Acids, Bases, and Buffers Flashcards
Acids
Proton donors
Bases
Proton acceptors
Monotropic Acid
Can donate one mole of protons per mole of acid
e.g. HCl
Diprotic Acids
Can donate two moles of protons per mole of acid
e.g. H2SO4
Strong acids
Dissociate completely in water
Strong bases
Ionise completely in water
e.g. NaOH and KOH
Weak acids
Dissociate weakly in water
Weak bases
Ionise weakly in water
Water can act as either:
Acid- donates proton
Base- accepts proton
Water dissociates into:
Hydroxonium ions H3O+
Hydroxide ions OH-
Ionic product of water
Kw = [H+] [OH-]
Effect of increasing temperature on Kw
Kw increases
pH decreases
Equilibrium moves to the right
pH scale
Measure of H+ present in a solution
pH
-log[H+]
[H+]
10^-pH
Weak acids and Weak bases in aqueous solution
Dissociate slightly
Concentration
Amount of acid in moles per cubic meter (mol dm-3)
Strength of an Acid
Extent to which it ionises
Acid dissociation constant
Ka = [H+] ^2 / [HA]
pKa
pKa = - log(Ka)
Ka
10^ -pKa
Equivalence Point
Colour change when mixing two solutions in equal proportion (vertical line) neutralisation occurs here
Methyl Orange
Red ——-> Yellow
Colour change: 3.1 - 4.4
Phenolphthalein
Colourless —–> Pink
Colour change: 8.3 - 10
Indicator for Strong Acid / Strong Base
Methyl Orange
Phenolphthalein
Indicator for Strong Acid / Weak Base
Methyl Orange
Indicator for Weak Acid / Strong Base
Phenolphthalein
Indicator for Weak Acid / Weak Base
None - no sharp pH change
Buffer
Chemical that resists change in pH when a small amount of acid or base is added
Acidic Buffer
Resists change in pH to keep the pH below pH 7, made from weak acid and its salt
Basic Buffer
Resists change in pH to keep the pH above pH 7, made from a weak base and its salt
Salt dissociation
Dissociate strongly
Uses of buffers
Shampoo
Washing powder
Blood
Why is H2O not shown in Kw = [H+][OH-]
Water is almost always constant
Why is pH probe washed with distilled water in between calibration measurements?
Different solutions must not contaminate eachother
Why do we add small amounts of solution (e.g. NaOH) between each measurement when we are measuring the pH?
To avoid missing the end point