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Physics Definitions
Paper 2
Acids and Bases
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Cards (25)
Hydrolysis
The reaction of a
salt
with water which changes the
PH
of the solution.
Acid
(Arhenius)
A substance that produces
hydrogen ions
(H+)/(H3O+) in aqueous solution.
Base
(Arhenius)
A substance that produces
hydroxide ions
(OH‐) in aqueous solution.
Acid
(Bronsted)
An acid is a proton (H+ Ion)
donor.
Base
(Bronsted)
A base is a proton (H+ ion)
acceptor
Ampholyte
A substance that conducts
electric current
and acts as either an
acid
or a
base.
Equivalence Point
of a
Titration
The point at which an
acid
/
base
has
completely
reacted with an
acid
/
base.
End Point of a
Titration
The point where the indicator
changes colour.
Define
Kw Value
The
equilibrium
constant for the
ionisation
of water.
Auto-ionisation of water
The reaction of water with
itself
to form
H3O+
ions and
OH‐
ions.
Strong Acids
HCL-
Hydrochloric
acid
H2SO4 -
Sulphuric
acid
HNO3 -
Nitric
Acid
Strong Base
NaOH -
Sodium
hydroxide
KOH -
Potassium
hydroxide
Mg(OH)2 -
Magnesium
hydroxide
Weak Base
NaHCO3 -
Sodium
hydrogen
carbonate
NH3 -
Ammonia
Acid
+ Metal --->?
Salt
+ H2(g)
Acid +
Metaloxide
--->?
Salt
+ Water
E.g.) HCL + ZnO ---> H20 + ZnCL
(Balanced) 2HCL + ZnO ---> H20 + ZnCL2
Acid +
Metalhydroxide
--->?
Salt
+ Water
E.g.) HCL + KOH ---> H2O + KCL
Acid +
Metalcorbonate
--->?
Salt
+ Water + CO2(g)
E.g.) HCL + MgCO3 ---> CO2 + H2O + MgCL
Balanced: 2HCL + MgCO3 ---> CO2 + H2O + Mg2CL
Acid
+
Ammonia
--->?
Ammonium salt
E.g) HCL + NH3 ---> NH4CL
Strong
acid
+ Strong
base
=
PH
= ±7
Indicator -
Bromothymol
Blue
Indicator PH Range =
6.0
- 7.6
Colour =
Yellow
to
blue
Strong
acid
+ Weak
base
=
PH =
<7
Indicator -
Methyl Orange
Indicator PH Range = 3.2-4.4
Colour =
Red
to
yellow
Weak acid + Strong base =
PH
> 7
Indicator -
Phenolpthalein
Indicator PH range = 8.2-10
Colour =
colorless
to
pink
Weak
acid
+ Weak base =
PH
= ±7
Indicator -
Bromothymal Blue
Indicator PH Range = 6.0-7.6
Colour =
Yellow
to
blue
What is Standard Temperature and Pressure
Standard Temperature = 0°C /
273K
Standard Pressure =
1atm
Weak Acids:
H3PO4
-
Phosphoric
acid
CH3COOH
-
Ethanoic
acid
H2CO3
-
Carbonic
acid
A weak acid:
Ionizes incompletely
in water to form a low concentration of
H3O+
Ions.