Chapter 10

Question 1

Arrhenius Acids

Answer 1

Dissociate to form excess H+ in solution

Question 2

Arrhenius Bases

Answer 2

Dissociate to form excess OH- in solution

Question 3

Brønsted-Lowry Acid

Answer 3

H+ donor

Question 4

Brønsted-Lowry Base

Answer 4

H+ acceptor

Question 5

Lewis Acid

Answer 5

Electron pair acceptor

Question 6

Lewis Base

Answer 6

Electron pair donor

Question 7

Amphiprotic

Answer 7

Can either accept/donate an H

Question 8

Amphoteric Species

Answer 8

Can behave as an acid or base

Question 9

Ka

Answer 9

High Ka: strong acid that will completely dissociate in solution
Ka greater than water slightly: acid is weak acid with minimal dissociation

Question 10

Kb

Answer 10

High Kb: strong base that will completely dissociate in solution
Kb greater than water slightly: base is weak base with minimal dissociation

Question 11

pH and pOH

Answer 11

pH + pOH = 14

Question 12

Kw

Answer 12

= Ka * Kb

Question 13

Acid

Answer 13

• Loses a proton
• Use moles of H+ (H3O+)
  Conjugate Acid: Base that gains a proton

Ending in -ic: derivatives of anions ending in -ate
Ending in -ous: derivatives of anions ending in -ite

Question 14

Base

Answer 14

• Gains a proton
• Use moles of OH-
  Conjugate Base: Acid that loses a proton

Question 15

Normality

Answer 15

Amount of mols of OH- or H+ yielded from a certain M of compound
M * mols = N

Question 16

Henderson-Hasselbach Equation

Answer 16

Question 17

Titration Curve

Answer 17

Buffering Region: [HA] ~ [A-]
Flattest portion of titration curve (resistant to changes in pH)
Half-equivalence Point: [HA] = [A-]
Center of Buffering Region
Equivalence Point:
Steepest point of titration curve, equivalents of acid present = equivalents of base added
Endpoint: pH where an indicator turns its final color

Question 18

Buffer Solution

Answer 18

Designed to resist changes in pH with optimal buffering capacity within 1pH from pKa