Question 1

Which of the following species is most likely to function as a ligand in a transition metal complex ion?

Accepted Answer

A) BF4F1F1F1S1F1F1F10 
B) AlBr3 
C) P(CH3)3 
D) Ca2F1F1F1S1F1F1F10 
E) BeCl2 
A) BF4F1F1F1S1F1F1F10 
B) AlBr3 
C) P(CH3)3 
D) Ca2F1F1F1S1F1F1F10 
E) BeCl2

Question 2

Lead pipes were used at one time for delivering drinking water. What is the maximum possible concentration of lead in this water if it comes from lead(II) hydroxide (Ksp F1F1F1S1F1F1F10 2.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1016) dissolving from the surface of the pipes? Note the U.S. Environmental Protection Agency's limit on lead in drinking water is 7.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M.

Accepted Answer

A) 4.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
B) 1.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
C) 6.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
D) 5.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
E) 8.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M 
A) 4.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
B) 1.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
C) 6.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
D) 5.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
E) 8.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M

Question 3

The following titration curve is most likely to be associated with

Accepted Answer

A) the titration of a strong acid with a strong base titrant. 
B) the titration of a weak acid with a strong base titrant. 
C) the titration of a strong base with a strong acid titrant. 
D) the titration of a weak base with a strong acid titrant. 
A) the titration of a strong acid with a strong base titrant. 
B) the titration of a weak acid with a strong base titrant. 
C) the titration of a strong base with a strong acid titrant. 
D) the titration of a weak base with a strong acid titrant.

Question 4

Let s be the number of moles of lead chloride (PbCl2) that dissolve in water to make exactly 1 L of solution.
(1) Write the solubility product expression for lead chloride in terms of s.
(2) Calculate a value for Ksp given that s F1F1F1S1F1F1F10 0.036 M.

Accepted Answer

(1) K_sp F1F1F1S1F1F1F10 [Pb²F1F1

Question 5

Which of the following would be the best choice for preparing a buffer with a pH F1F1F1S1F1F1F10 8.0?

Accepted Answer

A) a solution of formic acid and sodium formate, Ka F1F1F1S1F1F1F10 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
B) a solution of acetic acid and sodium acetate, Ka F1F1F1S1F1F1F10 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
C) a solution of hypochlorous acid and sodium hypochlorite, Ka F1F1F1S1F1F1F10 3.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) a solution of boric acid and sodium borate, Ka F1F1F1S1F1F1F10 5.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 
E) All of these solutions would be equally good choices for making this buffer. 
A) a solution of formic acid and sodium formate, Ka F1F1F1S1F1F1F10 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
B) a solution of acetic acid and sodium acetate, Ka F1F1F1S1F1F1F10 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
C) a solution of hypochlorous acid and sodium hypochlorite, Ka F1F1F1S1F1F1F10 3.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) a solution of boric acid and sodium borate, Ka F1F1F1S1F1F1F10 5.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 
E) All of these solutions would be equally good choices for making this buffer.

Question 6

Which sodium halide salt, if any, would you predict to have a solubility in water that increases as the pH decreases?

Accepted Answer

A) sodium fluoride 
B) sodium chloride 
C) sodium bromide 
D) sodium iodide 
E) The solubility of sodium halide salts should not depend on the pH. 
A) sodium fluoride 
B) sodium chloride 
C) sodium bromide 
D) sodium iodide 
E) The solubility of sodium halide salts should not depend on the pH.

Question 7

Which, if any, of the following compounds form an acidic solution when dissolved in water?
I. CaCl2 
II. CrCl3 
III. NaCl 
IV. FeCl2

Accepted Answer

A) None form an acidic solution. 
B) All form an acidic solution. 
C) Only I and III form an acidic solution. 
D) Only II and IV form an acidic solution. 
E) Only I, II, and IV form an acidic solution. 
A) None form an acidic solution. 
B) All form an acidic solution. 
C) Only I and III form an acidic solution. 
D) Only II and IV form an acidic solution. 
E) Only I, II, and IV form an acidic solution.

Question 8

Define the term Lewis acid and provide an example.

Accepted Answer

A Lewis acid is an electron-pa

Question 9

Which statement A-D regarding transition metal coordination compounds is not correct?

Accepted Answer

A) A coordination compound is formed when a Lewis acid reacts with a Lewis base. 
B) Many, but not all, coordination compounds consist of a complex ion and some number of counter ions. 
C) The Lewis bases attached to the metal ion are called ligands. 
D) A coordination compound has no net electrical charge. 
E) Statements A-D are all correct. 
A) A coordination compound is formed when a Lewis acid reacts with a Lewis base. 
B) Many, but not all, coordination compounds consist of a complex ion and some number of counter ions. 
C) The Lewis bases attached to the metal ion are called ligands. 
D) A coordination compound has no net electrical charge. 
E) Statements A-D are all correct.

Question 10

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates. This phenomenon is called ________

Accepted Answer

A) the common-ion effect. 
B) selective precipitation. 
C) supersaturation. 
D) a solubility anomaly. 
E) deionization. 
A) the common-ion effect. 
B) selective precipitation. 
C) supersaturation. 
D) a solubility anomaly. 
E) deionization.

Question 11

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

Accepted Answer

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

Question 12

Sketch a titration curve for titration of a weak acid with a strong base and label the following areas in the curve: a) before equivalence point, b) equivalence point, and c) after equivalence. Describe how the pH is calculated in each of the three regions of the curve.

Accepted Answer

@#IMG-DLM& a) pH in the region before equivalence

Question 13

A solution of ammonia (0.12 M, 15.00 mL) was titrated with 0.2 M hydrochloric acid (Kb of ammonia F1F1F1S1F1F1F10 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105). What is the pH at the equivalence point?

Accepted Answer

A) 3.75 
B) 5.19 
C) 7.00 
D) 8.81 
E) 10.25 
A) 3.75 
B) 5.19 
C) 7.00 
D) 8.81 
E) 10.25

Question 14

In the following reaction, which species is the Lewis acid?

Accepted Answer

A) Cu2F1F1F1S1F1F1F10 
B) NH3 
C) [Cu(NH3)]2F1F1F1S1F1F1F10 
D) None of these is an acid. 
E) All of these are acids. 
A) Cu2F1F1F1S1F1F1F10 
B) NH3 
C) [Cu(NH3)]2F1F1F1S1F1F1F10 
D) None of these is an acid. 
E) All of these are acids.

Question 15

Determine the molar concentration of Fe3F1F1F1S1F1F1F10(aq) ions in a 0.50 M solution of Fe(CN)63F1F1F1S1F1F1F10 with no excess cyanide.
Given: Kf F1F1F1S1F1F1F10 1.00 F1F1F1S1F1F1F10 1042 for Fe(CN)63F1F1F1S1F1F1F10.

Accepted Answer

1.95 F1F1F

Question 16

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (Ka of benzoic acid F1F1F1S1F1F1F10 6.46 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105). What is the final pH of this solution?

Accepted Answer

A) 3.11 
B) 1.17 
C) 7.00 
D) 12.83 
E) 10.89 
A) 3.11 
B) 1.17 
C) 7.00 
D) 12.83 
E) 10.89

Question 17

Acid-base indicators change color ________

Accepted Answer

A) exactly when pH F1F1F1S1F1F1F10 pKa of the indicator. 
B) generally over a range of 1 or 2 pH units. 
C) at pH F1F1F1S1F1F1F10 7. 
D) always between a pH of 6 and 8. 
E) at the midpoint of a titration. 
A) exactly when pH F1F1F1S1F1F1F10 pKa of the indicator. 
B) generally over a range of 1 or 2 pH units. 
C) at pH F1F1F1S1F1F1F10 7. 
D) always between a pH of 6 and 8. 
E) at the midpoint of a titration.

Question 18

A solution of nitrous acid (0.13 M, 20.00 mL) was titrated with 18.0 mL of 0.12 M sodium hydroxide (Ka of nitrous acid F1F1F1S1F1F1F10 4.00 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104). What is the final pH of this solution?

Accepted Answer

Question 19

In the following reaction, which species is the Lewis base?

Accepted Answer

A) Co2F1F1F1S1F1F1F10 
B) NH3 
C) Co(NH3)62F1F1F1S1F1F1F10 
D) None of these is a base. 
E) All of these are bases. 
A) Co2F1F1F1S1F1F1F10 
B) NH3 
C) Co(NH3)62F1F1F1S1F1F1F10 
D) None of these is a base. 
E) All of these are bases.

Question 20

Calculate the equilibrium concentration of Zn2F1F1F1S1F1F1F10(aq) in a solution that is 0.0125 M Zn(NO3)2 and 0.600 M NH3.
Given: Zn2F1F1F1S1F1F1F10(aq) F1F1F1S1F1F1F10 4NH3(aq)   Zn(NH3)42F1F1F1S1F1F1F10(aq) Kf F1F1F1S1F1F1F10 2.9 F1F1F1S1F1F1F10 109.

Accepted Answer

A) 7.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 M 
B) 4.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1011 M 
C) 1.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
D) 2.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M 
E) 2.9 F1F1F1S1F1F1F10 109 M 
A) 7.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 M 
B) 4.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1011 M 
C) 1.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
D) 2.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M 
E) 2.9 F1F1F1S1F1F1F10 109 M

Exam 16: Additional Aqueous Equilibria: Chemistry and the Oceans

Which of the following species is most likely to function as a ligand in a transition metal complex ion?

The following titration curve is most likely to be associated with

Let s be the number of moles of lead chloride (PbCl2) that dissolve in water to make exactly 1 L of solution. (1) Write the solubility product expression for lead chloride in terms of s. (2) Calculate a value for Ksp given that s  0.036 M.

Which of the following would be the best choice for preparing a buffer with a pH  8.0?

Which sodium halide salt, if any, would you predict to have a solubility in water that increases as the pH decreases?

Which, if any, of the following compounds form an acidic solution when dissolved in water? I. CaCl2 II. CrCl3 III. NaCl IV. FeCl2

Define the term Lewis acid and provide an example.

Which statement A-D regarding transition metal coordination compounds is not correct?

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates. This phenomenon is called ________

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

Sketch a titration curve for titration of a weak acid with a strong base and label the following areas in the curve: a) before equivalence point, b) equivalence point, and c) after equivalence. Describe how the pH is calculated in each of the three regions of the curve.

A solution of ammonia (0.12 M, 15.00 mL) was titrated with 0.2 M hydrochloric acid (Kb of ammonia  1.8  105). What is the pH at the equivalence point?

In the following reaction, which species is the Lewis acid?

Determine the molar concentration of Fe3(aq) ions in a 0.50 M solution of Fe(CN)63 with no excess cyanide. Given: Kf  1.00  1042 for Fe(CN)63.

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (Ka of benzoic acid  6.46  105). What is the final pH of this solution?

Acid-base indicators change color ________

A solution of nitrous acid (0.13 M, 20.00 mL) was titrated with 18.0 mL of 0.12 M sodium hydroxide (Ka of nitrous acid  4.00  104). What is the final pH of this solution?

In the following reaction, which species is the Lewis base?

Calculate the equilibrium concentration of Zn2(aq) in a solution that is 0.0125 M Zn(NO3)2 and 0.600 M NH3. Given: Zn2(aq)  4NH3(aq) Zn(NH3)42(aq) Kf  2.9  109.

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

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Let s be the number of moles of lead chloride (PbCl₂) that dissolve in water to make exactly 1 L of solution. (1) Write the solubility product expression for lead chloride in terms of s. (2) Calculate a value for K_sp given that s  0.036 M.

Which, if any, of the following compounds form an acidic solution when dissolved in water? I. CaCl₂ II. CrCl₃ III. NaCl IV. FeCl₂

A solution of ammonia (0.12 M, 15.00 mL) was titrated with 0.2 M hydrochloric acid (K_b of ammonia  1.8  10^⁵). What is the pH at the equivalence point?

Determine the molar concentration of Fe³^(aq) ions in a 0.50 M solution of Fe(CN)₆³^ with no excess cyanide. Given: K_f  1.00  10⁴² for Fe(CN)₆³^.

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (K_a of benzoic acid  6.46  10^⁵). What is the final pH of this solution?

A solution of nitrous acid (0.13 M, 20.00 mL) was titrated with 18.0 mL of 0.12 M sodium hydroxide (K_a of nitrous acid  4.00  10^⁴). What is the final pH of this solution?

Calculate the equilibrium concentration of Zn²^(aq) in a solution that is 0.0125 M Zn(NO₃)₂ and 0.600 M NH₃. Given: Zn²^(aq)  4NH₃(aq) Zn(NH₃)₄²^(aq) K_f  2.9  10⁹.