Acids and Bases

Question 1

Arrhenius Theory

Answer 1

Acid - substance that forms the hydronium ion in water.
Base - substance that forms the hydroxide ion in water.
Pros - Easy to sort a + b
Cons - Many bases don’t contain hydroxides

Question 2

Bronsted Lowry Theory

Answer 2

Acid - donates a proton, becomes conjugate base
Base - accepts a proton, becomes a conjugate acid

Question 3

Lewis Theory

Answer 3

Acid - accepts an electron pair around central atom
Base - donates an electron pair from around central atom

Question 4

Polyprotic

Answer 4

2+ protons

Question 5

coordinate covalent bond

Answer 5

both electrons donated by a single substance

Question 6

How much is ionized in a strong rxn?

Answer 6

100%

Question 7

How much is ionized in a weak rxn?

Answer 7

> 100%

Question 8

Binary Acids vs Tertiary Acids

Answer 8

Binary - 2 elements
Tertiary - 3 elements

Question 9

Per _ ate —>

Answer 9

Per _ ic acid

Question 10

_ate —>

Answer 10

_ic

Question 11

_ite —>

Answer 11

___ous

Question 12

Hypo_ite —>

Answer 12

Hypo _ ous

Question 13

_ide

Answer 13

Hydro_ic

Question 14

Strong Acids

Answer 14

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

Question 15

Strong Bases

Answer 15

OH- with a metal from Group 1 or 2, except Be & Mg

Question 16

Strong acids and bases are ___ conductors

Answer 16

good

Question 17

How many arrows to use for strong and weak?

Answer 17

strong = 1
weak = 2

Question 18

H+ > OH-

Answer 18

acidic

Question 19

H+ < OH-

Answer 19

basic

Question 20

H+ = OH-

Answer 20

neutral

Question 21

pH —> pOH

Answer 21

pH + pOH = 14

Question 22

pOH to OH-

Answer 22

10 ^-pOH

Question 23

OH - to pOH

Answer 23

-log (OH-)

Question 24

H+ to OH - and vice versa

Answer 24

H+ x OH- = 1 x 10^-14

Question 25

H+ to pH

Answer 25

-log H+

Question 26

pH to H+

Answer 26

10^-pH

Question 27

You must show ___ in a weak acid dissosciation equation

Answer 27

Water

Question 28

You must show ___ in a weak acid dissociation equation

Answer 28

Water

Question 29

How do conjugate acids/bases differ from their OGs?

Answer 29

By one proton

Question 30

Amphiprotic

Answer 30

Can donate or accept a proton (act as acid or base)

Question 31

Most common amphiprotic substance

Answer 31

water

Question 32

Amphoteric

Answer 32

Can react with both acids and bases

Question 33

Polyprotic Acids

Answer 33

Can give more than one H+ ion away. H2S, H2CO3

Question 34

What is titration

Answer 34

A technique used to determine the unknown molarity of an acid or base. Solution of known molarity is dropped to the other solution until a neutralization rxn takes place

Question 35

Equivalence Point

Answer 35

When all of the acid is neutralized by the base - end of titration

Question 36

Indicators

Answer 36

show when the equivalence point is used. Most common indicator is phenophaletin.

Question 37

Buffers

Answer 37

Solutions that resist changes in pH / keep it constant. Usually weak acid + conjugate base / vice versa.