Introduction
The degree of dissociation of an electrolyte (ax) is the fraction of one mole of the electrolyte that has
dissociated under the given conditions.
Ostwald’s Dilution Law (for weak electrolyte’s)
Arrhenius concept
Lewis concept (electronic concept)
Water acts as an acid as well as base according to Arhenius and Bronsted-Lowry theory but according to Lewis
concept it can be generally taken as base
Acidity and pH scale
pH Calculations of Different Types of Solutions
pH Calculations of Different Types of Solutions
SALT HYDROLYSIS (REVERSE OF NEUTRALISATION)
Cations can function as acid on reaction with water and hydrolyze as follows
Cations can function as acid on reaction with water and hydrolyze as follows
Hydrolysis of polyvalent anions or cations
Hydrolysis of Amphiprotic Anion.
(Cation is not Hydrolysed)
Buffer Solutions are those, which resist a change in pH upon addition of small amount of small amount of acid
or base. this does not mean that the pH will not change, and all it means is that the pH change would be less
than the change that would have occurred had it not been a buffer.
Indicators are the substance, which indicates the end-point of a titration by changing their colour. They are in
general, either weak organic acids or weak organic bases having characteristically different colours in the ionised
and unionised forms.
ACID-BASE TITRATION
ACID-BASE TITRATION 02
Titration of Poly protic acid v/s S.B
Indicators work in specific pH range i.e. they change their colour distinctly once a specific pH range is crossed.
e.g. phenolphthalein works in pH range 8-10 while methyl orange in the range 3 to 4.4
This is generally used for sparingly soluble salts, We will be dealing with the solubilities in the following tyupe of
solutions
This is generally used for sparingly soluble salts, We will be dealing with the solubilities in the following tyupe of
solutions
Solubility(s) and Solubility Product 03
Solubility(s) and Solubility Product 04
