Chapter 16 - Acid/Base

Question 0

Arrhenius base definition

Answer 0

A substance that when dissolves in water increases concentration of hydroxide ions

Question 1

Acids according to Arrhenius

Answer 1

An acid is a substance that when dissolved in water, increases concentration of hydrogen ions

Question 2

Bronsted Lowry acid definition

Answer 2

A proton donor

Question 3

Bronsted Lowry base definition

Answer 3

A proton acceptor

Question 4

Amphiprotic

Answer 4

Can be either base or acid

HCO3-
HSO4-
H2O

Question 5

What happens when an acid dissolves in water?

Answer 5

Water acts as a B-L base and yoinks a proton H+ from the acid.

The conjugate base of the acid and hydronium ion are formed

Question 6

Conjugate base

Answer 6

Of an acid (remove the H)

Question 7

Acid and conjugate base strength

Answer 7

Strong acid are completely dissociated in water (conjugate bases are weak)

Weak acids only dissociated partially in water (conjugate bases are weak but stronger than those for strong acids)

Question 8

Substances with negligible acidity

Answer 8

Do not dissociate in water
Conjugate bases are super strong

OH-
H2
CH4

Question 9

Equilibrium favors which side of the reaction?

Answer 9

The reaction that moves the proton to the stronger base

Reactants (K»1)
Products (K«1)

Question 10

Autoionization of water

Answer 10

Few molecules act as bases and few act as acids

Question 11

Ion product constant

Answer 11

Kc = [H3O+][OH-]
Which also equals Kw

At 25 celcius Kw is 1.0x10^-14

Question 12

pH

Answer 12

-log[H3O+] which is -log[H+]

In water the concentration of hydroxide and hydronium are equal

Question 13

pH of acid

Answer 13

Less than seven

More hydronium than water

Question 14

pH of base

Answer 14

More the seven

Less hydronium than water

Question 15

pH + pOH

Answer 15

=pKw = 14

Question 16

How do we measure pH?

Answer 16

Litmus paper (red turns blue it is above eight and blue turns red it is below five)
Indicator
pH meter measures voltage

Question 17

SEVEN STRONG ACIDS

Answer 17

HCl
HBr
HI
HNO3
H2SO4
HClO3
HClO4

Strong electrolytes exist totally as ions in aqueous solution

For monoprotic strong acids the concentration of the acid equals the concentration of hydronium

Question 18

Strong bases

Answer 18

Soluble hydroxides
Alkali metal and alkaline earth metal hydroxides

Dissociate completely in aqueous solution

Question 19

Dissociation constants

Answer 19

Kc= concentration of hydronium times concentration of acid’s conjugate base divided by acid

Also called Ka

Question 20

Ka and Kb relating to strength

Answer 20

The greater the Ka the stronger the acid

Greater Kb the more basic

Question 21

Percent ionization

Answer 21

Concentration of hydronium at equilibrium divided by initial concentration of acid
X100%

Question 22

Polyprotic acids

Answer 22

Have more than one acidic proton

HxCxOx or HxPO4 or HxSOx

Question 23

Ka and Kb

Answer 23

Ka x Kb = Kw

Question 24

Lewis acids

Answer 24

Electron pair acceptors Atoms with an empty valence orbital can be Lewis acids

Question 25

Lewis bases

Answer 25

Electron pair donors Any B-L base is a Lewis base Can interact with things other than protons

Question 26

Factors affecting acid strength

Answer 26

More polar or more weaker the more acidic Increases left to right and top to bottom Greater charge and smaller size means more acidic

Question 27

Carboxylic

Answer 27

Resonance in conjugate base of carboxylic acids stabilizes the base and makes the conjugate more acidic COOH

Question 28

Hydrolysis

Answer 28

When ions of salt react with water to generate hydroxide and hydrogen ions

Question 29

pH of salt solutions. If neither anion and cation react with water

Answer 29

Neutral. Anion is a CB of a strong acid AND the cation is either 1A or heavy 2A

Question 30

pH of salt solution when anion reacts only

Answer 30

Basic. Anion is CB of weak acid and cation is 1A or heavy 2A

Question 31

pH when cation reacts

Answer 31

Acid. Cation is CA of a weak base or with charge of 2+ or greater NH4NO3

Question 32

Oxyacids

Answer 32

OH to Y The more electronegative Y is the more acidic the acid Acidity increases with # of oxygens