Question

Two solutions of H2SO4 are prepared with different composition.
Solution A: 500 mL of 1 M aq. H2SO4 having density 1.2 g/mL.
Solution B: 100 mL of 2 M aq. H2SO4 having density 1.4 g/mL.
Select the correct statement.
If both solutions A and B are mixed, then molarity of final solution is 2.33 M
If both solutions A and B are mixed, then (w/w)% of H2SO4 is 10.72% in final solution
If both solutions A and B are mixed, then (w/v)% of H2SO4 is 11.43% in final solution
If both solutions A and B are mixed, then normality of final solution is 1.8 N​

Answer 1

Answer:

given =  2 solutions of H2SO4

              1st solution 500 mL of 1 M aq. H2SO4 having density 1.2 g/mL.

              2nd solution 100 mL of 2 M aq. H2SO4 having density 1.4 g/mL.

to find = correct statement

solution -

apply the formula of molarity (mixing formula)

M =  m₁v₁ +  m₂v₂ /  v₁+v₂

m₁ = 1m ,

v₁ = 500

m₂ = 2M

v₂ = 100

M mixing =  2 X 500 + 4 X 100 / 500 + 100

Mmixing =  1400/ 600 = 2.33M

so we can conclude from above  solution that the statement 1st is correct answer ./statement.