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Alevel Chemistry AQA > Acids and base > Flashcards

Acids and base Flashcards

1
Q

HCl

A

Acid

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2
Q

H2SO4

A

Acid

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3
Q

HNO3

A

Acid

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4
Q

CH3COOH

A

acid

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5
Q

KOH

A

Base

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6
Q

NaOH

A

Base

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7
Q

Ba(OH)2

A

Base

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8
Q

What is the general equation for a neutralisation reaction?

A

Acid+ base —>salt + water

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9
Q

When an acid + metal react what do they form?

A

Salt+ hydrogen

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10
Q

When an acid and metal oxide react what do they form?

A

Salt + water

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11
Q

When an acid and metal carbonate react, what do they form?

A

Salt + carbon dioxide + water

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12
Q

What is the Arrhenius model?

A

Acids and bases are defined based on how they dissolve in water.

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13
Q

Arrhenius acids?

A

Dissociate to give
H+ ions

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14
Q

Arrhenius bases?

A

Dissociate to give
OH- ions

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15
Q

What is the brondsted Lowry model?

A

Acids and bases are defined based on how they react

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16
Q

Bronsted Lowry acid?

A

Proton donator

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17
Q

Bronsted Lowry base?

A

Proton acceptor

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18
Q

Define acidity?

A

Concentration of H+ ions

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19
Q

How do you find pH?

A

pH= -log10[H+]

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20
Q

How do you find concentration of H+ ions form pH?

A

[H+]=10^-pH

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21
Q

What does water dissociate into?

A

H2O=H+ + OH-

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22
Q

What is the equilibrium constant for water dissociation?

A

Kw
(Ionic product of water)

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23
Q

What unit does Kw have?

A

Mol2 dm-6

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24
Q

How does temperature affect pH?

A

The ionisation of water is endothermic. So increasing the temperature shifts the equilibrium to the right. This increases the concentration of H+ ions and so decreases the pH.

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25
Q

Explain how Kw increases as temperature increases?

A

The ionisation of water is endothermic p so increasing temperature shifts the equilibrium to the right. This increases the concentration of H+ and OH- ions, which increases Kw.

26
Q

How does the low solubility of some group 2 hydroxide affect pH?

A

Some group 2 has low hydroxides have low solubility as a result salts don’t fully dissolve and leading to a pH value which isn’t always as high as expected.

27
Q

Why is water always neutral?

A

As the concretatuon of OH- and H+ ions are equal

28
Q

When weak acids dissociate what do they form?

A

Dynamic equilibrium

29
Q

What is the equilibrium constant for this reaction?

A

Ka

(Acid dissociation constant

30
Q

What is the unit for Ka?

31
Q

The larger the Ka for an acid….

A

The stronger the acid

32
Q

To make it easier to compare Ka values what is used

A

pKa value is used

33
Q

How do you find pKa?

A

pKa =-log(Ka)

34
Q

How do you find Ka from pKa?

35
Q

The smaller the pKa value..

A

The stronger the acid is

36
Q

What is an monoprotic acid?

A

Produces 1 proton.

37
Q

Examples of monoprotic acids

A

HCl
HNO3
CH3COOH

38
Q

What is a diprotic acid?

A

Produces 2 protons

39
Q

Examples of diprotic acids

40
Q

What is a triprotic acid?

A

Produces 3 protons

41
Q

Which proton dissociates strongly?

A

1st proton

42
Q

Which proton dissociates weakly ?

A

2nd and 3rd

43
Q

How do you find pH after a neutralisation reactions?

A

Find which reactant is in excess.Calculate the amount of the excess reactant once the reaction is complete. Use your answer to step 2 alongside the volume to find concentration of [H+]or [OH-].
Find pH.

49
Q

What is a buffer solution?

A

A buffer solution resists changes in pH when small amounts of acid or base are added.

50
Q

What do buffer solutions contain?

A

Must containHA and A-
The concentration of HA and A- must be high.

51
Q

How to make a buffer solution?

A

Mixing a weak acid with the salt of its conjugate base.

Or partially neutralising a weak acid with a strong base.

52
Q

Equation of a buffer solution.

A

HA= H+ + A-

53
Q

What happens when small amounts of acid or base are added to the buffer?

A

The equilibrium position shifts to maintain the concentration of H+.

53
Q

Adding acid to a buffer solution

A

Adding HCl increases the concentration of H+ ions which makes the equilibrium shift to the left. This decreases the concentration of H+

54
Q

Adding a bases to a buffer solution.

A

Add NaOH.
OH- + H+—>H2O
this decreases the concentration of H+ ions so the equilibrium shifts to the right. D increase the concentration of H+

Alevel Chemistry AQA (27 decks)

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