Central Science: Chapter 17 Flashcards

Which one of the following pairs cannot be mixed together to form a buffer solution?
A) HONH2, HONH3Cl
B) NaCl, HCl
C) RbOH, HF
D) KOH, HNO2
E) H2SO3, KHSO3

Which one of the following pairs cannot be mixed together to form a buffer solution?
A) NH3, NH4Cl
B) NaC2H3O2, HCl (C2H3O2- = acetate)
C) RbOH, HBr
D) KOH, HF
E) H3PO4, KH2PO4

Which one of the following pairs cannot be mixed together to form a buffer solution?
A) C5H5N, C5H5NHCl
B) HC2H3O2, NaOH (C2H3O2- = acetate)
C) KOH, HI
D) NH2CH3, HCl
E) NaClO, HNO3

A solution containing which one of the following pairs of substances will be a buffer solution?
A) NaI, HI
B) KBr, HBr
C) RbCl, HCl
D) CsF, HF
E) none of the above

A solution containing which one of the following pairs of substances will be a buffer solution?
A) KI, HI
B) AgBr, HBr
C) CuCl, HCl
D) CsI, HI
E) none of the above

What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?
A) The concentration of hydronium ions will increase significantly.
B) The concentration of fluoride ions will increase as will the concentration of hydronium ions.
C) The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.
D) The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.
E) The fluoride ions will precipitate out of solution as its acid salt.

The Henderson-Hasselbalch equation is ________.
A) [H+] = Ka + [base]/[acid]
B) pH = pKa - log [base]/[acid]
C) pH = pKa + log [base]/[acid]
D) pH = pKa + log [base]/[acid]
E) pH = log [base]/[acid]

In a solution, when the concentrations of a weak acid and its conjugate base are equal, ________.
A) the system is not at equilibrium
B) the buffering capacity is significantly decreased
C) the -log of the [H+] and the -log of the Ka are equal
D) All of the above are true.

Which solution has the greatest buffering capacity?
A) 0.335M HC2H3O2 and 0.497 M NaC2H3O2
B) 0.520 M HC2H3O2 and 0.116 M NaC2H3O2
C) 0.820 M HC2H3O2 and 0.715 M NaC2H3O2
D) 0.120 M HC2H3O2 and 0.115 M NaC2H3O2

Which solution has the greatest buffering capacity?
A) 0.335 M NH3 and 0.100 M NH4Cl
B) 0.085 M NH3 and 0.090 M NH4Cl
C) 0.540 M NH3 and 0.550 M NH4Cl
D) 0.200 M NH3 and 0.565 M NH4Cl
E) They are all buffer solutions and would all have the same capacity.

The addition of HF and ________ to water produces a buffer solution.
A) HBr
B) KNO3
C) KOH
D) NaCl
E) NaBr

The addition of HCl and ________ to water produces a buffer solution.
A) NH3
B) HC6H5O
C) KOH
D) KNO3
E) HNO3

The addition of HCl and ________ to water produces a buffer solution.
A) HC6H5O
B) C2H5NH2
C) KOH
D) KCl
E) none of the above

The addition of KOH and ________ to water produces a buffer solution.
A) HI
B) NH3
C) KF
D) LiC2H3O2
E) none of the above

Which of the following could be added to a solution of sodium acetate to produce a buffer?
A) acetic acid only
B) acetic acid or hydrochloric acid
C) hydrochloric acid only
D) potassium acetate only
E) sodium chloride or potassium acetate

Which of the following could be added to a solution of NaF to prepare a buffer?
A) HBr
B) NaOH
C) LiC2H3O2
D) KF
E) NH3

Which of the following could be added to a solution of HC2H3O2 to prepare a buffer?
A) HBr
B) HNO3
C) KOH
D) more HC2H3O2
E) None of the above can be added to an acetic acid solution to prepare a buffer.

Which of the following could be added to a solution of acetic acid to prepare a buffer?
A) sodium acetate only
B) sodium acetate or sodium hydroxide
C) nitric acid only
D) hydrofluoric acid or nitric acid
E) sodium hydroxide only

What is the primary buffer system that controls the pH of the blood?
A) carbonate, bicarbonate
B) carbon dioxide, carbonate
C) carbonic acid, bicarbonate
D) carbonic acid, carbon dioxide
E) carbonate, carbonic acid

The ________ and ________ are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood.
A) kidneys, liver
B) lungs, skin
C) lungs, kidneys
D) brain stem, heart
E) spleen, liver

Human blood is considered to be ________.
A) neutral
B) very basic
C) slightly basic
D) slightly acidic
E) very acidic

Decreasing the pH of blood will cause hemoglobin to release ________.
A) CO2
B) N2
C) H2
D) O2
E) Fe

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is ________.
A) a strong acid
B) a strong base
C) a weak acid
D) a weak base
E) neither an acid nor a base

A 50.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about ________ mol/L.
A) 0.120
B) 25.0
C) 0.240
D) 0.0600
E) 0.100

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?
A) methyl red
B) bromthymol blue
C) thymol blue
D) phenolpthalein
E) bromocresol purple

Which compound listed below has the greatest molar solubility in water?
A) CdCO3
B) Cd(OH)2
C) AgI
D) CaF2
E) ZnCO3

Which compound listed below has the smallest molar solubility in water?
A) ZnCO3
B) Cd(OH)2
C) CdCO3
D) AgI
E) CaF2

The molar solubility of ________ is not affected by the pH of the solution.
A) Na3PO4
B) NaF
C) KNO3
D) AlCl3
E) MnS

In which one of the following solutions is silver chloride the most soluble?
A) 0.200 M HCl
B) 0.750 M LiNO3
C) 0.0150 M NH3
D) 0.185 M KCl
E) pure H2O

Which one of the following is not amphoteric?
A) Al(OH)3
B) Ca(OH)2
C) Cr(OH)3
D) Zn(OH)2
E) Sn(OH)2

For which salt should the aqueous solubility be most sensitive to pH?
A) MgCl2
B) Mg(NO3)2
C) MgF2
D) MgBr2
E) MgI2

Which one of the following is amphoteric?
A) H2SO4
B) H2O2
C) CO2
D) H2O
E) NaOH

Why does fluoride treatment render teeth more resistant to decay?
A) Fluoride kills the bacteria in the mouth that make the acids that decay teeth.
B) Fluoride stimulates production of tooth enamel to replace that lost to decay.
C) Fluoride reduces saliva production, keeping teeth drier and thus reducing decay.
D) Fluoride converts hydroxyapatite to fluoroapatite that is less reactive with acids.
E) Fluoride dissolves plaque, reducing its decaying contact with teeth.

A result of the common-ion effect is ________.
A) that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria
B) that common ions, such as Na+ (aq), don't affect equilibrium constants
C) that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X-) that produces a compound (AgX) with a very low solubility
D) that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00
E) that common ions precipitate all counter-ions

The Ka of benzoic acid is 6.30 × 10^-5. The pH of a buffer prepared by combining 50.0 mL of potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.
A) 1.705
B) 0.851
C) 3.406
D) 4.201
E) 2.383

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 X 10^-5
A) 2.516
B) 3.892
C) 4.502
D) 10.158
E) 4.195

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The Ka of acetic acid is 1.76 X 10^-5
A) 2.516
B) 3.892
C) 4.502
D) 10.158
E) 5.056

The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl) in 1.00 L of 1.35 M methylamine (CH3NH2) is ________. The Kb for methylamine is 4.40 X 10^-4 (Assume the final volume is 1.00 L.)
A) 11.03
B) 2.97
C) 3.75
D) 10.64
E) 10.25

The pH of a solution prepared by dissolving 0.350 mol of acid in 1.00 L of 1.10 M of conjugate base is ________. The Kb for the conjugate base is 5.40 X 10^-4 (Assume the final volume is 1.00 L.)
A) 11.23
B) 1.66
C) 11.14
D) 2.77
E) none of the above

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of of KOH is ________ M.
A) 0.4
B) 1 × 10^-7
C) 0.7
D) 3 × 10^-13
E) 4 × 10^-2

The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is ________.
A) 6.29
B) 7.00
C) 8.11
D) 5.78
E) 0.00

The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)2 and 150.0 mL of 0.125 M HCl is ________.
A) 6.29
B) 4.11
C) 1.14
D) 5.78
E) 1.34

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is ________.
A) 13.29
B) 7.00
C) 8.11
D) 11.00
E) 12.14

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is ________ M.
A) 0.234
B) 0.469
C) 0.150
D) 0.300
E) 0.938

The concentration of iodide ions in a saturated solution of lead (II) iodide is ________ M. The solubility product constant of PbI2 is 1.4 x 10^-8
A) 3.8 × 10^-4
B) 3.0 × 10^-3
C) 1.5 × 10^-3
D) 3.5 × 10^-9
E) 1.4 × 10^-8

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF2 is 1.7 x 10^-6
A) 3.8 × 10^-4
B) 3.0 × 10^-3
C) 1.5 × 10^-2
D) 7.5 × 10^-3
E) 1.4 × 10^-4

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 x 10^-17
A) 3.8 × 10^-11
B) 3.0 × 10^-10
C) 9.1 × 10^-9
D) 3.5 × 10^-9
E) 1.4 × 10^-8

The solubility of lead (II) chloride (PbCl2) is 1.6 x 10^-2 M. What is the Ksp of PbCl2?
A) 5.0 × 10^-4
B) 4.1 × 10^-6
C) 3.1 × 10^-7
D) 1.6 × 10^-5
E) 1.6 × 10^-2

The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 x 10^-5 M. What is the Ksp of Mn(OH)2?
A) 1.1 × 10^-14
B) 4.3 × 10^-14
C) 2.1 × 10^-14
D) 4.8 × 10^-10
E) 2.2 × 10^-5

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 x 10^-4 M
A) 2.7 × 10^-12
B) 1.1 × 10^-11
C) 2.0 × 10^-8
D) 3.9 × 10^-8
E) 1.4 × 10^-4

Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 x 10^-12
A) 1.8 × 10^-5
B) 1.4 × 10^-6
C) 2.8 × 10^-6
D) 3.2 × 10^-10
E) 8.1 × 10^-12

Calculate the maximum concentration (in M) of calcium ions (Ca2+) in a solution that contains 0.055 M of CO32-. The Ksp of CaCO3 is 3.4 x 10^-9
A) 5.8 × 10^-5
B) 6.8 × 10^-9
C) 3.4 × 10^-9
D) 6.2 × 10^-8
E) 1.9 × 10^-10

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6x 10^-5
A) 2.0 × 10^-3
B) 1.1 × 10^-4
C) 1.8 × 10^-4
D) 7.1 × 10^-4
E) 1.6 × 10^-5

The Ksp for Cu(OH)2 is 4.8 × 10-20. Determine the molar solubility of Cu(OH)2 in a buffer solution with a pH of 10.1.
A) 6.0 × 10^-10
B) 7.6
C) 3.0 × 10^-12
D) 2.2 × 10^-10
E) 3.8 × 10^-16

Calculate the pH of a solution that is 0.278 M in sodium formate (NaHCO2) and 0.222 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10^-4.
A) 3.843
B) 3.647
C) 13.90
D) 10.16
E) 4.954

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO2). The Ka of formic acid is 1.77 × 10^-4.
A) 35.6
B) 0.1011
C) 10.8
D) 1.03 × 10^-3
E) 3.488

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.152 M in formic acid. The Ka of formic acid is 1.77 × 10^-4.
A) 2.74 × 10^-5
B) 0.0180
C) 3.44
D) 0.581
E) 8.44

Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10^-4
A) 3.093
B) 3.607
C) 14.26
D) 10.91
E) 4.589

What is the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2)? The acid dissociation constant of nitrous acid is 4.50 x 10^-4
A) 55.6
B) 15.5
C) 2.78 × 10^-3
D) 3.448
E) 0.162

What is the percent ionization of nitrous acid in a solution that is 0.189 M in nitrous acid? The acid dissociation constant of nitrous acid is 4.50 x 10^-4
A) 0.0450
B) 8.51 × 10^-5
C) 0.594
D) 4.20
E) 4.88

Which solution would have the greatest buffering capacity?
A) 0.574 M HF and 0.312 M NaF
B) 0.287 M HF and 0.156 M NaF
C) 0.189 M HF and 0.103 M NaF
D) 1.15 M HF and 0.624 M NaF
E) They are all buffer solutions and would all have the same capacity.

The addition of hydrofluoric acid and ________ to water produces a buffer solution.
A) NaF
B) HF
C) NaN
D) NaBr
E) KI

What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10^-4
A) 14.38
B) 10.53
C) 5.38
D) 3.47
E) 4.23

What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO) and 0.131 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10^-8
A) 14.12
B) 6.70
C) 9.07
D) 7.54
E) 7.30

A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The Ka of hypochlorous acid is 1.36 × 10^-3.
A) H2O
B) H3O+
C) hypochlorite ion
D) hypochlorous acid
E) This is a buffer solution: the pH does not change upon addition of acid or base.

A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution. The Ka of benzoic acid is 6.3 × 10^-5.
A) H2O
B) H3O+
C) benzoate
D) benzoic acid
E) This is a buffer solution: the pH does not change upon addition of acid or base.

What is the pH of a solution that contains 0.800 M weak acid (Ka = 1.76 × 10^-5) and 0.172 M of its conjugate base?
A) 8.578
B) 5.422
C) 8.370
D) 4.087
E) 9.913

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.
A) 0.0735
B) 0.0762
C) 0.0980
D) 0.0709
E) 0.00253

A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. What is the concentration (M) of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution?
A) 0.0900
B) 0.122
C) 0.130
D) 0.0953
E) 0.00976

The Ka of some weak acid HA is 1.76 × 10^-5. The pH of a buffer prepared by combining 15.0 mL of 1.00 M A- and 50.0 mL of 1.00 M HA is ________.
A) 1.705
B) 4.232
C) 0.851
D) 2.383
E) 3.406

The Kb of ammonia is 1.76 × 10^-5. What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?
A) 9.372
B) 4.632
C) 4.742
D) 9.291
E) none of the above

Calculate the pH of a solution prepared by dissolving 0.270 mol of weak acid HA and 0.260 mol of its conjugate base in water sufficient to yield 1.00 L of solution. The Ka of HA is 1.77 x 10^-4
A) 2.099
B) 3.736
C) 10.264
D) 3.952
E) 2.307

What is the pH of a solution which is prepared by dissolving 0.850 mol of NH3 and 0.300 mol of NH4Cl in water sufficient to yield 1.00 L of solution? The Kb of ammonia is 1.77 x 10^-5
A) 9.700
B) 5.204
C) 8.781
D) 8.796
E) 4.300

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H) and 0.150 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 1.8 x 10^-5
A) 4.409
B) 3.965
C) 10.035
D) 9.591
E) 5.190

A buffer solution with a pH of 4.31 is prepared with 1.0 M HC2H3O2 and ________ M NaC2H3O2. The Ka of HC2H3O2 is 1.8 x 10^-5
A) 0.37
B) 0.74
C) 4.2 × 10-6
D) 8.8 × 10-10
E) 0.18

A buffer solution with a pH of 4.63 is prepared with 0.14 M formic acid and ________ M sodium formate. The Ka of formic acid is 1.8 x 10^-4
A) 1.1
B) 2.1
C) 5.4 × 10^-6
D) 3.0 × 10^-8
E) 0.54

0.78 M NaC2H3O2 and ________ M HC2H3O2 are required to prepare a buffer solution with a pH of 4.40 . The Ka of HC2H3O2 is 1.8 x 10^-5
A) 3.5
B) 4.1 × 10⁴
C) 1.7
D) 0.86
E) 0.35

________ M formic acid and 0.90 M sodium formate are required to prepare a buffer solution with a pH of 4.78 . The Ka of formic acid is 1.8 x 10^-4
A) 0.17
B) 0.083
C) 3.3 × 103
D) 0.041
E) 9.8

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of 0.0990 M HBr to the equivalence point?
A) 29.5
B) 0.332
C) 4.57
D) 0.208
E) 21.2

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of acetic acid is 4.50 × 10^-4.
A) 11.74
B) 9.26
C) 4.74
D) 7.00
E) 8.81

A 25.0-mL sample of 0.150 M hydrocyanic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of hydrocyanic acid is 4.9 × 10^-10.
A) 5.07
B) 8.6 × 10^-6
C) 9.31
D) 8.49
E) 3.1 × 10⁸

A 25.0 mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hydrazoic acid is 1.9 × 10-5.
A) 2.54
B) 11.47
C) 7.00
D) 4.70
E) 4.74

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 × 10^-8.
A) 7.60
B) 50.0
C) 41.6
D) 60.1
E) 7.35

Which is the correct Ksp expression for PbCl2 (s) dissolving in water?
A) Ksp = [Pb²⁺] [Cl^–]²
B) Ksp = [Pb²⁺] [Cl^–]
C) Ksp = [Pb²⁺]2 [C^l–]
D) Ksp = [PbCl⁺] [Cl^–]
E) Ksp = [Pb⁺] [Cl^2–]²

A 25.0-mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10^-8.
A) 7.25
B) 1.34
C) 4.43
D) 7.58
E) 7.46

A 25.0 mL sample of 0.723 M HCl is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 0.00 mL of KOH is ________ M.
A) 0.0181
B) 0.430
C) 0.723
D) 0.273
E) none of the above

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 10.2 mL of the base is added. The concentration of acetic acid in the sample was ________ M.
A) 0.365
B) 0.175
C) 0.119
D) 0.0714
E) none of the above

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is ________ M.
A) 11.7
B) 0.00214
C) 0.0856
D) 0.267
E) 0.139

The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 35.0 mL of 0.145 M HCl is ________.
A) 1.314
B) 1.403
C) 0.00824
D) 12.597
E) 12.923

What is the pH of a solution which is prepared by mixing 55.0 mL of 0.183 M KOH and 10.0 mL of 0.145 M HC2H3O2?
A) 13.122
B) 9.97
C) 7.74
D) 0.878
E) none of the above

What is the molar solubility of calcium carbonate ( CaCO3 ) in water? The solubility-product constant for CaCO3 is 4.5 × 10^-9 at 25 °C.
A) 2.3 × 10^-9
B) 9.0 × 10^-9
C) 8.35
D) 9.5 × 10^-5
E) 6.7 × 10^-5

What is the molar solubility of silver carbonate ( Ag2CO3 ) in water? The Ksp for Ag2CO3 is 8.1 × 10^-12 at 25 °C
A) 1.3 × 10^-4
B) 1.4 × 10^-6
C) 2.0 × 10^-4
D) 4.0 × 10^-6
E) 2.7 × 10-¹²

In which aqueous system is CaF2 least soluble?
A) H2O
B) 0.5 M HF
C) 0.2 M HF
D) 1.0 M HNO3
E) 0.8 M KF

AgBr would have the lowest solubility in ________.
A) 0.040 M SrBr2
B) pure H2O
C) 0.040 M NaBr
D) 0.040 M KBr
E) 0.010 M AgNO3

In which of the following aqueous solutions would you expect AgI to have the highest solubility?
A) pure water
B) 0.050 M BaI2
C) 0.050 M NaI
D) 0.050 M KI
E) 0.010 M AgNO3

In which of the following aqueous solutions would you expect AgF to have the lowest solubility?
A) 0.030 M LiF
B) pure water
C) 0.023 M NaF
D) 0.015 M KF
E) 0.0075 M AgNO3

) In which of the following aqueous solutions would you expect AgF to have the highest solubility?
A) 0.00750 M LiF
B) 0.030 M AgNO3
C) 0.023 M NaF
D) 0.015 M KF
E) AgF will have the same solubility in all solutions.

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?
A) 0.0100 M KBr
B) 0.040 M CuNO3
C) 0.030 M NaBr
D) 0.020 M LiBr
E) CuBr will have the same solubility in all solutions.

In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?
A) 0.020 M BaCl2
B) 0.020 M Pb(NO3)2
C) 0.020 M NaCl
D) 0.020 M KCl
E) pure water

Of the substances below, ________ will decrease the solubility of Pb(CN)2 in a saturated solution.
A) Pb(MnO4)2
B) NaMnO4
C) HMnO4
D) H2O2
E) NaCl

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba²⁺. When the concentration of F^- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 x 10^-6
A) 7.0 × 10^-5
B) 1.2 × 10^-2
C) 2.1 × 10^-8
D) 3.0 × 10^-3
E) 1.4 × 10^-4

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-4.

Calculate the pH of a buffer solution that contains 0.010 moles of A- and 0.010 moles of HA in 100 ml of water. The Ka of HA is 1.77 × 10^-5.

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH. What is the final pH? The Ka of HA is 1.77 × 10^-5.

Suppose you have just added 500.0 ml of a solution containing 0.2000 moles of acetic acid per liter to 200.0 ml of 0.250 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10^-5.

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH. What is the final pH? The Ka of acetic acid is 1.77 × 10^-5.

In general, the solubility of a slightly soluble salt is decreased by the presence of a second solute that furnishes a ________.

CaCO3 is very soluble in the presence of ________.

A complex ion is when a metal ion binds to a ________.

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

________ analysis determines how much of a given substance is present.

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each raised by its coefficient in the equilibrium reaction.

The solubility of a slightly soluble salt is increased by the presence of a second solute that provides a common ion to the system.

The solubility of slightly soluble salts containing basic anions is directly proportional to the pH of the solution.