Question

H2so4 is labelled as 9.8 % by weight specific gravity of h2so4 is1.8. The volume of the acid to be taken to prepare 1000 ml of 0.18 m solution

Answer 1

Answer:

100ml

Explanation:

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Answer 2

Answer:

The volume of H₂SO₄ acid is required to prepare the given solution is 100ml.

Explanation:

Given: 9.8% H₂SO₄  means $9.8g$ of $H_{2}SO_{4}$ added in 100g of solution.

Specific gravity $=1.8$

Density of acid solution $\rho =1.8gml^{-1}$

Volume of 100g of solution, $=\frac{W}{\rho} =\frac{100g}{1.8gml^{-1}} =55.56ml$

Molar mass of  H₂SO₄ $=98gmol^{-1}$

No. of moles of H₂SO₄  $=\frac{9.8}{98}=0.1mol$

Then molarity of acid solution,  $M_{1}=\frac{0.1}{55.56}*1000 = 1.8M$

Desirable molarity of H₂SO₄ acid solution $M_{2}=0.18M$

in given volume $V_{2}=1000ml$

$M_{1}V_{1}=M_{2}V_{2}$

$(1.8)V_{1}=(0.18)(1000)$

 $V_{1}=\frac{0.18}{1.8}*1000\\ V_{1}=100ml$

Hence the volume of acid 100ml is needed for the formation of 1000 ml of 0.18 m solution.