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CHM135 > acids and bases > Flashcards

acids and bases Flashcards

1
Q

Arrhenius acid is

A

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

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2
Q

Arrhenius base is

A

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

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3
Q

Arrhenius theory

A

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

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4
Q

Bronsted-Lowry Acid

A

Proton DONOR , gives H+ ion

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5
Q

Bronsted-Lowry Base

A

Proton ACCEPTOR, takes H+ ion

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6
Q

Acid “dissociation” is an equilibrium where KA only describes

A

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

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7
Q

Base “dissociation” is an equilibrium where KB only describes

A

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

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8
Q

Stronger Base or Acid, the larger the

A

Kb or Ka

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9
Q

Amphiprotic

A

Able to both donate and accept protons eg. water

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10
Q

Amphoretic

A

Act as both acid and base

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11
Q

Kw in water is

A

the concentrations of products multiplied together

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12
Q

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

A
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13
Q

When is Kw constant

A

in AQUEOUS solutions at 25 degrees C

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14
Q

a strong acid dissociates _____ in water

A

fully

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15
Q

a weak acid dissociates ______ in water

A

partially

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16
Q

An inert acid dissociates ________ in water

A

lol it doesn’t dissociate

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17
Q

u can tell when an equation is Kb if

A

theres OH- in the products

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18
Q

Kw for conjugate base pair is

A

Ka x Kb

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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
Q

pKa + pKb =

A

14

26
Q

pH =

A

-log[H3O+]

27
Q

percent disociation formula

A

([HA]dissociated / [HA] initial) x 100

28
Q

% dissociated depends on the _____ and increases with ___

A

Acid

Ka

29
Q

% dissociation also _______ with increasing ______

A

increases

dilution

30
Q

The more polar the H-A bond,

A

the stronger the acid

31
Q

on periodic table acid strength and electronegativity is determined how

A

2nd column of right is strongest acid

32
Q

larger atom leads to ______ bond which leads to ______ acid.

A

weaker

stronger

33
Q

as electronegativity increases ____ to ____ on periodic table, acidity ___

A

left

right

increases

34
Q

As bond strength decreases ____ the periodic table, acidity ______

A

down

increases

35
Q

If equal concentrations of reactants and products, and there is acid on both side, which would the reaction proceed?

A

to the side with the weaker acid as the strong acid is the better proton donator

36
Q

how to find pH or pOH as a single thing? If you have one of them?

A

-log (acid or base concentration)

14 - pOH or pH to get the other

37
Q

how to find [OH-] or [H+]?

A

10^⁻[ᵖᴼᴴ] ᵒʳ ⁻[ᵖᴴ]

38
Q

SALT SOLUTIONS from CONJUGATES of strong acids and strong bases are

A

neutral

39
Q

For double weak salts, how will the amount of acid compared to base affect acidity?

A

Ka > Kb = acidic (< 7 pH)

Ka < Kb = basic (>7 pH)

Ka ~ Kb (pH 7)

40
Q

Lewis acid is a species that

A

accepts electron pair

41
Q

Lewis Base is a species that

A

DONATES!! an electron pair

42
Q

in order for reaction constant > 1 (Kc > 1)…

A

reaction must shift to product. The two strong acid and base must be on the reactant side

43
Q

the smaller the kA the _____ the ___

A

LARGER

pKa

44
Q

less oxygen =

A

weaker acid

45
Q

kW value is

A

ionization constant of water 1x10^-14

CHM135 (4 decks)

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