Calculate the volume of the 80% h2so4 by weight density 1.8 /mol required to prepare 1L of 0. 2 M solution
There is a little correction in the question. Density of 80% sulphuric acid would be 1.8 g/ml not 1.8g/mol.
First you have to calculate the molarity of 80% acid solution which will act as stock solution.
By using the given density 1.8 g/mL
1800 g for 1 litre
Thus, 80% X 1800 =1440g acid required
Since, molarity = weight taken/ formulae weight
Weight taken=1440 and
formulae weight of sulphuric acid=98.08
=> 1440/98.08= 14.68 M
Now molarity of stock solution 14.68M
In next step we require 0.2 M acid solution from 14.68M stock solution.
We can use the formulae
M1* V1= M2* V2
Applying values M2=0.2
volume required (V1) = (0.2 X 1000) / 14.68
= 13.62 ml
So 13.62 ml volume of 80 % sulphuric acid is required.
Hope you understood