Question 1

Which salt would you predict to have a solubility in water that increases as the pH decreases?

Accepted Answer

A) calcium fluoride 
B) silver chloride 
C) silver iodide 
D) mercury(I) bromide 
E) lead(II) chloride 
A) calcium fluoride 
B) silver chloride 
C) silver iodide 
D) mercury(I) bromide 
E) lead(II) chloride

Question 2

A Lewis acid is ________

Accepted Answer

A) a proton donor. 
B) a proton acceptor. 
C) an electron-pair donor. 
D) an electron-pair acceptor. 
E) never viewed also as a Brønsted-Lowry acid. 
A) a proton donor. 
B) a proton acceptor. 
C) an electron-pair donor. 
D) an electron-pair acceptor. 
E) never viewed also as a Brønsted-Lowry acid.

Question 3

Halfway to the equivalence point in a titration curve of a weak acid with a strong base, ________

Accepted Answer

A) nothing is happening yet. 
B) the pH F1F1F1S1F1F1F10 pKa of the weak acid. 
C) pH F1F1F1S1F1F1F10 3.5 exactly. 
D) pH F1F1F1S1F1F1F10 pKa of the indicator. 
E) the pH has not yet changed. 
A) nothing is happening yet. 
B) the pH F1F1F1S1F1F1F10 pKa of the weak acid. 
C) pH F1F1F1S1F1F1F10 3.5 exactly. 
D) pH F1F1F1S1F1F1F10 pKa of the indicator. 
E) the pH has not yet changed.

Question 4

To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (Ka F1F1F1S1F1F1F10 6.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108) and disodium hydrogen phosphate (Ka F1F1F1S1F1F1F10 3.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1013) together in an aqueous solution. What mole ratio of Na2HPO4/NaH2PO4 did she need to use?

Accepted Answer

A) 1.2 
B) 1.6 
C) 0.90 
D) 1.0 
E) 0.96 
A) 1.2 
B) 1.6 
C) 0.90 
D) 1.0 
E) 0.96

Question 5

Suppression of the solubility of one ion by the addition of the counter-ion in its insoluble salt is known as the ________

Accepted Answer

A) ionic suppression effect. 
B) counter-ion effect. 
C) common-ion effect. 
D) excession effect. 
E) supersaturation effect. 
A) ionic suppression effect. 
B) counter-ion effect. 
C) common-ion effect. 
D) excession effect. 
E) supersaturation effect.

Question 6

Which of the following represents the correct Ksp expression for the reaction shown below? Zn3(PO4)2(s)   3Zn2F1F1F1S1F1F1F10(aq) F1F1F1S1F1F1F10 2PO43F1F1F1S1F1F1F10(aq)

Accepted Answer

A) [Zn2F1F1F1S1F1F1F10][PO43F1F1F1S1F1F1F10] 
B) 3[Zn2F1F1F1S1F1F1F10] F1F1F1S1F1F1F10 2[PO43F1F1F1S1F1F1F10] 
C)    
D)    
E) [Zn2F1F1F1S1F1F1F10]3[PO43F1F1F1S1F1F1F10]2 
A) [Zn2F1F1F1S1F1F1F10][PO43F1F1F1S1F1F1F10] 
B) 3[Zn2F1F1F1S1F1F1F10] F1F1F1S1F1F1F10 2[PO43F1F1F1S1F1F1F10] 
C)    
D)    
E) [Zn2F1F1F1S1F1F1F10]3[PO43F1F1F1S1F1F1F10]2

Question 7

If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a Ksp value of 9.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1011.

Accepted Answer

A) Barium sulfate will precipitate. 
B) There will be no precipitate. 
C) It is impossible to tell. 
D) Sodium nitrate will precipitate. 
E) Barium nitrate will precipitate. 
A) Barium sulfate will precipitate. 
B) There will be no precipitate. 
C) It is impossible to tell. 
D) Sodium nitrate will precipitate. 
E) Barium nitrate will precipitate.

Question 8

Which one of the following would make the best buffer? (Ac F1F1F1S1F1F1F10 acetate)

Accepted Answer

A) a solution of hydrochloric acid and sodium chloride, HCl and NaCl 
B) a solution of acetic acid and ammonia, NaAc and NH3 
C) a solution of acetic acid and ammonium chloride, HAc and NH4Cl 
D) a solution of sodium acetate and ammonium chloride, NaAc and NH4Cl 
E) a solution of ammonia and ammonium chloride, NH3 and NH4Cl 
A) a solution of hydrochloric acid and sodium chloride, HCl and NaCl 
B) a solution of acetic acid and ammonia, NaAc and NH3 
C) a solution of acetic acid and ammonium chloride, HAc and NH4Cl 
D) a solution of sodium acetate and ammonium chloride, NaAc and NH4Cl 
E) a solution of ammonia and ammonium chloride, NH3 and NH4Cl

Question 9

A Lewis base is ________

Accepted Answer

A) an electron-pair acceptor. 
B) an electron-pair donor. 
C) a proton donor. 
D) a proton acceptor. 
E) never viewed also as a Brønsted-Lowry base. 
A) an electron-pair acceptor. 
B) an electron-pair donor. 
C) a proton donor. 
D) a proton acceptor. 
E) never viewed also as a Brønsted-Lowry base.

Question 10

Which statement A-D regarding a complex ion in a transition metal coordination compound is not correct?

Accepted Answer

A) The complex ion consists of a metal cation bonded to ligands through coordinate covalent bonds. 
B) The ligands in the complex ion are Lewis bases. 
C) The ligands are said to occupy the inner coordination sphere. 
D) The coordination number is the number of electron pairs bonded to the metal cation. 
E) All complex ions have a net positive charge. 
A) The complex ion consists of a metal cation bonded to ligands through coordinate covalent bonds. 
B) The ligands in the complex ion are Lewis bases. 
C) The ligands are said to occupy the inner coordination sphere. 
D) The coordination number is the number of electron pairs bonded to the metal cation. 
E) All complex ions have a net positive charge.

Question 11

Lactic acid, which is found in milk products, has a pKa of 3.85. A 50.0 mL solution of 0.05 M lactic acid is titrated with 0.025 M sodium hydroxide. What is the pH of the solution after 64.0 mL of the sodium hydroxide has been added?

Accepted Answer

A) 3.85 
B) 3.60 
C) 9.90 
D) 4.10 
E) 7.00 
A) 3.85 
B) 3.60 
C) 9.90 
D) 4.10 
E) 7.00

Question 12

A Lewis acid is any species capable of ________ an electron pair.

Accepted Answer

A) accepting 
B) donating 
C) creating 
D) neutralizing 
E) losing 
A) accepting 
B) donating 
C) creating 
D) neutralizing 
E) losing

Question 13

The solubility product for an insoluble salt with the formula M2X3 is written as ________, where s is the molar solubility.

Accepted Answer

A) Ksp F1F1F1S1F1F1F10 108s5 
B) Ksp F1F1F1S1F1F1F10 6s5 
C) Ksp F1F1F1S1F1F1F10 18s5 
D) Ksp F1F1F1S1F1F1F10 s5 
E) Ksp F1F1F1S1F1F1F10 56s5 
A) Ksp F1F1F1S1F1F1F10 108s5 
B) Ksp F1F1F1S1F1F1F10 6s5 
C) Ksp F1F1F1S1F1F1F10 18s5 
D) Ksp F1F1F1S1F1F1F10 s5 
E) Ksp F1F1F1S1F1F1F10 56s5

Question 14

The bond between a metal cation and a ligand can best be described as ________

Accepted Answer

A) an ionic bond. 
B) a covalent bond. 
C) a coordinate covalent bond. 
D) a polar covalent bond. 
E) a bidentate bond. 
A) an ionic bond. 
B) a covalent bond. 
C) a coordinate covalent bond. 
D) a polar covalent bond. 
E) a bidentate bond.

Question 15

A solution that contains a weak acid and its conjugate base in roughly equal concentrations is ________

Accepted Answer

A) neither acidic or basic. 
B) a half-acid solution. 
C) a buffer. 
D) a heterogeneous mixture. 
E) neutral. 
A) neither acidic or basic. 
B) a half-acid solution. 
C) a buffer. 
D) a heterogeneous mixture. 
E) neutral.

Question 16

The solubility product for an insoluble salt with the formula MX2 is written as ________, where s is the molar solubility.

Accepted Answer

A) Ksp F1F1F1S1F1F1F10 s2 
B) Ksp F1F1F1S1F1F1F10 4s3 
C) Ksp F1F1F1S1F1F1F10 4s2 
D) Ksp F1F1F1S1F1F1F10 2s3 
E) Ksp F1F1F1S1F1F1F10 2s2 
A) Ksp F1F1F1S1F1F1F10 s2 
B) Ksp F1F1F1S1F1F1F10 4s3 
C) Ksp F1F1F1S1F1F1F10 4s2 
D) Ksp F1F1F1S1F1F1F10 2s3 
E) Ksp F1F1F1S1F1F1F10 2s2

Question 17

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 18

Calculate the pH of a solution that is 0.30 M in ammonia (NH3) and 0.20 M in ammonium chloride (NH4Cl, Ka F1F1F1S1F1F1F10 5.62 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010).

Accepted Answer

Question 19

What would happen to the AgF1F1F1S1F1F1F10 and ClF1F1F1S1F1F1F10 concentrations if NaCl(s) were dissolved in a saturated solution of AgCl in water?

Accepted Answer

A) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] both would increase. 
B) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] both would decrease. 
C) [AgF1F1F1S1F1F1F10] would become larger, and [ClF1F1F1S1F1F1F10] would become smaller. 
D) [AgF1F1F1S1F1F1F10] would become smaller, and [ClF1F1F1S1F1F1F10] would become larger. 
E) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] would remain the same because the solution is saturated. 
A) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] both would increase. 
B) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] both would decrease. 
C) [AgF1F1F1S1F1F1F10] would become larger, and [ClF1F1F1S1F1F1F10] would become smaller. 
D) [AgF1F1F1S1F1F1F10] would become smaller, and [ClF1F1F1S1F1F1F10] would become larger. 
E) [AgF1F1F1S1F1F1F10] and [ClF1F1F1S1F1F1F10] would remain the same because the solution is saturated.

Question 20

The solubility product for an insoluble salt with the formula MX 3 is written as ________, where s is the molar solubility.

Accepted Answer

A) Ksp F1F1F1S1F1F1F10 s2 
B) Ksp F1F1F1S1F1F1F10 4s3 
C) Ksp F1F1F1S1F1F1F10 27s4 
D) Ksp F1F1F1S1F1F1F10 3s3 
E) Ksp F1F1F1S1F1F1F10 3s4 
A) Ksp F1F1F1S1F1F1F10 s2 
B) Ksp F1F1F1S1F1F1F10 4s3 
C) Ksp F1F1F1S1F1F1F10 27s4 
D) Ksp F1F1F1S1F1F1F10 3s3 
E) Ksp F1F1F1S1F1F1F10 3s4

Exam 16: Additional Aqueous Equilibria: Chemistry and the Oceans

Which salt would you predict to have a solubility in water that increases as the pH decreases?

A Lewis acid is ________

Halfway to the equivalence point in a titration curve of a weak acid with a strong base, ________

Suppression of the solubility of one ion by the addition of the counter-ion in its insoluble salt is known as the ________

Which of the following represents the correct Ksp expression for the reaction shown below? Zn3(PO4)2(s) 3Zn2(aq)  2PO43(aq)

If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a Ksp value of 9.1  1011.

Which one of the following would make the best buffer? (Ac  acetate)

A Lewis base is ________

Which statement A-D regarding a complex ion in a transition metal coordination compound is not correct?

Lactic acid, which is found in milk products, has a pKa of 3.85. A 50.0 mL solution of 0.05 M lactic acid is titrated with 0.025 M sodium hydroxide. What is the pH of the solution after 64.0 mL of the sodium hydroxide has been added?

A Lewis acid is any species capable of ________ an electron pair.

The solubility product for an insoluble salt with the formula M2X3 is written as ________, where s is the molar solubility.

The bond between a metal cation and a ligand can best be described as ________

A solution that contains a weak acid and its conjugate base in roughly equal concentrations is ________

The solubility product for an insoluble salt with the formula MX2 is written as ________, where s is the molar solubility.

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Calculate the pH of a solution that is 0.30 M in ammonia (NH3) and 0.20 M in ammonium chloride (NH4Cl, Ka  5.62  1010).

What would happen to the Ag and Cl concentrations if NaCl(s) were dissolved in a saturated solution of AgCl in water?

The solubility product for an insoluble salt with the formula MX 3 is written as ________, where s is the molar solubility.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Which of the following represents the correct K_spexpression for the reaction shown below? Zn₃(PO₄)₂(s) 3Zn²^(aq)  2PO₄³^(aq)

If 500 mL of a solution containing 1.00 g of barium nitrate (199.33 g/mol) is combined with 500 mL of a solution containing 1.00 g of sodium sulfate (142.03 g/mol), will there be a precipitate? Barium sulfate has a K_sp value of 9.1  10^¹¹.

Lactic acid, which is found in milk products, has a pK_a of 3.85. A 50.0 mL solution of 0.05 M lactic acid is titrated with 0.025 M sodium hydroxide. What is the pH of the solution after 64.0 mL of the sodium hydroxide has been added?

The solubility product for an insoluble salt with the formula M₂X₃ is written as ________, where s is the molar solubility.

The solubility product for an insoluble salt with the formula MX₂ is written as ________, where s is the molar solubility.

Calculate the pH of a solution that is 0.30 M in ammonia (NH₃) and 0.20 M in ammonium chloride (NH₄Cl, K_a  5.62  10^¹⁰).

What would happen to the Ag^ and Cl^ concentrations if NaCl(s) were dissolved in a saturated solution of AgCl in water?

The solubility product for an insoluble salt with the formula MX ₃ is written as ________, where s is the molar solubility.