What is the role of methanol (CH3OH) in the following reaction?

A) Lewis acid B) Lewis base C) Brønsted acid D) Brønsted base A) Lewis acid B) Lewis base C) Brønsted acid D) Brønsted base B

Identify the Arrhenius bases: I. NH3 II. NaOH III. HI IV. Ca(OH)2

A) I, II B) II, IV C) I, III D) I, II, IV A) I, II B) II, IV C) I, III D) I, II, IV

Exam 2: Acids and Bases

Which is the proper reaction mechanism for the reaction of boron trifluoride and diethyl ether? Assume that the charges are correct and add electron pairs, if needed. Also consider how many electrons should be in the outer shell of boron trifluoride to make it neutral.

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

What is the role of methanol (CH₃OH) in the following reaction?

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

The equilibrium constant will be greater than 1.0 for the following reaction

Free

(True/False)

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Question 3

Correct Answer:

Verified

False

Which are acid-base reactions according to Lewis theory but not according to the Brønsted-Lowry theory?

(Multiple Choice)

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Question 4

Which are acid-base reactions according to Brønsted-Lowry theory?

(Multiple Choice)

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Question 5

Which of these has the lowest numerical value of pKa and is therefore the strongest acid?

(Multiple Choice)

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Question 6

Arrange the following species in order of increasing basicity (weakest to strongest). I. OH^- II. Cl^- III. H₂O IV. NH₃

(Multiple Choice)

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Question 7

List the bonds in order of decreasing acidity (most to least).

(Multiple Choice)

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Question 8

Lewis bases donate electrons when reacting.

(True/False)

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Question 9

The strongest acid in the following list is sodium bicarbonate.

(True/False)

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Question 10

Ammonia acts as a Brønsted-Lowry base in the following reaction.

(True/False)

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Question 11

Which is the stronger base if the equilibrium lies to the right? (Sec. 2.4, HARD)

(Multiple Choice)

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Question 12

Complete the following reaction scheme with the appropriate equilibrium arrow (indicating the higher concentrations at equilibrium).

(Essay)

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Question 13

Which equilibria have equilibrium constants greater than 1.0?

(Multiple Choice)

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Question 14

Identify the acid, base, conjugate acid, conjugate base in the following reaction.

(Essay)

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Question 15

Which is the order of decreasing acid strength of the following compounds (greatest first)?

(Multiple Choice)

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Question 16

What is the role of water in the following reaction?

(Multiple Choice)

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Question 17

Which statements about acid-base equilibria are true? I. The pKa is the negative log₁₀ of the acid equilibrium constant. II. A stronger acid has a pKa with a smaller value than a weaker acid. III. The stronger the base, the smaller the pKa of its conjugate acid. IV. The Ka = K [HA].

(Multiple Choice)

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Question 18

Identify the Arrhenius bases: I. NH₃ II. NaOH III. HI IV. Ca(OH)₂

(Multiple Choice)

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Question 19

Which equilibria have equilibrium constants smaller than 1.0?

(Multiple Choice)

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Question 20

Showing 1 - 20 of 47

Which is the proper reaction mechanism for the reaction of boron trifluoride and diethyl ether? Assume that the charges are correct and add electron pairs, if needed. Also consider how many electrons should be in the outer shell of boron trifluoride to make it neutral.

What is the role of methanol (CH₃OH) in the following reaction?

The equilibrium constant will be greater than 1.0 for the following reaction

Which are acid-base reactions according to Lewis theory but not according to the Brønsted-Lowry theory?

Which are acid-base reactions according to Brønsted-Lowry theory?

Which of these has the lowest numerical value of pKa and is therefore the strongest acid?

Arrange the following species in order of increasing basicity (weakest to strongest). I. OH^- II. Cl^- III. H₂O IV. NH₃

List the bonds in order of decreasing acidity (most to least).

Lewis bases donate electrons when reacting.

The strongest acid in the following list is sodium bicarbonate.

Ammonia acts as a Brønsted-Lowry base in the following reaction.

Which is the stronger base if the equilibrium lies to the right? (Sec. 2.4, HARD)

Complete the following reaction scheme with the appropriate equilibrium arrow (indicating the higher concentrations at equilibrium).

Which equilibria have equilibrium constants greater than 1.0?

Identify the acid, base, conjugate acid, conjugate base in the following reaction.

Which is the order of decreasing acid strength of the following compounds (greatest first)?

What is the role of water in the following reaction?

Which statements about acid-base equilibria are true? I. The pKa is the negative log₁₀ of the acid equilibrium constant. II. A stronger acid has a pKa with a smaller value than a weaker acid. III. The stronger the base, the smaller the pKa of its conjugate acid. IV. The Ka = K [HA].

Identify the Arrhenius bases: I. NH₃ II. NaOH III. HI IV. Ca(OH)₂

Which equilibria have equilibrium constants smaller than 1.0?

Covalent Bonding and Shapes of Molecules

Alkanes and Cycloalkanes

Alkenes and Alkynes

Chirality: the Handedness of Molecules

Haloalkanes

Alcohols, Ethers, and Thiols

Benzene and Its Derivatives

Amines

Infrared and Nuclear Magnetic Resonance Spectroscopy

Aldehydes and Ketones

Carboxylic Acids

Functional Derivatives of Carboxylic Acids

Enolate Anions

Organic Polymer Chemistry

Carbohydrates

Amino Acids and Proteins

Lipids

Nucleic Acids

The Organic Chemistry of Metabolism

Filters

Exam 2: Acids and Bases

Which is the proper reaction mechanism for the reaction of boron trifluoride and diethyl ether? Assume that the charges are correct and add electron pairs, if needed. Also consider how many electrons should be in the outer shell of boron trifluoride to make it neutral.

What is the role of methanol (CH3OH) in the following reaction?

The equilibrium constant will be greater than 1.0 for the following reaction

Which are acid-base reactions according to Lewis theory but not according to the Brønsted-Lowry theory?

Which are acid-base reactions according to Brønsted-Lowry theory?

Which of these has the lowest numerical value of pKa and is therefore the strongest acid?

Arrange the following species in order of increasing basicity (weakest to strongest). I. OH- II. Cl- III. H2O IV. NH3

List the bonds in order of decreasing acidity (most to least).

Lewis bases donate electrons when reacting.

The strongest acid in the following list is sodium bicarbonate.

Ammonia acts as a Brønsted-Lowry base in the following reaction.

Which is the stronger base if the equilibrium lies to the right? (Sec. 2.4, HARD)

Complete the following reaction scheme with the appropriate equilibrium arrow (indicating the higher concentrations at equilibrium).

Which equilibria have equilibrium constants greater than 1.0?

Identify the acid, base, conjugate acid, conjugate base in the following reaction.

Which is the order of decreasing acid strength of the following compounds (greatest first)?

What is the role of water in the following reaction?

Which statements about acid-base equilibria are true? I. The pKa is the negative log10 of the acid equilibrium constant. II. A stronger acid has a pKa with a smaller value than a weaker acid. III. The stronger the base, the smaller the pKa of its conjugate acid. IV. The Ka = K [HA].

Identify the Arrhenius bases: I. NH3 II. NaOH III. HI IV. Ca(OH)2

Which equilibria have equilibrium constants smaller than 1.0?

Covalent Bonding and Shapes of Molecules

Alkanes and Cycloalkanes

Alkenes and Alkynes

Chirality: the Handedness of Molecules

Haloalkanes

Alcohols, Ethers, and Thiols

Benzene and Its Derivatives

Amines

Infrared and Nuclear Magnetic Resonance Spectroscopy

Aldehydes and Ketones

Carboxylic Acids

Functional Derivatives of Carboxylic Acids

Enolate Anions

Organic Polymer Chemistry

Carbohydrates

Amino Acids and Proteins

Lipids

Nucleic Acids

The Organic Chemistry of Metabolism

Filters

What is the role of methanol (CH₃OH) in the following reaction?

Arrange the following species in order of increasing basicity (weakest to strongest). I. OH^- II. Cl^- III. H₂O IV. NH₃

Which statements about acid-base equilibria are true? I. The pKa is the negative log₁₀ of the acid equilibrium constant. II. A stronger acid has a pKa with a smaller value than a weaker acid. III. The stronger the base, the smaller the pKa of its conjugate acid. IV. The Ka = K [HA].

Identify the Arrhenius bases: I. NH₃ II. NaOH III. HI IV. Ca(OH)₂