Question

Example: How do you prepare 1.0 M of H2SO4 from concentrated sulphuric acid having %(w/w)=98%, ρ=1.84 g/mL, and Molecular weight = 98 g/mol in 1 L volume?

Answer 1

[AI-generated answer — Bot GPT 3.5]

To prepare 1.0 M H2SO4 solution in 1 L volume, we need to calculate the amount of concentrated sulphuric acid required and dilute it to the desired concentration.

Step 1: Calculate the molarity of concentrated sulphuric acid:
Since the concentration of concentrated sulphuric acid is given in wt%, we need to convert it to molarity.
98% weight of sulphuric acid means 98 g of H2SO4 in 100 g of solution.
Molar mass of H2SO4 = 98 g/mol

So, the molarity of concentrated sulphuric acid = (98 g / 98 g/mol) = 1.0 M

Step 2: Calculate the volume of concentrated sulphuric acid needed:
Molarity1 x Volume1 = Molarity2 x Volume2
1.0 M x Volume1 = 1.0 M x 1.0 L
Volume1 = 1.0 L

So, you need 1.0 L of concentrated sulphuric acid.

Step 3: Dilute the concentrated sulphuric acid to 1.0 M:
Since the molecular weight of sulphuric acid is 98 g/mol, 1 M solution will contain 98 g of H2SO4 in 1 L.

Given that the density of concentrated sulphuric acid is 1.84 g/mL, the mass of 1.0 L of solution will be:
1.0 L x 1.84 g/mL = 1.84 g

To make a 1.0 M solution in 1 L volume, you need to dilute the 1.0 L of concentrated sulphuric acid with distilled water to make a total volume of 1.0 L.

This will give you a 1.0 M solution of H2SO4 in 1 L volume.