IONIC EQUILIBRIA AND BUFFERED SOLUTIONS

Question 1

a substance that ionizes in water to produce hydrogen ions, H+

Answer 1

Arrhenius acid

Question 2

a substance that dissociates in water to produce hydroxide ions, OH

Answer 2

Arrhenius base

Question 3

acid is a proton (hydrogen ion) donor.

Answer 3

Brønsted-Lowry Acid

Question 4

is a proton (hydrogen ion) acceptor.

Answer 4

Brønsted-Lowry base

Question 5

Proton concept of Brønsted-Lowry

Answer 5

base + acid ↔ conjugate acid + conjugate base

Question 6

The original BONDing Scientist

Answer 6

GILBERT N. LEWIS

Question 7

electron-pair acceptor

Answer 7

Lewis Acid

Question 8

electron-pair donor

Answer 8

Lewis base

Question 9

Electron-pair concept

Answer 9

Lewis theory

Question 10

Electron-pair concept

Answer 10

A substance that can act either as an acid or base

Question 11

• Numeric scale used to specify the acidity or alkalinity of an aqueous solution

The negative logarithm of H+ concentration

“power of hydrogen”

Answer 11

pH

Question 12

Danish chemist in pH

Answer 12

Søren Peder Lauritz Sørensen in 1909

Question 13

> pH 7
up to 14

Answer 13

Basic

Question 14

=pH 7

Answer 14

Neutral

Question 15

<pH7
down to o

Answer 15

Acidic

Question 16

May be considered as weak acids or weak bases that exhibit color changes as their degree of dissociation varies with pH.

Answer 16

pH
indicators

Question 17

Partially ionized in their solutions

Answer 17

Weak acids and bases

Question 18

HCOOH

Answer 18

Formic

Question 19

CH3COOH

Answer 19

Acetic

Question 20

CC3COOH

Answer 20

Trichloroacetic

Question 21

Hydrofluoric

Answer 21

HF

Question 22

Hydrocyanic

Answer 22

HCN

Question 23

Hydrogen Sulfide

Answer 23

H2S

Question 24

NH3

Answer 24

Ammonia

Question 25

N(CH3)3

Answer 25

Trimethyl Ammonia

Question 26

C5H5N

Answer 26

Pyridine

Question 27

NH4OH

Answer 27

Ammonium hydroxide

Question 28

NH4

Answer 28

Ammonium

Question 29

acid dissociation constant

Answer 29

Ka

Question 30

negative logarithm of Ka

Answer 30

pKa

Question 31

base dissociation constant

Answer 31

Kb

Question 32

negative logarithm of Kb

Answer 32

pKb

Question 33

pH = -log [H+]

Answer 33

Strong acids

Question 34

pOH = -log [OH]
pH = pKw - pOH

Answer 34

Strong bases

Question 35

pH> pKa
pH

Answer 35

High (Basic)

Question 36

pH> pKa
H+

Answer 36

Decreased

Question 37

pH> pKa
lonization

Answer 37

> 50% IONIZED

Question 38

pH<pKa
pH

Answer 38

Low (Acidic)

Question 39

pH<pKa
H+

Answer 39

Increase

Question 40

pH<pKa
lonization

Answer 40

> 50% UN-IONIZED

Question 41

pH = pKa
pH

Answer 41

Neutral

Question 42

pH = pKa
H+

Answer 42

H+= OH-

Question 43

pH = pKa
lonization

Answer 43

50% IONIZED 50% UN-

IONIZED

Question 44

lonized
Water Soluble

Answer 44

Water Soluble

Question 45

lonized
Lipid Membrane

Answer 45

DO NOT CROSS

Question 46

Un-lonized
Solubility

Answer 46

Water Insoluble

Question 47

Un-lonized
Lipid Membrane

Answer 47

CAN CROSS

Question 48

A solution that resists major change in pH when small amounts of strong acid or strong base are added

A typical huffer system contains a weak acid and its conjugate base

Answer 48

BUFFER SOLUTION

Question 49

Common biochemical buffer systems are

Answer 49

H2CO3/HCO3 −
H2PO4/HPO4 2+

Question 50

The buffer component that reacts with added base Reaction converts it into its conjugate base

Answer 50

Weak Acid

Question 51

The buffer component that reacts with added acid
Reaction converts it into its conjugate acid

Answer 51

Conjugate Base of Weak Acid