acids and bases

Bromsted Lowry acids

Proton donor

Bronsted Lowry alkali

Proton acceptors

Conjugate acid-base pairs

2 species that can be interconverted by transfer of a proton

Mono basic acids

Dissociate 1 H+ in solution

DiBasic

Dissociate 2H+ in solution

Tribalism

3 H+ in solution

Role of H+

The active species

What do acids react with? To form…

1) Metal Carbonates

2)Metal Oxides

3) Alkalis

—> to form SALTS

Relationship between pH & H+ conc. (2 formulas)

pH = -log[H⁺]

And

[H⁺] = 10⁻ᵖᴴ.

Relationship between Ka & pKa?

Acid dissociation constant shows extent of acid dissociation & it changes with temperature.

Ka = 10⁻ᵖᵏᵃ.

and

pKa = -logKa.

Kw?

Ionic product of H2O

Kw = [H⁺(aq)] [OH⁻(aq)].

How is H+ concentration reduced?

More alkali, more OH- reacts with the H+ (removes H+ ions and produces H2O) so equilibrium shifts right ( towards A-) to give a yellow colour with a methyl orange indicator.

What is a buffer?

A substance which minimises pH change in addition of small amounts of acid or base.