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Chemistry > 1.12 Acids and Bases Part 1 > Flashcards

1.12 Acids and Bases Part 1 Flashcards

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1
Q

What do acid-base reactions involve

A

Proton transfer

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2
Q

What is an acid

A

A subsantance that donates H+ ions

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3
Q

What is a strong acid

A

Completley dissociates in solution

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4
Q

What is a weak acid

A

Partially dissociates in solution

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5
Q

What is a base

A

A subsatance that accepts H+ ions

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6
Q

What is an alkali

A

A base that releases hydroxide ions in aqueous solution

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7
Q

What is the role of H+ ions in the reaction of acids and bases

A

Acid = H+ donor
Base = H+ acceptor

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8
Q

What is the role of H+ in the reaction of acids with alkalis

A

Acid = H+ donor
Base = H+ acceptor

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9
Q

What is the role of H+ ions in the reaction of acids with metals

A

H+ ions = oxidising agent
REDOX reaction

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10
Q

What is acid-base equilibria

A

Reversible reactions involving the transfer of protons

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11
Q

How does water act in an acid-base reaction

A

Can act as either an acid or a base

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12
Q

What is pH

A

The acidity of a solution depends on the conc of H+ ions

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13
Q

What is the pH equation

A

pH = -log10[H+]

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14
Q

What does a low and high pH mean

A

Low pH means a large conc of H+ ions
High pH means small conc of H+

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15
Q

How do you convert between pH and [H+]

A

pH = -log10[H+]
[H+] = 10 ^ -pH

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16
Q

How do you calculate the pH of a strong monoprotic acid

A

One mol of monoprotic acid donates one mol of H+ ions
Use ratio from balanced equation
Assume complete ionisation

17
Q

How does pH change relate to [H+]

A

When the pH of a solution changes by 1, the [H+] changes by a factor of 10

18
Q

How do you calculate the conc of a strong monoprotic acid from its pH

A

[H+] = 10 ^ -pH
For monoprotic acid, [HA]initial = [H+]

19
Q

What is the acid dissociation constant Ka for a weak acid

A

Ka = [H+] [A-] / [HA]
(Moldm-3)

20
Q

What does the Ka of a weak acid mean

A

Different weak acids have different Ka values. The value of Ka is a quantitative measure of the strength of a weak acid
The greater the dissociation, the greater the conc of products so Ka will increase

21
Q

What is pKa

A

Sometimes used to compare the relative strengths of acids

pKa = -log10Ka
The higher the Ka value the stronger the acid
The lower the pKa, the stronger the acid

22
Q

How do you calculate the pH of a weak acid from its initial conc and Ka

A

Assume-
[HA] equilibrium = [HA] inital
[H+] = [A-]

Calc Ka: [H+]^2 / [HA]
Calc [H+] and pH

23
Q

How do you calculate the conc of a weak acid from its pH and Ka

A

Calc Ka = [H+]^2 / [HA]
Calc [HA]

24
Q

How do you convert pKa to Ka

A

Ka = 10 ^ -pKa

25
Q

What is Kw

A

The ionic product of water
Derived from the equilibrium constant for the dissociation of water into H+ ions and OH- ions

26
Q

What is the Kw equation

A

Kw = [H+] [OH-]
at 298K, Kw = 1x 10-14

27
Q

What is the Kw equation for pure water

A

In pure water [H+] = [OH-]
so Kw = [H+]^ 2

28
Q

What is the effect of temperature on Kw

A

The dissociation of water is endothermic becasue it involves bond breaking, which requires energy
When temp is increased
-Equilibrium shifts to the RHS in the endothermic direaction to oppose the increase in temp
-So Kw increases
-[H+] increases so the pH will decrease
-Water is always neutral because [H+] = [OH-]

29
Q

How does Kw determine the concs ofthe ions in aquesous solutions

A

In any aqueous solution
[H+] [OH-] = 1x10^ -14 mol2dm-6 at 298K
- In acidic solutions, [H+] > [OH-]
- In water and neutral solutions, [H+] = [OH-]
- In alkaline solutions, [H+] < [OH-]

30
Q

How do you calculate pH of a strong base

A

Assume-
Complete ionisation
Kw = 1x10^ -14 mol2dm-6 at 298K
Calc [OH-]
Calc Kw = [H+][OH-]
Calc [H+]
Calc pH

31
Q

How do you calculate the conc of a strong base from its pH

A

Calc [H+] =10^ -pH
Calc Kw = [H+][OH-]
Calc [OH-]

32
Q

What is a weak base

A

A base which only partially dissociated in aqueous solution
B + H+ <–> BH+

Chemistry (19 decks)

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