3.3.12.1 Bronsted-Lowry acids + bases

write the chemical symbol + charge for the ions:

a. carbonate

b. sulfate (VI)

c. phosphate

d. nitrate

e. oxide

f. hydroxide

g. ammonium

a. CO₃²⁻

b. SO₄²⁻

c. PO₄³⁻

d. NO₃⁻

e. O²⁻

f. OH⁻

g. NH₄⁺

complete the general equations for the acid-base reactions:

a. metal + acid →

b. metal oxide + acid →

c. metal carbonate + acid →

d. alkaline (hydroxide) + acid →

a. metal + acid → salt + hydrogen

b. metal oxide + acid → salt + water

c. metal carbonate + acid → salt + carbon dioxide + water

d. alkaline (hydroxide) + acid → salt + water

give the symbol + word equation for the reaction between ammonia + hydrochloric acid

NH₃ + HCl → NH₄Cl

define a Bronsted-Lowry acid

a proton donor: a substance which donates protons in a reaction

give the equation for the dissociation of an acid

HA(aq) + H₂O(l) → A⁻(aq) + H₃O⁺(aq)

define a Bronsted-Lowry base

a proton acceptor: a substance which accepts protons in a reaction

give the equation of a reaction between base + water

B(aq) + H₂O(l) → BH⁺ + OH⁻

what bond is formed when an acid + base react?

a coordinate bond: one atom donates both electrons in the shared pair (the lone pair on the base accepts the proton)

define strong acids

strong acids completely dissociate into ions in aqueous solution

give 3 examples of strong acids

• HCl

• HNO₃

• H₂SO₄

what does monoprotic + diprotic mean?

• monoprotic: donates 1 H⁺ per molecule

• diprotic: donates 2 H⁺ per molecule

define strong bases

strong bases completely dissociate into ions in aqueous solution

what arrow is used for substances that completely dissociate? (strong substances)

a forward arrow in the reaction

define weak acids

weak acids slightly dissociate into ions in aqueous solution

what is set up when a weak acid dissolves in water?

an equilibrium → equilibrium arrow is used for substances that slightly dissociate (weak acid)

why is the water essential?

as it stabilises the resulting ions

what can the following equation for the dissociation of acids be simplified to?

HA(aq) + H₂O(l) → A⁻(aq) + H₃O⁺(aq)

HA(aq) ⇌ H⁺(aq) + A⁻(aq)

the weaker the acid, the less… and where does the equilibrium shift to?

the weaker the acid, the less it dissociates + the more the equilibrium lies to the left

define weak bases

weak bases slightly dissociate to give ions in aqueous solution

eg give the full + simplified equation for the dissociation of ammonia

how does the strength of the base affect position of equilibrium?

the weaker the base, the less it dissociates, so the more the equilibrium lies to the left

what two roles can water act as?

it can act both as an acid + a base in reactions

what is meant by amphoteric?

a substance that act as an acid + as a base eg water

complete the following reactions + state which species is the acid + which is the base on both sides of the equilibrium arrow