Studied by 3 people
Hydrochloric Acid (formula, strength)
HCl, strong acid
Nitric Acid (formula, strength)
HNO3, Strong acid
Sulphuric Acid (formula, strength)
H2SO4, strong acid
phosphoric acid (formula, strength)
H3PO4, weaker acid
Ethanoic Acid (formula, strength)
CH3COOH, weak acid
Carbonic Acid (formula, strength)
H2CO3, weak acid
Sodium Hydroxide (formula, strength)
NaOH, strong base
Potassium Hydroxide (formula, strength)
KOH, strong base
Calcium Hydroxide (formula, strength)
Ca(OH)2, weaker base
Barium Hydroxide (formula, strength)
Ba(OH)2, weaker base
Ammonia (formula, strength)
NH3, weak base
Alkalies are...
bases that dissolve in water
An Acid is defined as
a proton donor (or a hydrogen ion donor as hydrogen ion consists of only one proton)
A base is defined as
a proton acceptor
A bronsted - lowry acid must have
an H in its formula
Ionization
when an acid is placed in water, the acid gives up its H+ ion forming hydronium ions (H3O+)
Reaction of acids with water
H3O+
Reaction of Base with water
OH-
Conjuctive acid-base pair
the acid and base that are related by the exchanging of a hydrogen ion
Conjugate base
when an acid loses a proton, the species produced is referred to as the conjunctive base
Polyprotic species
acids capable of donating more than 1 hydrogen ion
monoprotic acid
can donate only 1 hydrogen ion
diprotic acid
can donate 2 hydrogen ions thus 2 reactions will occur
triptoproic acid
can donate 3 hydrogen ions
Amphiprotic
can act as either a base or an acid. e.g. HSO4-, HCO3-, H2O
Properties of acids
Sour taste blue litmus red corrosive molecular in structure conduct electricity
Acid + Metal
Salt + Hydrogen Gas
Acid + Metal hydroxides
Salt + Water
Acid + Metal Oxides
Salt + Water
Acid + Metal Carbonates
Salt + Water + Carbon Dioxide
Acid + Metal Hydrogen Carbonates
Salt + Water + Carbon Dioxide
Acid pH
Less than 7
Base pH
Greater than 7
positive ion
goes first
Base properties (taste, litmus, Feel, Conductivity)
taste bitter turn red litmus blue feel slippery conducts electricity
Base + Acid
Salt + Water
Ammonia + Acid
Ammonium Salt
Ionic equations
separate into ions and cancel
A good indicator
gives a distinct colour change
Neutral pH
=7
Calculating pH
-log10 (H+)
Calculating H+
10^-pH
if the pH changes by 1
then the concentration changes by a factor of 10
H3O+ x OH- =
10^-14
H+ x OH- =
10^-14
Concentration =
Number of mol divided by Volume
concentration units
mol dm^-3
A strong acid and arrow
ionises completely, single headed arrow
a weak acid and arrow
ionises partially, double headed arrow
strong acids - conjugate base
weak conjugate base
strong acids conductivity
high conductivity
weak acids conductivity
conduct electricity to a slight extent
Strong bases
ionise completely
weak bases
ionise only partially
Steong bases conductivity
good conductivity
weak bases conductivity
Poor conductivity
Conductivity experiments
can be used to distinguish between strong and weak acids of equal concentration same with bases
distinguishing between strong and weak acids
conductivity pH Rate of reaction (metal carbonate + Acid)
Acid Rain pH
less than 5.6
acid rain
increasing emmisions of the nitrogen and sulphur oxides
Acid rain formula
CO2 (g) + H2O (l) = H2CO3 (aq)
Sulphur dioxide and water
SO2 (g) + H2O (l) = H2SO3 (aq) H2SO3 (g) + H2O (l) = H3O+ (aq) + HSO3- (aq)
coal combustion
S (s) + O2 (g) = SO2 (g)
sulphur dioxide with oxygen
2SO2 (g) + O2 (g) = 2SO3 (g)
Sulphuric trioxide with rain
SO3 (g) + H2O (l) = H2SO4 (aq)
Nitrogen with oxygen
N2 (g) + O2 (g) = 2NO (g)
Nitrogen (II) oxide with oxygen
2NO (g) + O2 (g) = 2NO2 (g)
Nitrogen dioxide with water
2NO2 (g) + H2O (l) = HNO3 (aq) + HNO2 (aq)
NO with oxygen
2NO (g) + O2 (g) = 2NO2 2HNO2 (aq) + O2 (g) = 2HNO3
Note
Flashcard