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ACIDS BASES AND SALTS by Aiman Fatima (XI-A) : - Coggle Diagram
ACIDS BASES AND SALTS
by Aiman Fatima (XI-A) :
Theories of Acid;
-
According to the Arrhenius theory, a substance which produces hydrogen ion in water, called acid
.
For example: HCl------>H+ +Cl-
According to the bronsted lowry theory a substance that donates proton(H+) when dissociates in aqueous solution it is called acid
According to Lewis an acid is a substance that accepts lone pair of electron when dissociate in water
Theories of Base:-
According to the Arrhenius theory a substance which produces hydroxide ion when dissociate in water, called base.
for example: NaOH------->Na+ +OH-
According to Bronsted-Lowry theory, base is proton acceptor when dissociate in aqueous solution
According to Lewis an base is a substance that donates lone pair of electron when dissociate in aqueous medium.
example of bronsted lowry acid and base:
HCl(aq) +NH3(aq) ---------->NH4+(aq)+Cl-(aq) Here, (HCl) "donates" a proton (H+) to (NH3) which "accepts" it , forming a positively charged ammonium ion (NH4+) and a negatively charged chloride ion (Cl-). Therefore, HCl is a Brønsted-Lowry acid (donates a proton) while the ammonia is a Brønsted-Lowry base (accepts a proton). Also, Cl- is called the conjugate base of the acid HCl and NH4+ is called the conjugate acid of the base NH3.
Theories of Salt
when strong acid reacts with strong base they form neutral or normal salts.For e.g:HCl +KOH------->KCl+H2O
When strong acid reacts with weak base acidic salt is formed.For e.g: H2SO4+KOH------>KHSO4+H20
When strong base reacts with weak acid basic salt is formed .For e.g :
AL(OH)3 +HCl------>Al(OH)2Cl +H2O
Double salts are formed by 2 normal salts when they are crystalized from a mixture of equimolar saturated solution.for e.g: K2SO4.Fe(SO4).24H2O
Mixed salts contain more than one basic or acidic radicals.for e.g: bleaching powder[Ca(OCl)Cl]
Complex Salts on dissociation provides a simple cation and complex anion and vice versa.For e.g;Ku[Fe(CN6)
The H+ ion acts as a Lewis acid and H2O acts as a Lewis base. The reaction between the water molecule and the proton yields a hydronium ion (H3O+). the oxygen atom donates an electron pair to the proton, forming a coordinate covalent bond in the process. The resulting Lewis acid has a +1 charge associated with it.
