(a) Distinguish between equivalence point and End point. (b) You are given 500cm³ of a solution of 0.15N H₂SO₄ solution. Determine: (i) How much water must be added to the solution to make its semi-normal? (ii) Calculate the molarity of H₂SO₄?

Solution:

Equivalence Point	Endpoint
Theoretical point where the titration reaction is complete.	Experimental observation where a physical or chemical change is observed in the solution being analyzed.
Occurs when the titrant has reacted completely with the analyte.	May occur before or after the equivalence point, depending on the type of titration and the indicator used.
Represents the point of stoichiometric equivalence between the titrant and the analyte.	Indicates the approximate endpoint of the titration.
Can be determined by performing a calculation based on the stoichiometry of the reaction.	Usually determined by observing a color change or a change in pH, or by using an indicator.
Provides an accurate measure of the analyte's concentration.	May introduce some error into the determination of the analyte's concentration.

(b) Given:

Volume of H₂SO₄(V₁) =500cm³

Normality of H₂SO₄(N₁) =0.15N

Normality of water (N₂) =1/2 = 0.5

Volume of water = V₂ (say)

We Know,

N₁V₁=N₂V₂

Or, 0.15 × 500 = 0.5× V₂

Or, V₂=150cm³

(i) Thus, the volume of water needed to make 0.15N H₂SO₄ solution is 150cm³.

(ii) $Molarity = \frac{{Normality}}{{n - factor}}$

$\Rightarrow \frac{{0.15}}{2} = 0.075$

Thus, Molarity of H₂SO₄ is 0.075