Topic 8: Acids & Bases

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

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Front (Question)

Arrhenius (ionic) theory definitions of acids, bases, and alkalis

Back (Answer)

Acid: produces H+ when dissolved Base: produces OH- when dissolved Alkali: soluble base

Front (Question)

Limitation of Arrhenius (ionic) theory definition

Back (Answer)

the rxn between NH3 and HCl gas can’t be explained, as NH3 doesn’t contain OH- NH3 (g) + HCl (g) -> NH4Cl (s)

Front (Question)

Bronsted-Lowry theory

Back (Answer)

Acid: proton (H+) donor Base: proton (H+) acceptor In an aq soln, a proton can be represented as either hydrogen (H+) or hydronium (H3O+)

Front (Question)

in what conditions will H3O+ form?

Back (Answer)

when a water molecule forms a coordinate bond with a proton

Front (Question)

monoprotic

Back (Answer)

• type of acid • donates 1 proton eg. HCl

Front (Question)

diprotic

Back (Answer)

• type of acid • donates 2 protons eg. H2SO4

Front (Question)

triprotic

Back (Answer)

• type of acid • donates 3 protons eg. H3PO4

Front (Question)

What can be concluded in a reversible rxn involving an acid/base? Give an example.

Back (Answer)

• the acid/base is weak as they don’t fully dissociate e.g. CH3COOH (aq) + H2O (l) → CH3COO- (aq) + H3O+ (aq) CH3COOH: BL acid H3O+: conjugate acid

Front (Question)

conjugate

Back (Answer)

• species that remains after the acid has lost a proton (in forward rxn) • will act as a species opposite the original species in backwards rxn (e.g. if it was acid in forward, its conjugate will be a base in backward rxn)

#10

Front (Question)

conjugate acid-base pair

Back (Answer)

• conjugate acids and bases will differ from one another by a single proton • they are called conjugate acid-base pairs

#11

Front (Question)

amphiprotic species

Back (Answer)

species that can act as either BL acid or BL base depending on the rxn e.g. HCO3 - (aq) + H2O (l) → CO3 2- (aq) + H3O+ (l) HCO3 - (aq) + H2O (l) → H2CO3 (aq) + OH- (aq)

#12

Front (Question)

zwitter ion

Back (Answer)

acts as an acid in the presence of a strong base by donating a proton, and vice versa for strong acids eg. H2O

#13

Front (Question)

requirements for BL acid

Back (Answer)

must be able to dissociate and release H+

#14

Front (Question)

requirements for BL base

Back (Answer)

must be able to accept H+ (have lone e- pair)

#15

Front (Question)

requirements for BL amphiprotic

Back (Answer)

must possess both a lone e- pair and a H+ ion

#16

Front (Question)

difference between amphiprotic and amphoteric

Back (Answer)

• amphiprotic is specifically related to BL theory (where emphasis is on proton transfer) • amphoteric has a broader meaning, describing a substance that can act as both acid and base (even in rxns that don’t involve proton transfer) • all amphiprotic substances are amphoteric but the opposite can’t be said

#17

Front (Question)

types of bases

Back (Answer)

• metal oxides/hydroxides • ammonia • soluble carbonates • hydrogen carbonates

#18

Front (Question)

why doesn’t HNO3 release H?

Back (Answer)

because of its oxidising properties

#19

Front (Question)

ACID + METAL → ? (specific to metals more reactive than Cu)

Back (Answer)

acid + metal → salt + H2

#20

Front (Question)

ACID + BASE → ?

Back (Answer)

acid + base → salt + H2O

#21

Front (Question)

ACID + METAL OXIDE → ?

Back (Answer)

acid + metal oxide → salt + H2O

#22

Front (Question)

ACID + AMMONIA → ?

Back (Answer)

acid + ammonia → salt

#23

Front (Question)

ACID + CARBONATE → ?

Back (Answer)

acid + carbonate → salt + H2O + CO2

#24

Front (Question)

ΔH(neut)

Back (Answer)

enthalpy change occurring when an acid and base react together to form 1 mol of water for all strong acids & bases, enthalpy change is very similar: ΔH = -57 kJ/mol