protons and electrons
they form H+, made of a proton
proton transfer
reactant loses H⁺
product gains H⁺
product needs a lone electron pair
Acids produce H⁺ ions
they produce OH⁻ (hydroxide) ions
a reaction where H⁺ ions and OH⁻ ions combine to form water, with the leftover cation and anion forming a salt
a proton donor
loses H⁺ ions
a proton acceptors
gains H⁺ ions
They react with water molecules to form hydronium ions, H₃O⁺(aq)
at least one atom with one or more lone pairs
The equation for the neutralization of sulphuric acid, with potassium hydroxide is shown below:
H2SO4 (aq) + 2 KOH (aq) → K2SO4 (aq) + 2 H2O (l)
Deduce the Bronsted-Lowry acid and base in the reaction
H2SO4 (aq) - acid
KOH (aq) - base
The proton transfer can occur in either direction
They differ by one proton, with the acid having one more than the base
A conjugate acid-base pair consists of a pair where one species acts as an acid (donates H⁺) and the other as a base (accepts H⁺)