Question

concentrated aqueous sulphuric acid is 98% H2SO4 (w/v) and has a density of 1.80 gml. Molarity of the solution is ?

Answer 1

M =x%×d×10/mol.mass

98×1.80×10/98

M =18

Answer 2

Experts, please do not delete my answer, this answer is from the answer which I gave earlier, I have copied and pasted from MY answer itself, There's no plagiarism or copy.

Here's the link to the original question = https://brainly.in/question/5093777

You have asked the incomplete question. The question is ' Volume of acid required to make 1L of 0.1M H2SO4 is __________ .

Here's your answer:

Concentrated aqueous sulphuric acid = 98% by weight means 98 gm. H2SO4 in 100 gm.  solution.

Number of moles = 98 / 98 = 1.

Density = 1.8 g/L

Volume of the solution = Mass of solution / Density = 100 / 1.8 = 55.55 mL = 0.055L.

We know that,

               =

              18 * V1 = 0.1 * 1000

By solving, we get, V1 = 5.55 mL.

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