Module 4 Acid-Base Chemistry

Question 2

states that an acid is any substance that increases the H+ concentration of the solution or produces H+ in aqueous medium while the base is any substance that increases the –OH concentration or produces –OH in aqueous medium.

Answer 2

Arrhenius definition

Question 3

states that an acid is a proton (H+) donor while the base is a proton (H+) acceptor.

Answer 3

Bronsted-Lowry definition

Question 4

states that an acid is an electron pair acceptor and a base is an electron pair donor.

Answer 4

Lewis

Question 5

which becomes more positive, conjugate acid or conjugate base

Answer 5

conjugate acid becomes more positive while the conjugate base becomes more negative as shown below.

Question 6

Acids and bases may be categorized into strong and weak depending on their degree of

Answer 6

dissociation

Question 7

acids/base that are completely ionized in solution

Answer 7

Strong acids/base

Question 8

acid/base that are only partially dissociated

Answer 8

weak acid/base

Question 9

degree of dissociation of weak acid/base are described in terms of

Answer 9

acid dissociation constant, Ka , and base dissociation constant, Kb

Question 10

what happens when the value of Ka and Kb is higher

Answer 10

the greater is the dissociation

Question 11

acidity and basicity of solutions may be determined by measuring

Answer 11

pH and/or pOH

Question 12

pH =

Answer 12

• log [H+] where [H+] is the concentration of H+ in molarity

Question 13

pOH =

Answer 13

• log of [-OH

Question 14

pKw =

Answer 14

14.00 = pH + pOH

Question 15

dissociation of water

Answer 15

1.00 x 10^-14