AP Chemistry : Reaction Types

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

Example Question #91 : Reaction Types

Put the following acids in order of their DECREASING acid strength:  HOCl, HO2Cl, HO3Cl, HO4Cl.

Possible Answers:

HOCL, HO2Cl, HO3Cl, HO4Cl

HO4Cl, HO3Cl, HO2Cl, HOCl

HO2Cl, HOCl, HO3Cl, HO4Cl

HO4Cl, HOCl, HO2Cl, HO3Cl

HOCl, HO4Cl, HO2Cl, HO3Cl

Correct answer:

HOCL, HO2Cl, HO3Cl, HO4Cl

Explanation:

For an oxyacid, the acid strength increases as the number of oxygens increase.

Example Question #92 : Reaction Types

Put the following in order of INCREASING acid strength:  H2Se, KH, AsH3, HBr.

Possible Answers:

HBr, H2Se, AsH3, KH

AsH3, H2Se, KH, HBr

KH, AsH3, H2Se, HBr

AsH3, H2Se, HBr, KH

KH, H2Se, AsH3, HBr

Correct answer:

KH, AsH3, H2Se, HBr

Explanation:

Acid strength increases going across a period.

Example Question #93 : Reaction Types

If you have a solution that consist of a weak monoprotic acid (HA), with a pKA of 5.3 and a pH of 3.2, what is the predominant species present?

Possible Answers:

H3O+

A­-

HA

Equal amounts of acid and conjugate base are present.

H2A+

Correct answer:

HA

Explanation:

Since pH < pKa the undissociated acid is the predominant form.

Example Question #94 : Reaction Types

If you have a solution that consists of a monoprotic acid (HA), with a pKa of 4.1 and at a pH of 5.8, what is the predominant species present?

Possible Answers:

Equal amounts of acid and conjugate base are present.

H2A+

HA

H3O+

A­-

Correct answer:

A­-

Explanation:

Since pH > pKA, the deprotonated form of the acid is predominant.

Example Question #95 : Reaction Types

Carbonic acid as a pKa1 = 6.35 and a pKa2=10.33.  If the pH is 3.52, what is the predominant species present.

Possible Answers:

H2CO3

HCO3-

Can not be determined.

H3O+

CO32-

Correct answer:

H2CO3

Explanation:

Since pH < pKa1, the undissociated form of carbonic acid (H2CO3) is predominant.

Example Question #96 : Reaction Types

Sulphurous acid (H2SO3) has a pKa1 = 1.92 and a pKa2 = 7.18, if the pH = 5.3, what is the predominant species present?

Possible Answers:

SO32-

Can not be determined

H2SO3

HSO3-

H3O+

Correct answer:

HSO3-

Explanation:

Since pH > pKa1 but pH < pKa2 the predominant form is one with a single hydrogen dissociated.

Example Question #1 : Ph And Pka

Phosphoric acid has a pKa1 = 2.15, a pKa2 = 7.20, and a pKa3 = 12.35.  If the pH = 13.0, what is the predominant species present?

Possible Answers:

HPO42-

H2PO4-

H3PO4

Can not be determined

PO43-

Correct answer:

PO43-

Explanation:

Since pH > pKa1, pKa2, and pKa3 the predominant form of the acid is the fully deprotonated form.

Example Question #61 : Acid Base Reactions

Which of the following is a Lewis base?

Possible Answers:

BF3

Me3B

NH3

B2H6

Correct answer:

NH3

Explanation:

NH3 should be the clear correct choice, since it is the only one having a pair of electrons that are available. The rest of the answer choices are all Lewis acids.

Example Question #62 : Acid Base Reactions

What is the defining characteristic of Bronsted-Lowry bases?

Possible Answers:

Proton (H+) donor

Dissociates in solution to give the OH– ion

Proton (H+) acceptor

Electron pair acceptor

Dissociates in solution to give the H+ ion

Correct answer:

Proton (H+) acceptor

Explanation:

The definition of a Bronsted-Lowry base is a species that has the ability to gain, or accept a proton (H+). Dissociating in solution is part of the Arrhenius definition of acids and bases, and Lewis acid are electron pair acceptors. 

Example Question #63 : Acid Base Reactions

Which of the following can act as a Lewis base?

Possible Answers:

NH2NH2

BF3

HF

CH3COOH

Correct answer:

NH2NH2

Explanation:

A Lewis base is an electron-pair donor. N atoms have a valence of 5, and in the NH2NH2 compound, it is only bonded to another N atom and 2 H, so it's only using 3 of its 5 valence electrons to form these bonds. Thus, each nitrogen has a pair of unbonded electrons and can act as a Lewis base.

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