅H₅N(aq)⇌ C₅H₅NHCl(aq)
C)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
D)H₂SO₄(aq)+ 2 KOH(aq)⇌2 H₂O(l)+ K₂SO₄(aq)

Question 18

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄)and codeine (C₁₈H₂₁NO₃)is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?

A)4)8 × 10^-24
B)6)3 × 10^-23
C)1)6 × 10^-6
D)1)4 × 10¹⁵

Question 19

Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?

A)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
B)H₃O⁺(aq)+ OH^-(aq)⇌ 2 H₂O(l)
C)HCl(aq)+ NH₃(aq)⇌ NH₄Cl(aq)
D)H₃O⁺(aq)+ NH₃(aq)⇌ NH₄⁺(aq)+ H₂O(l)

Question 20

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

A)HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)
B)H₃O⁺(aq)+ OH^-(aq)⇌ 2 H₂O(l)
C)HF(aq)+ NaOH(aq)⇌ H₂O(l)+ NaF(aq)
D)HF(aq)+ OH^-(aq)⇌ H₂O(l)+ F^-(aq)

Question 21

What is the pH of a buffered system made by dissolving 17.42 g of KH₂PO₄ and 20.41 g of K₂HPO₄ in water to give a volume of 200.0 mL? The K_a2 for dihydrogen phosphate is 6.2 × 10^-8 and the equilibrium reaction of interest is
H₂PO₄^-(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ HPO₄^-(aq).

A)7)03
B)7)17
C)7)38
D)7)58

Question 22

What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pK_a = 9.60?

A)50%
B)9%
C)5%
D)1%

Question 23

A buffer solution is prepared by dissolving 27.22 g of KH₂PO₄ and 3.37 g of KOH in enough water to make 0.100 L of solution.What is the pH of the H₂PO₄^-/HPO₄^2- buffer if the K_a2 = 6.2 × 10^-8?

A)6)84
B)7)00
C)7)21
D)7)84

Question 24

A buffer solution is prepared by dissolving 0.200 mol of NaH₂PO₄ and 0.100 mol of NaOH in enough water to make 1.00 L of solution.What is the pH of the H₂PO₄^-/HPO₄^2- buffer if the
K_a2 = 6.2 × 10^-8?

A)6)91
B)7)21
C)7)51
D)7)71

Question 25

What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The K_a2 for hydrogen phthalate is 3.1 × 10^-6.

A)3)25
B)5)08
C)5)51
D)5)94

Question 26

What is the pH of 1 L of 0.30 M TRIS,0.60 M TRISH⁺ buffer to which one has added 5.0 mL of 12 M HCl? The K_b for the TRIS/TRISH⁺ is 1.2 × 10^-6.

A)5)92
B)6)36
C)7)36
D)7)64

Question 27

What is the magnitude of the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH₃CO₂H and 0.100 M NaCH₃CO₂? The K_a for acetic acid is1.8 × 10^-5.

A)0)00
B)0)20
C)0)47
D)1)30

Question 28

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5 for CH₃CO₂H.

A)0)50:1
B)0)94:1
C)1)1:1
D)2)0:1

Question 29

What is the Henderson-Hasselbalch equation for the acidic buffer HA/A^-?

A)pH = -log[H₃O⁺]
B)pH = 14 - pOH
C)pH = pK_a + log{[A^-]/[HA]}
D)pH = pK_a - log{[A^-]/[HA]}

Question 30

What volume of 0.100 M NaOH is needed to make 100.0 mL of a buffer solution with a pH of 6.00 if one starts with 50.0 mL of 0.100 M potassium hydrogen phthalate? The K_a2 for potassium hydrogen phthalate is 3.1 × 10^-6.

A)22.4 mL
B)27.6 mL
C)30.2 mL
D)37.8 mL

Question 31

Which is the best acid to use in the preparation of a buffer with pH = 3.3?

A)HOI (K_a = 2.0 × 10^-11)
B)HNO₂ (K_a = 4.5 × 10^-4)
C)HNO₃
D)HIO₃ ((K_a = 1.7 × 10^-1)

Question 32

Which is the best acid to use in the preparation of a buffer with pH = 9.3?

A)CH₃NH₂ (K_b = 3.7 × 10^-4)
B)NH₃ (K_b = 1.8 × 10^-5)
C)NH₂OH (K_b = 9.1 × 10^-9)
D)C₆H₅NH₂ (K_b = 4.3 × 10^-10)

Question 33

What is the pH of a buffer system made by dissolving 10.70 grams of NH₄Cl and 20.00 mL of 12.0 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.8 × 10^-5 for NH₃.

A)9)18
B)9)26
C)9)34
D)11.03

Question 34

What is not a correct expression for the weak acid HA?

A)K_a = [H₃O⁺][A^-]/[HA]
B)pK_a = pH - log{[A^-]/[HA]}
C)pK_a = logK_a
D)pK_a = 14 - pK_b

Question 35

Which statement about buffers is true?

A)Buffers have a pH = 7.
B)Buffers consist of a strong acid and its conjugate base.
C)A buffer does not change pH on addition of a strong acid or strong base.
D)Buffers resist change in pH upon addition of small amounts of strong acid or strong base.

Question 36

When equal molar amounts of the following sets of compounds are mixed in water,which will not form a buffer solution?

A)NaH₂PO₄ with Na₂HPO₄
B)NH₃ with NH₄Cl
C)CH₃CO₂H with NaCH₃CO₂
D)HNO₃ with NaNO₃

Question 37

TRIS {(HOCH₂)₃CNH₂} is one of the most common buffers used in biochemistry.A solution is prepared by adding enough TRIS and 12 M HCl(aq)to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH⁺] = 0.60 M.What is the pH of this buffered system if the pK_b is 5.92?

A)5)92
B)6)22
C)7)78
D)8)08

Question 38

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄^2- and the K_a2 = 6.2 × 10^-8?

A)5)21
B)5)61
C)6)73
D)7)69

Question 39

Which of the following combinations of chemicals could be used to make a buffer solution?

A)HCl/NaOH
B)HCl/NH₃
C)HCl/H₃PO₄
D)NaOH/NH₃

Question 40

What is the percent dissociation of acetic acid if the solution has a pH = 4.74 and a pK_a = 4.74?

A)100%
B)50%
C)10%
D)1%

Question 41

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 100.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

A)12.5 mL
B)50.0 mL
C)100.mL
D)200.mL

Question 42

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

A)0)30
B)3)18
C)3)76
D)4)03

Question 43

What is the pH at the equivalence point of a weak acid-strong base titration?

A)pH < 7
B)pH = 7
C)pH > 7
D)pH = 14.00

Question 44

At what pH is the amino acid glycine with a K_a of 2.51 × 10^-10 sixty-six (66%)percent dissociated?

A)9)60
B)9)89
C)10.10
D)10.60

Question 45

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

A)9)70
B)10.69
C)11.11
D)12.70

Question 46

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? K_a = 1.8 × 10^-4 for formic acid.

A)2)46
B)5)88
C)8)12
D)11.54

Question 47

Which of the following titrations result in a basic solution at the equivalence point?

A)HI titrated with NaCH₃CO₂
B)HOCl titrated with NaOH
C)HBr titrated with KOH
D)Pb(NO₃)₂ titrated with NaI

Question 48

Sulfurous acid,H₂SO₃ has acid dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H₂SO₃?

A)1)82
B)3)60
C)4)25
D)7)20

Question 49

The equivalence point pH of the titration of four weak acids is given.Which is the strongest acid?

A)7)24
B)7)86
C)8)12
D)8)43

Question 50

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added?

A)4)85
B)6)02
C)7)39
D)9)70

Question 51

Which of the following titrations result in an acidic solution at the equivalence point?

A)CH₃COOH titrated with NaOH
B)KF titrated with KOH
C)HCl titrated with NaOH
D)C₅H₅N titrated with HCl

Question 52

What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5 for CH₃CO₂H.

A)9)56
B)8)95
C)5)05
D)4)44

Question 53

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

A)2)34
B)4)85
C)5)59
D)6)72

Question 54

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

A)96%
B)10%
C)5%
D)1%

Question 55

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 28.30 mL of 0.500 M HCl to reach the equivalence point?

A)0)208 M
B)0)353 M
C)0)708 M
D)1)21 M

Question 56

Oxalic acid,H₂C₂O₄ has acid dissociation constants K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.
What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H₂C₂O₄?

A)1)23
B)2)10
C)2)80
D)4)19

Question 57

The equivalence point pH of the titration of four weak bases is given.Which is the strongest base?

A)4)21
B)5)67
C)6)33
D)7)58

Question 58

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

A)0)0134 M
B)0)0476 M
C)0)0567 M
D)0)0676 M

Question 59

What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

A)0)85
B)1)85
C)12.15
D)13.15

Question 60

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

A)1)74
B)5)75
C)8)25
D)12.26

Question 61

What is the molar solubility of AgCl in 1.0 M K₂S₂O₃ if the complex ion Ag(S₂O₃)₂^3- forms? The Ksp for AgCl is 1.8 × 10^-10 and the K_f for Ag(S₂O₃)₂^3- is 2.9 × 10¹³.

A)0)50 M
B)1)0 M
C)1)5 M
D)2)0 M

Question 62

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is 5.6 × 10^-12.

A)5)6 × 10^-10 M
B)5)6 × 10^-8 M
C)2)4 × 10^-6 M
D)1)1 × 10^-4 M

Question 63

What is the most soluble salt of the following set?

A)AgCN with K_sp = 6.0 × 10^-17
B)Al(OH)₃ with K_sp = 1.9 × 10^-33
C)Fe(OH)₃ with K_sp = 2.6 × 10^-39
D)Sn(OH)₂ with K_sp = 1.6 × 10^-19

Question 64

Which of the following reactions are not consistent with the concept of acid base amphoterism?

A)Al(OH)₃(s)+ OH^-(aq)→ Al(OH)₄^-(aq)
B)Al(OH)₃(s)+ 3 H₃O⁺(aq)→ Al³⁺(aq)+ 6 H₂O(l)
C)H₂O(l)+ H₂O(l)⇌ H₃O⁺(aq)+ OH^-(aq)
D)Al(OH)₃(s)⇌ Al³⁺(aq)+ 3 OH^-(aq)

Question 65

Calculate the molar solubility of thallium(I)chloride in 0.30 M NaCl at 25°C.K_sp for TlCl is
1)7 × 10^-4.

A)5)1 × 10^-5 M
B)5)7 × 10^-4 M
C)7)1 × 10^-3 M
D)1)3 × 10^-2 M

Question 66

Precipitation of an ionic compound will occur upon mixing of desired reagents if the initial ion product is ________.

A)greater than the K_sp
B)equal to the pK_sp
C)equal to the K_sp
D)less than the K_sp

Question 67

What is the chromium ion concentration for a saturated solution of Cr(OH)₃ if the K_sp for Cr(OH)₃ is 6.7 × 10^-31?

A)8)19 × 10^-16 M
B)1)26 × 10^-8 M
C)2)17 × 10^-8 M
D)3)76 × 10^-8 M

Question 68

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

A)The BaCrO₄ precipitates first out of solution.
B)The Ag₂CrO₄ precipitates first out of solution and then BaCrO₄ precipitates.
C)Both BaCrO₄ and Ag₂CrO₄ precipitate simultaneously out of solution.
D)Neither BaCrO₄ nor Ag₂CrO₄ precipitates out of solution.

Question 69

In which of the following solutions would solid PbCl₂ be expected to be the least soluble at 25°C?

A)0)1 M HCl
B)0)1 M NaCl
C)0)1 M CaCl₂
D)0)1 M KNO₃

Question 70

What is the silver ion concentration for a saturated solution of Ag₂CO₃ if the K_sp for Ag₂CO₃ is 8.4 × 10^-12?

A)2)90 × 10^-6 M
B)2)03 × 10^-4 M
C)2)56 × 10^-4 M
D)4)06 × 10^-4 M

Question 71

What is the equilibrium constant expression for the K_sp of Ca₃(PO₄)₂?

A)K_sp = [Ca²⁺]³[PO₄^3-]²
B)K_sp = {[Ca²⁺]³[PO₄^3-]²}/[Ca₃PO₄]
C)K_sp = {[Ca²⁺]³[PO₄^3-]²}/{[Ca₃PO₄][H₂O]}
D)K_sp = 1/{[Ca²⁺]³[PO₄^3-]²}

Question 72

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is

A)0)050 M
B)0)10 M
C)0)20 M
D)0)40 M

Question 73

Calculate the solubility (in g/L)of silver carbonate in water at 25°C if the K_sp for Ag₂CO₃ is
8)4 × 10^-12.

A)8)0 × 10^-4 g/L
B)3)5 × 10^-2 g/L
C)4)4 × 10^-2 g/L
D)5)6 × 10^-2 g/L

Question 74

The balanced equation for the solubility equilibrium of Fe(OH)₂ is shown below.What is the equilibrium constant expression for the K_sp of Fe(OH)₂?
Fe(OH)₂(s)⇌ Fe²⁺(aq)+ 2 OH^-(aq)

A)K_sp = {[Fe²⁺][OH^-]²}/{[Fe(OH)₂][H₂O]}
B)K_sp = {[Fe²⁺][OH^-]²}/[Fe(OH)₂]
C)K_sp = [Fe²⁺][OH^-]²
D)K_sp = 1/{[Fe²⁺][OH^-]²}

Question 75

What is the most soluble salt of the following set?

A)Ba(OH)₂ with K_sp = 5.0 × 10^-3
B)Ca(OH)₂ with K_sp = 4.7 × 10^-6
C)Cd(OH)₂ with K_sp = 5.3 × 10^-15
D)Fe(OH)₂ with K_sp = 2.5 × 10^-37

Question 76

Calculate the K_sp for silver sulfate if the solubility of Ag₂SO₄ in pure water is 4.5 g/L.

A)3)0 × 10^-6
B)1)2 × 10^-5
C)2)1 × 10^-4
D)4)2 × 10^-4

Question 77

What is the molar solubility of CaF₂ in 0.10 M NaF solution at 25°C? The K_sp for CaF₂ is

A)8)5 × 10^-10 M
B)3)4 × 10^-10 M
C)3)4 × 10^-9 M
D)2)0 × 10^-4 M

Question 78

What is the molar solubility of lead(II)chromate in 0.10 M HNO₃ if the K_sp for PbCrO₄ is
2)8 × 10^-13? and the K_a2 for H₂CrO₄ is 3.0 × 10^-7? Note that H₂CrO₄ is considered to be a strong acid.

A)9)2 × 10^-11 M
B)2)9 × 10^-10 M
C)9)3 × 10^-7 M
D)3)1 × 10^-4 M

Question 79

Which of the following metal hydroxides are amphoteric?

A)Al(OH)₃,Zn(OH)₂,Cr(OH)₃,Sn(OH)₂
B)Cu(OH)₂,Mn(OH)₂,Fe(OH)₂,Fe(OH)₃
C)Be(OH)₂,Ca(OH)₂,Ba(OH)₂,Sr(OH)₃
D)LiOH,NaOH,KOH,RbOH

Question 80

What is the molar solubility of AgCl in 0.10 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and the K_f for Ag(NH₃)₂⁺ is 1.7 × 10^7.

A)1)3 × 10^-5 M
B)5)0 × 10^-3 M
C)5)5 × 10^-3 M
D)5)5 × 10^-2 M