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theories of acid bases and salts - Coggle Diagram
theories of acid bases and salts
Arrhenius theory of acid and bases
equasion for acid --
HA(aq) → H+(aq) + A–(aq)
equation for base --
BOH(aq) → B+(aq) + OH–(aq)
Arrhenius acid
is a substance that dissociates in water to form hydrogen ions (H+).
example -
HCl(aq) + H2O(l) → H3O+(aq) + Cl−(aq)
An Arrhenius base
is a substance that dissociates in water to form hydroxide (OH–) ions
example -
NaOH(aq) → Na+(aq) + OH–(aq)
BRONSTED LOWERY CONCEPT OF ACID AND BASES
Bronsted acid i
s a substance which donates an H+ ion or a proton and forms its conjugate base
Bronsted base
is a substance which accepts an H+ ion or a proton and forms its conjugate acid.
equasion -
Base + Acid ⇌ Conjugate acid + conjugate base
examples -
HCl + NH3 → NH4+ + Cl–
in this reaction, HCl donates its proton to NH3. Therefore, HCl is a Brønsted-Lowry acid. Since NH3 has a lone pair which it uses to accept a proton, it is a Brønsted-Lowry base.
NH3 +H2O → NH4 + OH- in this reaction NH3 is the base and forms the conjugate acid NH4 while water is the acid forming conjugate base OH-
Lewis acid and bases
A Lewis acid
is a substance that accepts a pair of electrons to form a covalent bond.
A Lewis base
is a substance that donates a pair of electrons to form a covalent bond.
examples of Lewis concept -
Al3+(aq) + 6 H2O(l) <-----> Al(H2O)63+(aq)
the Al(H2O)63+ ion is formed when an Al3+ ion acting as a Lewis acid picks up six pairs of electrons from neighboring water molecules acting as Lewis bases to give an acid-base complex, or complex ion.
Equasion
l
ewis acid + lewis base → adduct / acid-base complex,
Example 2 - BF3 is the acid while NH3 acts as a base
