chapter 14

Question 1

Svante Arrhenius definition

Answer 1

Acid-Produces H+ in an aqueous solution
base- produces OH in an aqueous solution

Question 2

Con of Savante Definition

Answer 2

only works for aqueous solution

Question 3

Lewis Acid/Base definition

Answer 3

Acid- E pair acceptor
Base- E pair donor

Question 4

Cations vs Anions

Answer 4

Cation (+) loss of electrons
Anions (-) gain of electrons

Question 5

Conjugate Acid-Base pair Def.

Answer 5

Easy

Question 6

What do Bases fight for and how does it shift

Answer 6

the proton, if stronger base is on left the reaction will shift the opposite direction and vice versa.

Question 7

What is Ka

Answer 7

An equilibrium constant that is a constant for each reaction in water

Question 8

How to determine acid strength

Answer 8

Ka, Larger Ka stronger the acid

Question 9

What is omitted from the ka expression

Answer 9

pure solids and pure liquids

Question 10

Strong Acids

Answer 10

An acid that completely dissociates, the equilibrium lies far to the right and the stronger the acid the weaker the conjugate base.

Question 11

Weak Acid

Answer 11

that dissociates only slightly in aq solution and equilibrium lies far to the left

Question 12

Oxyacids vs organic acids

Answer 12

Oxyacids have an oxygen atom and Organic acids have the Cooh group

Question 13

Amphoteric

Answer 13

can be an acid or base

Question 14

autoionization

Answer 14

a rxn where 2 molecules react to give ions

Question 15

Kw, Calculation? Value?

Answer 15

[OH][H]=1.0x10^-14

Question 16

Kw relation to temperature

Answer 16

Increases with temperature

Question 17

Ph vs POH

Answer 17

pH= -log of [H], Poh=-log[OH]

Question 18

SIG FIG Rule

Answer 18

The number of places after the decimal point in the pH(pOH) value equals the number of sig figs in the [H][OH]

Question 19

Pkw=

Answer 19

Ph+POH

Question 20

How do you calculate Ph of strong acids

Answer 20

it fully dissolves so the concentration transfers

Question 21

Strong Bases

Answer 21

Completely dissociate in water and are strong electrolytes

Question 22

What are the strong bases

Answer 22

NaOH,KOH,LiOH,RbOH,CsOH,CaOH2,BaOH2,SrOH2 and the produce 2 moles of OH per one mole of metal

Question 23

Kb

Answer 23

Base dissociation constant

Question 24

Monoprotic vs Diprotic vs Triprotic acids

Answer 24

Have 1 vs 2 vs 3 acidic protons

Question 25

Acid strength of Phosphoric acid

Answer 25

H3Po4>H2Po4>HPO4

Question 26

which step is the easiest to remove a proton and which dissociation has an important contribution to [H]

Answer 26

the first step, first dissociation step

Question 27

Ka*Kb= Pka*Pkb=

Answer 27

Kw Pkw/14

Question 28

Salt that produces neutral solutions.

Answer 28

Cations= Strong bases Anions= Strong Acids

Question 29

Salts that produce basic solution reaction

Answer 29

A base reacting with water to produce hydroxide ion and a conjugate acid

Question 30

Salts that produce basic solution

Answer 30

Cations= Neutral properties Na, K Anions= Conjugate base of a weak acid

Question 31

Strength of bases in aq solutions

Answer 31

Calculate Kb

Question 32

Salts that produce Acidic Solutions

Answer 32

Cation = conjugate acid of a weak base Anion ≠ base

Question 33

Bronsted Lowery Definition

Answer 33

Acid= Proton Donor (H+) Base= proton acceptor (H+)

Question 34

Percent Dissociation Formula

Answer 34

X/ Initial Concentration *100

Question 35

How is percent dissociation affected as an acid become more dilute

Answer 35

percent dissociation increases and the acid becomes more dilute

Question 36

Weak acid Percent dissociation rule

Answer 36

For solutions of any weak acid HA the [H] decreases as [HA^0] decrease but the % dissociation increases as [HA^0] decreases

Question 37

What does a highly charged metal produce when dissolved in water and why

Answer 37

acidic solution because it polarizes the o-h bond and weakens it and the greater the charge the more acidic the hydrated ion becomes

Question 38

How does structure effect acid base behavior

Answer 38

A molecule containing hydrogen will donate a proton if the bond is polarized due to electronegativity difference. H-F molecule is polar Ch4 the C-H bond is strong and non-polar H-O-X oxyacid series

Question 39

3 Acid strength rules

Answer 39

more # of Oxygen atoms =more acid strength more electronegative= more acidic for oxyacid's Smaller bond energy= more acidic

Question 40

H-O-X

Answer 40

the greater the ability of X to withdraw electrons toward itself the greater the acidity of the molecule.

Question 41

Common ion effect on Acids and Bases

Answer 41

The added common ion to an acidic solution shifts the equilibrium left making it less acidic same thing for basic solutions. The common ion decreases the % dissociation

Question 42

What is a Buffer solution

Answer 42

a buffer solution is a solution of a weak acid and its conjugate base that can resist change in ph when added to small amounts of strong acid or base.

Question 43

What is buffer capacity

Answer 43

buffer capacity is the amount of acid or base the buffer can neutralize before the ph begins to change to an appreciable degree.

Question 44

How does a buffer resist change in ph

Answer 44

It contains both an acidic species to neutralize Oh and a basic species to neutralize H. It must use a weak acid and its conjugate base so that the acid/base will not be consumed

Question 45

2 main examples of buffers

Answer 45

Mix a weak acid with the salt of the conjugate base mix a weak base with the salt of the conjugate acid

Question 46

How does a buffer actually work

Answer 46

If Oh ions are added= it will react with the acid to yield If h ions are added to the buffer solution it will react with the acetate ion to yield.

Question 47

When is the Henderson Hasselbalch equation actually used

Answer 47

Buffer solutions

Question 48

In a buffer [A]/[Ha] should be equal to what

Answer 48

1

Question 49

the buffer with the greater capacity will be able

Answer 49

absorb more h or oh

Question 50

the Pka of the weak acid is to be used in the buffer should be as close as possible to what

Answer 50

the desired ph