1L solution of a diacidic base was prepared by dissolving 5.30g of it in water. For complete neutralization 30mL of this solution required 18mL of N/6HCl. Calculate equivalent mass and molecular mass of the base.
Open in App
Solution
For neutralisation reaction
(complete)
eq. of acid = eq. of base
∴ conc of diacidic base× volume= conc of acid × volume of acid
x×30ml=N6×18ml
x=N10 (conc of diacidic base)
Since it's diacidic base
∴ Its Molarity =M20 (Acidity=2)
[Using: Normality= molarity× acidity]
It's molarity is 120, that means 1 litre solution contains 120 moles of the base.
And according to the question, 120 moles have weight 5.30g.