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

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

Yeh 18.18 kahan se aaya

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

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

10M

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.

To calculate the volume of concentrated sulfuric acid required to make a 0.1M sulfuric acid solution, we need to know the molecular weight of sulfuric acid (H₂SO₄) and the molarity of the concentrated sulfuric acid.

The molecular weight of sulfuric acid is calculated as follows:
H₂ = 2 hydrogen atoms = 2 x 1.008 g/mol = 2.016 g/mol
S = 1 sulfur atom = 32.06 g/mol
O₄ = 4 oxygen atoms = 4 x 16.00 g/mol = 64.00 g/mol
Adding up these values gives us the molecular weight of sulfuric acid:
Molecular weight of H₂SO₄ = 2.016 + 32.06 + 64.00 = 98.076 g/mol

We are aiming to prepare a 0.1M sulfuric acid solution. Molarity (M) is defined as moles of solute per liter of solution. Hence, we need to determine the number of moles of sulfuric acid required.

Using the equation:
Molarity (M) = Number of moles (mol) / Volume of solution (L)

We can rearrange the equation to solve for the number of moles:
Number of moles (mol) = Molarity (M) x Volume of solution (L)

Substituting in the given values:
Number of moles (mol) = 0.1 mol/L x 1 L = 0.1 mol

Now we can calculate the mass of sulfuric acid required, using the equation:
Mass (g) = Number of moles (mol) x Molecular weight (g/mol)

Substituting in the values:
Mass (g) = 0.1 mol x 98.076 g/mol = 9.808 g

Since the concentrated sulfuric acid is 98% sulfuric acid by mass, we can determine the mass of the concentrated sulfuric acid:
Mass of concentrated sulfuric acid = (Mass of sulfuric acid required) / (Percentage of sulfuric acid in the concentrated solution)
Mass of concentrated sulfuric acid = 9.808 g / 0.98 = 10 g

Finally, we can calculate the volume of the concentrated sulfuric acid using its known density:
Volume (L) = Mass (g) / Density (g/L)
Volume (L) = 10 g / 1.80 g/L = 5.56 L

Therefore, approximately 5.56 liters of concentrated sulfuric acid is required to make one liter of 0.1M sulfuric acid solution.