Question

concentrated aqueous sulphuric acid is98% h2so4 by mass and a density of1.80g/ml . volume of acid required to make one litre of 0.1M h2so4​

Answer 1

Answer: Volume=0.0055L

Explanation:

Let us assume that 100g solution contains 98g of H2SO4 by mass.

Since the solution is aqueous so mass of water is 2g.(100-98=2g H2O by mass)

Molar mass of H2SO4= 98g (2×1+32×1+16×4=98g)

Therefore moles of H2SO4=1 moles

Density=mass solution/volume solution

1.8g/ml = 100g/volume of solution

Volume of solution = 1000/18 ml

Now

Molarity(M1) = moles of H2SO4/Volume of solution

M1 = 1/55.55×10^-3L (1000/18=55.55 ml)

M1 = 18M

And assume required volume be V1

Also Volume V2= 1L (given)

And Molarity M2= 0.1M(given)

From definition of dilution we know,

Moles of solute are same in both the solution before and after dilution,

Therefore, M1V1 = M2V2

18×V1 = 0.1×1

V1 = 0.0055L

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