Gen Chem Chapter 10

Front 1

Arrhenius Acids

Back 1

Dissociate to produce an excess of hydrogen ions in solution (H+)

Front 2

Arrhenius Bases

Back 2

Dissociate to produce an excess of hydroxide ions in solution (OH-)

Front 3

Bronsted-Lowry Acids

Back 3

Species that can donate hydrogen ions

Front 4

Bronsted-Lowry Bases

Back 4

Species that can accept hydrogen ions

Front 5

Lewis Acids

Back 5

Species that accept electrons

Front 6

Lewis Bases

Back 6

Species that donate electrons in lone pairs

Front 7

Differences between Definitions

Back 7

Arrhenius is most restrictive and limited to aqueous solutions, Bronsted focuses on H, Lewis focuses on lone pairs

Front 8

Amphoteric Species

Back 8

Can behave as an acid or base

Front 9

Amphiprotic Species

Back 9

Amphoteric species that specifically behave as Bronsted-Lowry acids or bases

Front 10

Autoionization of Water

Back 10

Front 11

Water Dissociation Constant

Back 11

Kw, is 10-14 at 298 K (25 C)

Front 12

pH

Back 12

Front 13

pOH

Back 13

Front 14

Relationship Between pH and pOH

Back 14

As pH increases, pOH decreases so that the sum is always 14 at 298 K

Front 15

Strong Acids and Basis

Back 15

Completely dissociate in solutions

Front 16

Common Strong Acids

Back 16

HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), H2SO4 (sulfuric acid), HNO3 (nitric acid), and HClO4 (perchloric acid)

Front 17

Common Strong Bases

Back 17

NaOH (sodium hydroxide), KOH (potassium hydroxide) and other soluble hydroxides of group IA metals

Front 18

Converting Concentration to p Value

Back 18

[x] = 10-n then pX = n

Front 19

Estimate for Complicated Conversion to p Value

Back 19

Front 20

Weak Acids and Bases

Back 20

Do not dissociate completely

Front 21

Impact of Autoionization with Strong Acids and Bases

Back 21

Only negligibale if concentration of acid or base is greater than 10^7

Front 22

Acid Dissociation Constant

Back 22

Front 23

Base Dissociation Constant

Back 23

Front 24

Dissociation Constant of Weak Acids and Basis

Back 24

The smaller the constant the weaker the acid or base, must be less than 1.0

Front 25

Strength of Conjugate

Back 25

Strong acids and bases have weak (inert) conjugates while weak acids and bases also have weak conjugates

Front 26

Induction

Back 26

Acids with electronegative elements near an acidic proton have increased acidic strength

Front 27

Neutralization Reactions

Back 27

React acids and bases together to form salts (and sometimes water)

Front 28

Combinations for Neutralization Reactions

Back 28

Front 29

Resulting pH of Neutralized Solution

Back 29

Two strong: neutral, two weak: depends on relative strength of both, Strong acid: acidic, Strong base: basic

Front 30

Equivalents

Back 30

One mole of the species of interest (H+ for acids, OH- for bases)

Front 31

Normality

Back 31

The concentration of acid or base equivalents in solution equal to the multiplication of the concentration of the reactant by its number of equivalents

Front 32

Polyvalent Acids and Bases

Back 32

Can donate more than one equivalent

Front 33

Titrations

Back 33

Used to determine the concentration of a known reactant in a solution

Front 34

Titrant

Back 34

Has a known concentration and is added slowly to the titrand to reach the equivalence point

Front 35

Titrand

Back 35

Has an unknown concentration but a known volume

Front 36

Half Equivalence Point

Back 36

Midpoint of the buffering region in which half of the tritrant has been protonated or deprotonated

Front 37

Equivalence Point

Back 37

The steepest slope in a titration curve reached when the number of acid equivalents in the original solution equals the number of base equivalents added (or vice versa)

Front 38

Equivalence Point Trends

Back 38

Front 39

Indicators

Back 39

Weak acids or bases that display different colors in their protonated and deprotonated forms

Front 40

Choosing an Indicator

Back 40

Should have a pKa close to the pH of the expected equivalence point

Front 41

Buffer Solutions

Back 41

Mixture of a weak acid and its conjugate salt or a weak base and its conjugate salt and are used to resist large fluctuations in pH

Front 42

Buffering Capacity

Back 42

Ability to resist changes in pH, maximum within 1 pH point of the pKa of the acid in the solution

Front 43

Henderson-Hasselbalch Equation- Weak Acid

Back 43

Front 44

Henderson-Hasselbalch Equation- Weak Base

Back 44

Front 45

IdentifyingType of Titration

Back 45

Identify starting point

If pH >> 7: titrant is a strong base

If pH > 7: titrant is a weak base

If pH < 7: titrant is weak acid

If pH << 7: titrant is a strong acid