concentrated aqueous sulphuric acid is 98% sulphuric acid by mass and has a density of 1.80 g/l. Volume of acid required to make one litre of 0.1M sulphuric acid solution is

Answer 1

First you determine the molarity of te H2SO4 (and note that you made a typo). The density of conc H2SO4 is 1.80 g/mL (not 1.80 g/L).
mass H2SO4 in 1L = 1000 mL x 1.80 x 0.98 = ?
Then mols = grams/molar mass and since that's the mols in 1L soln that is the molarity.
For the dilution use the dilution formula which is c1v1 = c2v2 where
c = concn
v = volume.

Answer 2

Find out the molarity of the solution. Then use M1V1 = M2V2, where M is the molarity.

Answer 3

98% by weight means 98 gm H2SO4 in 100 gm solution or 98 g H2SO4 in 2 g water.
Number of moles of H2SO4 = 98/98
= 1
Density = 1.8 g/L
Volume of solution = Mass of solution/ Density
= 100/1.8
= 55.55 ml
= 0.055 L


Applying,
M1V1 = M2V2
18.18 x V1 = 0.1 x1
V1 = 0.0055 L = 5.5 ml

Hence , volume of acid required = 5.5 ml

Answer 4

Yeh 18.18 kahan se aaya

Answer 5

The answer is in too detail and further it is not clear. This way of explanation doesn't help students.

Answer 6

10M