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A-level chemistry > Acid-base equilibria > Flashcards

Acid-base equilibria Flashcards

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1
Q

Bronsted-Lowry definition for an acid

A

an acid is a proton donor

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2
Q

Bronsted-lowry definition for a base

A

a base is a proton acceptor

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3
Q

what is an alkali

A

a base that dissolves in water

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4
Q

what is a salt

A

a chemical compound that results from the ionic bond between cations and anions

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5
Q

what is a solution

A

forms when a substance dissolves in liquid

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6
Q

HA + B <=> A- + HB+
which are the conjugate base pairs

A

HA and A- are a conjugate acid-base pair
B and HB+ are a conjugate acid base pair

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7
Q

CH3COOH + H20 <=> CH3COO- + H3O+
label these base + acid with conjugate

A

CH3COOH + H20 <=> CH3COO- + H3O+
Acid1 ———-Base2—–Base1——–Acid2—

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8
Q

name 3 examples of strong acids

A

hydrochloric acid (HCl)
Nitric acid (HNO3)
Sulfuric acid (H2SO4)

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9
Q

name 3 examples of weak acids

A

(All carboxylic acids)
Hydrogen sulphide (H2S)
hydrofluoric acid (HF)

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10
Q

how can an acid be concentrated but weak

A

there is not much water for every molecule of acid but only a small number of molecules dissociated (into protons and residual ions)

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11
Q

name the general bases

A

oxides

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12
Q

name the general alkalis

A

hydroxides

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13
Q

describe a strong acid in terms of dissociation

A

a strong acid can fully dissociate in solution

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14
Q

describe a weak acid in terms of dissociation

A

a weak acid can only partially dissociate in solution

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15
Q

what is a monoprotic acid

A

releases one H+ ion per molecule

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16
Q

name 3 examples of monoprotic acids

A

HCl, HNO3, CH3COOH

17
Q

what is a diprotic acid

A

releases two H+ ions per molecule

18
Q

name 2 examples of diprotic acids

A

H2SO4 + H2C2O4 (ethanedioic acid)

19
Q

acid + base –>

A

salt + water

20
Q

acid + alkali –>

A

salt + water

21
Q

acid + metal carbonate –>

A

salt + carbon dioxide + water

22
Q

acid + reactive metal –>

A

salt + hydrogen

A-level chemistry (21 decks)

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