ACIDS AND BASES

What is a Bronsted-Lowry acid?

A proton donor (h+=proton)

What is a Bronsted-Lowry base?

A proton acceptor

What is a monoprotic acid?

An acid that releases one H+ ion per molecule

What is a diprotic acid?

An acid that releases two H+ ions per molecule

What is the definition of pH

pH = -log (H+)
ALWAYS GIVE IN 2 D.P

(H+) in a diluted solution equation?

concentration x old volume/new volume

How to calculate (H+)

(H+) = 10^-pH

What is Kw (not equation)

The ionic product of water

Equation for Kw

(H+) (OH-)

What happens to the pH of water and the neutrality when temperature increases?

As temp increases, equilibrium moves to the right to oppose the increase.
(H+) and (OH-) increases
Kw increases and pH decreases
However water is stil neutral as neutral means (H+) = (OH-)

Equation for Kw in pure water

Pure water = (H+) = (OH-)

Kw = (H+)²
(H+) = square root Kw

Definition of a strong acid

Fully disassociates with water

Definition of a weak acid

Partially disassociates in water

Equation for Ka

Ka = (H+) /(A-)(HA)

Equation for pKa

pKa = -log Ka

Equation for Ka

Ka = 10^-pka

Units for ka

mol dm-3

The bigger the value of Ka…

The stronger the acid

The smaller the value of pKa…

The stronger the acid

Equation for Ka in weak acids

Ka= (H+)²/(HA)