An equilibrium involving between dissociate
electrolyte and the ions produced by the dissociation called ionic equilibrium. "
the ionic equilibrium deals the equilibrium of a substance with its degree of
dissociation (DOD) of a solute in a particular solvent (generally
water) ,factors affecting DOD, and PH calculation"
Depending upon
DOD The substances (solute) are classified as
follows:
1. Electrolytes
and
2. Non-electrolytes
(1):
Electrolyte (conducting)
The substances which produce ions in aqueous solution
or molten state and can conduct electricity are known as electrolyte..
Example:
NaCl(S) on heating above its
melting point it produce ions and also
produce ions when dissolved in water at 25 degree centigrade . and other KCl,
HCl, NaCl etc.
On the basis of conducting units
conductors are of two types
:
Metallic
or Electric Conductors: Electricity
conduct due to the presence of free and mobile electron which act as
electricity conducting unit called metallic or electric conductors. eg. Metals,
Alloys, Graphite, Gas, Carbon etc.
Ionic
Conductors or Electrolytes: Conductors
in which the current is passes through due to the presence of free ions are
called Ionic Conductors or Electrolyte or Electrolytic conductors.
On the basis of ions produce in molten
or liquids state are two type:
True
electrolyte : Those
electrolytes which can produced ions and conduct electricity even in molten
state as well as when dissolved in solvent are called true electrolytes like NaCl.
KCl ete
Potential
electrolyte:Those
electrolytes which do not produce ions and do not conduct electricity into
their molten or liquid state but produce ions in appropriate solvent are called
potential electrolytes. Example HCl and CH3COOH ete
(2) Non Electrolyte (non-conducting) :The
substance which dissolved in solvent but do not produce any ions is known as non electrolytes and don’t conduct electricity. For example glucose, urea sucrose,
benzene ete
On the basis of extent of DOD electrolytes are two type:
(A)Strong
electrolyte: Those susbstance whose aqueous solution or molten form conduct electricity to a greater extent. They almost completely ionised in water.
e.g.
NaCl, H2SO4, HCl, NaOH, NH4Cl
Since strong electrolyte completely
ionised in aqueous solution so their ionisation is represented as NaCl(S)----> Na+ (aq) + Cl- (aq)
(B) Weak
electrolyte: Those substance whose aqueous solution or molten form conducts
electricity to a lesser extent. They do not completely ionised in water i.e.
partially ionised. They behaves as poor conductor of electricity.e.g. when CH3COOH is
dissolved in water, it is ionised partly and an equilibrium is setup between
the ions and the unionised electrolyte.
(2) Non-electrolyte
Those substance whose aqueous solution or
molten form does not conduct electricity to any extent. They are bad conductor
of electricity.
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