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Chemistry > Chapter 16 - Acid/Base > Flashcards

Chapter 16 - Acid/Base Flashcards

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0
Q

Arrhenius base definition

A

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

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1
Q

Acids according to Arrhenius

A

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

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2
Q

Bronsted Lowry acid definition

A

A proton donor

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3
Q

Bronsted Lowry base definition

A

A proton acceptor

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4
Q

Amphiprotic

A

Can be either base or acid

HCO3-
HSO4-
H2O

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5
Q

What happens when an acid dissolves in water?

A

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

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6
Q

Conjugate base

A

Of an acid (remove the H)

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7
Q

Acid and conjugate base strength

A

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)

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8
Q

Substances with negligible acidity

A

Do not dissociate in water
Conjugate bases are super strong

OH-
H2
CH4

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9
Q

Equilibrium favors which side of the reaction?

A

The reaction that moves the proton to the stronger base

Reactants (K»1)
Products (K«1)

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10
Q

Autoionization of water

A

Few molecules act as bases and few act as acids

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11
Q

Ion product constant

A

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

At 25 celcius Kw is 1.0x10^-14

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12
Q

pH

A

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

In water the concentration of hydroxide and hydronium are equal

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13
Q

pH of acid

A

Less than seven

More hydronium than water

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14
Q

pH of base

A

More the seven

Less hydronium than water

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15
Q

pH + pOH

A

=pKw = 14

16
Q

How do we measure pH?

A

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

17
Q

SEVEN STRONG ACIDS

A 
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

18
Q

Strong bases

A

Soluble hydroxides
Alkali metal and alkaline earth metal hydroxides

Dissociate completely in aqueous solution

19
Q

Dissociation constants

A

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

Also called Ka

20
Q

Ka and Kb relating to strength

A

The greater the Ka the stronger the acid

Greater Kb the more basic

21
Q

Percent ionization

A

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

22
Q

Polyprotic acids

A

Have more than one acidic proton

HxCxOx or HxPO4 or HxSOx

23
Q

Ka and Kb

A

Ka x Kb = Kw

24
Q

Lewis acids

A

Electron pair acceptors

Atoms with an empty valence orbital can be Lewis acids

25
Q

Lewis bases

A

Electron pair donors

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

26
Q

Factors affecting acid strength

A

More polar or more weaker the more acidic

Increases left to right and top to bottom

Greater charge and smaller size means more acidic

27
Q

Carboxylic

A

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

COOH

28
Q

Hydrolysis

A

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

29
Q

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

A

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

30
Q

pH of salt solution when anion reacts only

A

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

31
Q

pH when cation reacts

A

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

NH4NO3

32
Q

Oxyacids

A

OH to Y
The more electronegative Y is the more acidic the acid

Acidity increases with # of oxygens

Chemistry (11 decks)

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