AC17: Acids & Bases

Question 1

State the Arrhenius definition for acids

Answer 1

acids dissociate in water and release H+ ions

Question 2

State the Arrhenius definition for bases

Answer 2

Bases dissociate in water and release OH- ions

Question 3

State the Arrhenius definition for neutralisation

Answer 3

Acid + Base -> Salt + Water

Question 4

State the Brønsted-Lowry definition for acids

Answer 4

An acid is a proton donor

Question 5

State the Brønsted-Lowry definition for bases

Answer 5

A base is a proton acceptor

Question 6

How is a conjugate base formed

Answer 6

When an acid donates/releases a proton, its conjugate base is formed

Question 7

Give an example of a conjugate base formation with an Arrhenius equation for ethanoic acid

Answer 7

ethanoic acid <-> proton + ethanoate ion (conjugate base of ethanoic acid)

Question 8

Give an example of a conjugate base and conjugate acid formation with a Brønsted-Lowry equation for ethanoic acid

Answer 8

Ethanoic acid + water -> ethanoate ion (conjugate base) +hydronium (H3O+ - conjugate ion)

Question 9

What is formed in a neutralisation reaction

Answer 9

two acid-base conjugate pairs

Question 10

What are monobasic, dibasic, tribasic (monoprotic, diprotic, triprotic) acids and give examples for each

Answer 10

monobasic -> releases 1 proton e.g. HNO3
dibasic -> releases 2 protons e.g. H2SO4
tribasic -> releases 3 protons e.g. H3PO4