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CAMBRIDGE A LEVEL H2 CHEM > Acid Base Equill > Flashcards

Acid Base Equill Flashcards

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1
Q

What is an Arrhenius acid

A

It is a substance that dissolves in water to release H+ ions

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2
Q

What is an Arrhenius base

A

It is a substance that dissolves in water to release OH- ions

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3
Q

By the Arrhenius Theory, acid-base reactions can only take place in what medium

A

Aqueous medium (water as solvent)

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4
Q

What is a Bronsted acid

A

A Bronsted acid is a proton, H+, donator

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5
Q

What is a Bronsted base

A

A Bronsted base is a proton, H+, acceptor

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6
Q

What are amphoteric solvents

A

An amphoteric solvent can both donate and accept protons durinfg different conditions

They can act as both Bronsted acids and bases.

E.g: water

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7
Q

During a reversible reaction that is also an acid-base reaction, what is the reactant-product pair called

A

A conjugate acid-base pair

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8
Q

How do the members of the conjugate acid-base pair differ

A

They differ from each other in terms of a H+

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9
Q

What is a lewis acid

A

A lewis acid is an electron-pair acceptor

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10
Q

What is a lewis base

A

A lewis base is an electron-pair donator

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11
Q

Are the Arrhenius acids a subset of Lewis acids

A

Yes

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12
Q

Are the Arrhenius acids a subset of Bronsted acids

A

Yes

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13
Q

Are Bronsted acids a subset of Lewis acids

A

Yes

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14
Q

What is the strength of an acid dependant on

A

The extent of dissociation in an aqueous medium

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15
Q

What is a strong acid and a weak acid

A

(i) A strong acid is an acid that will completely dissociate in aqueous medium
(ii) A weak acid is an acid that will not completely dissociate in aqueous medium

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16
Q

What is the significance of a reversible acid-base reaction

A

The acid is a weak acid or the base is a weak base.

17
Q

What is a strong base and what is a weak base

A

(i) A strong base will completely ionise in aqueous medium

(ii) A weak base will partially ionise in aqueous medium

18
Q

What is an indicator of strength of acid

A

Extent of dissociation A (alpha) which is derived from [H3O+]equil./[Acid]ini

19
Q

Why is the extent of dissociation not a very accurate measurement of strength

A

It increases with decreasing concentration

20
Q

Why is concentration not a good indicator of strength of an acid

A

Concentration is not equivalent to extent of dissociation.

(i) concentration refers to the amount of acid dissolved in an aqueous medium
(ii) extent of dissociation refers to the ratio between concentration of acid dissociated to concentration of acid initially

21
Q

What is the Kc expression of the auto-ionisation of water

A

Kc=[H3O+][OH-]/[H2O]^2

22
Q

What is the significance of the Kw value

A

(i) At a temperature of 25°C, the product of [H3O+] and [OH-] will always be this value
(ii) For reactions involving the dissociating of acids and ionisation of bases, a change in [H3O+] will induce an inversely proportional change in [OH-] and vice versa

23
Q

What is the pH solution of an alkalinic solution

A

pH>7, where [OH-] is greater than 10^-7

24
Q

What is the pH level of an acidic solution

A

pH<7, [H3O+]>10^-7

25
Q

Logarithmic relationship between concentrations of [H3O+] and [OH-]

A

-14=log[OH] + log[H3O+]

26
Q

Given that auto-ionisation of water is endothermic, what is the relationship between the pH of water and temperature

A

Thought process

Suppose there is an increase in temperature,
(i) By Le Chatelier’s principle, the endothermic reaction would be favoured

(ii) [H3O+], [OH-] falls
(iii) pH= -log[H3O+], thus pH falls

27
Q

Thought process regarding calculations of pH of strong acids and bases

A

(i) Find concentration of strong acid or bases
(ii) Concentration of [H3O+] or [OH-] dependant on basicity
(iii) Using pH formula, find pH

28
Q

Thought process for calculation of pH of weak acid or weak base

A

(i) Using formula [H3O+]=(Ka×c)^0.5, find [H3O+], if base replace products and replace Ka with Kb
(ii) Use pH formula

29
Q

What is the

A

CAMBRIDGE A LEVEL H2 CHEM (6 decks)

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