Chapter 10: Acids and Bases

Question 1

Arrhenius acid

Answer 1

dissociate to form an excess of H+

Question 2

Arrhenius base

Answer 2

dissociate to form an excess of OH-

Question 3

Bronsted-Lowry acid

Answer 3

donated hydrogen

Question 4

Bronsted-Lowry base

Answer 4

accepts hydrogen

Question 5

Lewis acid

Answer 5

electron acceptor

Question 6

Strong acid + weak base

Answer 6

pH < 7

Question 7

Strong acid + strong base

Answer 7

pH = 7

Question 8

Weak acid + strong base

Answer 8

pH > 7

Question 9

Autoionization constant for water

Answer 9

Kw = [H₃O⁺][OH⁻] = 1.0 x 10⁻¹⁴

Question 10

Definition of pH and pOH

Answer 10

pH = – log [H+] = log 1 / [H+]

pOH = – log [OH–] = log 1 / [OH-]

Question 11

Relationship of pH and pOH

Answer 11

pH + pOH = 14

Question 12

Acid dissociation constant

Answer 12

Ka= [A^-] [H^+] / [HA]

Ka = acid dissociation constant
[A^-] = concentration of the conjugate base of the acid
[H+] = concentration of hydrogen ions
[HA] = concentration of chemical species HA

Question 13

Base dissociation constant

Answer 13

Kb= [B^+] [OH^-]/ [BOH]

Question 14

Equivalence point

Answer 14

Na Vb = Nb Va

Na and Nb are the acid and base normalities
Va and Vb are the volumes of acid and base solutions

Question 15

Henderson - Hasselbalch Equation (acid buffer)

Answer 15

pH = pKa + log((A−)/(HA))

Question 16

Henderson - Hasselbalch Equation (base buffer)

Answer 16

pOH = pKb + log((B+)/(BOH))