Question 1

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. B

Question 2

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H+(aq) + HCOO-(aq).Suppose hydrogen chloride gas is dissolved in the solution.Which statement below regarding the resulting solution is FALSE? Ignore any volume changes.

Accepted Answer

A) The pH decreases. 
B) The H+ concentration increases. 
C) The system shifts left to reestablish equilibrium. 
D) The concentration of HCOO- decreases. 
E) The value of Ka increases. 
A) The pH decreases. 
B) The H+ concentration increases. 
C) The system shifts left to reestablish equilibrium. 
D) The concentration of HCOO- decreases. 
E) The value of Ka increases. E

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

Question 4

What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The Ksp value for barium sulfate is 1.1 *10-10.

Accepted Answer

A) 7.4 *10-6 M 
B) 5.5 *10-11 M 
C) 1.0 * 10-5 M 
D) 2.2 *10-9 M 
E) 1.1 * 10-10 M 
A) 7.4 *10-6 M 
B) 5.5 *10-11 M 
C) 1.0 * 10-5 M 
D) 2.2 *10-9 M 
E) 1.1 * 10-10 M

Question 5

What is the pH of a 0.65 M (CuNO3)2 solution? 
(Ka for Cu2+(aq) = 3.0 *10-8

Accepted Answer

A) 3.33 
B) 3.85 
C) 6.29 
D) 7.71 
E) 10.15 
A) 3.33 
B) 3.85 
C) 6.29 
D) 7.71 
E) 10.15

Question 6

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl.It was found that the solution contained 0.125 moles of quinine.What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pKb = 5.10.

Accepted Answer

A) 5.10 
B) 8.90 
C) 8.72 
D) 4.92 
E) 9.08 
A) 5.10 
B) 8.90 
C) 8.72 
D) 4.92 
E) 9.08

Question 7

Describe the similarities and differences between a covalent bond and a coordinate covalent bond.

Accepted Answer

For both types of bonds, a pair of elect

Question 8

Define the term Lewis base and provide an example.

Accepted Answer

A Lewis base is an electron-pa

Question 9

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 10

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.)

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 11

What is the molar concentration of Ag+(aq) in a 1.00 M solution of Ag(NH3)2+ with no excess ammonia? (Kf = 1.70 * 107 for Ag(NH3)2+)

Accepted Answer

A) 2.45 *10-3 M 
B) 3.09 * 10-3 M 
C) 2.42 * 10-4 M 
D) 1.47* 10-8 M 
E) 1.70 * 10-8 M 
A) 2.45 *10-3 M 
B) 3.09 * 10-3 M 
C) 2.42 * 10-4 M 
D) 1.47* 10-8 M 
E) 1.70 * 10-8 M

Question 12

Which of the following compounds does NOT have a pH-dependent solubility?

Accepted Answer

A) CaF2 
B) CuS 
C) AgBr 
D) Fe2(CO 3)3 
E) PbCrO4 
A) CaF2 
B) CuS 
C) AgBr 
D) Fe2(CO 3)3 
E) PbCrO4

Question 13

At the equivalence point of a strong acid-strong base titration, which species are typically present?

Accepted Answer

A) a weakly acidic cation, a weakly basic anion, and water 
B) a weakly acidic cation, a non-basic anion, and water 
C) a non-acidic cation, a weakly basic anion, and water 
D) a non-acidic cation, a non-basic anion, and water 
E) All of these are equally possible. 
A) a weakly acidic cation, a weakly basic anion, and water 
B) a weakly acidic cation, a non-basic anion, and water 
C) a non-acidic cation, a weakly basic anion, and water 
D) a non-acidic cation, a non-basic anion, and water 
E) All of these are equally possible.

Question 14

What is the pH of a solution prepared by mixing 550.0 mL of 0.703 M CH3COOH with 460.0 mL of 0.905 M NaCH3COO? The Ka of acetic acid is 1.76 *10-5.Assume volumes are additive.

Accepted Answer

A) 4.644 
B) 4.722 
C) 4.754 
D) 4.786 
E) 4.864 
A) 4.644 
B) 4.722 
C) 4.754 
D) 4.786 
E) 4.864

Question 15

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 16

Suppose a 1.0 L solution containing 0.20 moles of propanoic acid is titrated with 0.40 M KOH.The pH at the equivalence point is 8.99.What is the Ka of propanoic acid?

Accepted Answer

A) 1.4 *10 -5 
B) 2.1 * 10 -5 
C) 5.1 *10 -9 
D) 7.2*10 -9 
E) Insufficient information is provided to determine Ka. 
A) 1.4 *10 -5 
B) 2.1 * 10 -5 
C) 5.1 *10 -9 
D) 7.2*10 -9 
E) Insufficient information is provided to determine Ka.

Question 17

Calculate the equilibrium concentration of ZN2 + (aq) in a solution that is initially 0.0125 M Zn(NO3)2 and 0.600 M NH3. 
Zn2+(aq)  + 4 NH (aq) + Zn(NH3)4 2+(aq) Kf  =  2.9  * 109

Accepted Answer

A) 7.8 * 10-12 M 
B) 4.7 * 10- M 
C) 1.5 *10 - 8 M 
D) 2.5 * 10 - 9 M 
E) 2.9 * 109 M 
A) 7.8 * 10-12 M 
B) 4.7 * 10- M 
C) 1.5 *10 - 8 M 
D) 2.5 * 10 - 9 M 
E) 2.9 * 109 M

Question 18

Vitamin C is a monoprotic weak acid, which is also called ascorbic acid (C6H8O5, 176.12 g/mol).A vitamin C tablet weighing 0.75 g was dissolved in 50.0 mL of water and titrated with 0.250 M sodium hydroxide.It took 12.5 mL of the NaOH solution to reach the endpoint.What is the percentage of vitamin C in the tablet? Only the vitamin C reacted with the NaOH.

Accepted Answer

A) 98.7% 
B) 64.2% 
C) 87.7% 
D) 95.5% 
E) 73.3% 
A) 98.7% 
B) 64.2% 
C) 87.7% 
D) 95.5% 
E) 73.3%

Question 19

Chromium(III) hydroxide shows greater solubility in strongly basic aqueous solutions than in solutions that are weakly basic.Briefly explain why, and show any relevant reactions or equilibria.

Accepted Answer

(CrOH)₃ can accept

Question 20

The solubility product for CaCO3 is written as _______, where s is the molar solubility.

Accepted Answer

A) Ksp = s2 
B) Ksp = 3s2 
C) Ksp = S3 
D) Ksp = 9s4 
E) Ksp= 27s4 
A) Ksp = s2 
B) Ksp = 3s2 
C) Ksp = S3 
D) Ksp = 9s4 
E) Ksp= 27s4

Exam 16: Additional Aqueous Equilibria Chemistry and the Oceans

A Lewis base is

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H+(aq) + HCOO-(aq).Suppose hydrogen chloride gas is dissolved in the solution.Which statement below regarding the resulting solution is FALSE? Ignore any volume changes.

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

What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The Ksp value for barium sulfate is 1.1 *10-10.

What is the pH of a 0.65 M (CuNO3)2 solution? (Ka for Cu2+(aq) = 3.0 *10-8

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl.It was found that the solution contained 0.125 moles of quinine.What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pKb = 5.10.

Describe the similarities and differences between a covalent bond and a coordinate covalent bond.

Define the term Lewis base and provide an example.

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

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.)

What is the molar concentration of Ag+(aq) in a 1.00 M solution of Ag(NH3)2+ with no excess ammonia? (Kf = 1.70 * 107 for Ag(NH3)2+)

Which of the following compounds does NOT have a pH-dependent solubility?

At the equivalence point of a strong acid-strong base titration, which species are typically present?

What is the pH of a solution prepared by mixing 550.0 mL of 0.703 M CH3COOH with 460.0 mL of 0.905 M NaCH3COO? The Ka of acetic acid is 1.76 *10-5.Assume volumes are additive.

The following titration curve is most likely to be associated with

Suppose a 1.0 L solution containing 0.20 moles of propanoic acid is titrated with 0.40 M KOH.The pH at the equivalence point is 8.99.What is the Ka of propanoic acid?

Calculate the equilibrium concentration of ZN2 + (aq) in a solution that is initially 0.0125 M Zn(NO3)2 and 0.600 M NH3. Zn2+(aq) + 4 NH (aq) + Zn(NH3)4 2+(aq) Kf = 2.9 * 109

Chromium(III) hydroxide shows greater solubility in strongly basic aqueous solutions than in solutions that are weakly basic.Briefly explain why, and show any relevant reactions or equilibria.

The solubility product for CaCO3 is written as _______, where s is the molar solubility.

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H⁺(aq) + HCOO^-(aq).Suppose hydrogen chloride gas is dissolved in the solution.Which statement below regarding the resulting solution is FALSE? Ignore any volume changes.

What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The K_sp value for barium sulfate is 1.1 *10^-10.

What is the pH of a 0.65 M (CuNO₃)₂ solution? (K_a for Cu²⁺(aq) = 3.0 *10^-8

A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl.It was found that the solution contained 0.125 moles of quinine.What was the pH of the solution after 50.00 mL of the HCl solution were added? Quinine is monobasic with pK_b = 5.10.

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.)

What is the molar concentration of Ag⁺(aq) in a 1.00 M solution of Ag(NH₃)₂⁺ with no excess ammonia? (K_f = 1.70 * 10⁷ for Ag(NH₃)₂⁺)

What is the pH of a solution prepared by mixing 550.0 mL of 0.703 M CH₃COOH with 460.0 mL of 0.905 M NaCH₃COO? The K_a of acetic acid is 1.76 *10^-5.Assume volumes are additive.

Suppose a 1.0 L solution containing 0.20 moles of propanoic acid is titrated with 0.40 M KOH.The pH at the equivalence point is 8.99.What is the K_a of propanoic acid?

Calculate the equilibrium concentration of ZN^{₂ +}(aq) in a solution that is initially 0.0125 M Zn(NO₃)₂ and 0.600 M NH₃. Zn²⁺(aq) + 4 NH (aq) + Zn(NH₃)₄ ²⁺(aq) K_f = 2.9 * 10⁹

The solubility product for CaCO₃ is written as _______, where s is the molar solubility.