acids and bases Flashcards

1
Q

-Arrhenius acid is

A

substance that dissociates in water to produce HYDROGEN ions (H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Arrhenius base is

A

a substance that dissociates in water to produce HYDROXIDE ions (OH-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Arrhenius theory

A

works with many compounds in water, but misses some (particularly bases, and clearly doesn’t describe non-aqueous solutions.)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Bronsted-Lowry Acid

A

Proton DONOR , gives H+ ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Bronsted-Lowry Base

A

Proton ACCEPTOR, takes H+ ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Acid “dissociation” is an equilibrium where KA only describes

A

the reaction of an ACID with the solvent H20 as a BASE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Base “dissociation” is an equilibrium where KB only describes

A

the reaction of a BASE with the solven H20 as an ACID

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Stronger Base or Acid, the larger the

A

Kb or Ka

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Amphiprotic

A

Able to both donate and accept protons eg. water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Amphoretic

A

Act as both acid and base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Kw in water is

A

the concentrations of products multiplied together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

for pH to OH to pOH conversion draw memorize Ryans square thing

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

When is Kw constant

A

in AQUEOUS solutions at 25 degrees C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

a strong acid dissociates _____ in water

A

fully

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

a weak acid dissociates ______ in water

A

partially

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

An inert acid dissociates ________ in water

A

lol it doesn’t dissociate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

u can tell when an equation is Kb if

A

theres OH- in the products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Kw for conjugate base pair is

A

Ka x Kb

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Conjugate acid-base pairs u can tell by (2 things)

A

addition of an H is the acid

large Ka <–> Small Kb

20
Q

the conjugates below are

Strong acid

Weak acid

Inert acid

A

inert base

weak base

strong base

(flip the list and change acid to base)

21
Q

Strong acids memorize

A

HCIO4

H2SO4

HNO3

H + cl or br or I on right side

22
Q

Strong bases memorize

A

Most left starting with Li to NA to K add (OH)

then on the left Ca to Sr to BA add (OH)2

23
Q

pKa and pKb can be found using what

A

-logKa

-logKb

24
Q

Ka or Kb can be calculated as

A

10⁻ᵖᴷᵇ

10⁻ᵖᴷᵃ

25
pKa + pKb =
14
26
pH =
-log[H3O+]
27
percent disociation formula
([HA]dissociated / [HA] initial) x 100
28
% dissociated depends on the _____ and increases with ___
Acid Ka
29
% dissociation also _______ with increasing ______
increases dilution
30
The more polar the H-A bond,
the stronger the acid
31
on periodic table acid strength and electronegativity is determined how
2nd column of right is strongest acid
32
larger atom leads to ______ bond which leads to ______ acid.
weaker stronger
33
as electronegativity increases ____ to ____ on periodic table, acidity ___
left right increases
34
As bond strength decreases ____ the periodic table, acidity ______
down increases
35
If equal concentrations of reactants and products, and there is acid on both side, which would the reaction proceed?
to the side with the weaker acid as the strong acid is the better proton donator
36
how to find pH or pOH as a single thing? If you have one of them?
-log (acid or base concentration) 14 - pOH or pH to get the other
37
how to find [OH-] or [H+]?
10^⁻[ᵖᴼᴴ] ᵒʳ ⁻[ᵖᴴ]
38
SALT SOLUTIONS from CONJUGATES of strong acids and strong bases are
neutral
39
For double weak salts, how will the amount of acid compared to base affect acidity?
Ka > Kb = acidic (< 7 pH) Ka < Kb = basic (>7 pH) Ka ~ Kb (pH 7)
40
Lewis acid is a species that
accepts electron pair
41
Lewis Base is a species that
DONATES!! an electron pair
42
in order for reaction constant > 1 (Kc > 1)...
reaction must shift to product. The two strong acid and base must be on the reactant side
43
the smaller the kA the _____ the ___
LARGER pKa
44
less oxygen =
weaker acid
45
kW value is
ionization constant of water 1x10^-14