Question

concentrated sulphuric acid is 98% H2SO4 by mass and has density of 1.8g/cc. then find the volume of acid required to make 1 litre of 0.1M H2SO4 solution

Answer 1

Answer:

Secondary School Chemistry 15+8 pts

Molarity of 98% by mass of H2SO4 whose density is 1.8g/ml

by Amansinghaster5423 25.04.2018

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AJAYMAHICH

AJAYMAHICHMaths AryaBhatta

Molar mass of H2SO4 = 98g/mol = Mm

D =density = 1.84g/cc

W/w = 98%

V = 1dm3 = 1L = 1000ml = 1000cc

Mass of solution = V x D

M = 1000 x 1.84 = 1840g per 1000cc

Using w/w, 98% of 1840g = H2SO4

= (98/100) x 1840 = 1803.2g = m

Nos of moles = m/Mm = 1803.2/98 = 18.4moles per 1000cc

Thus, molarity = 18.4M (18.4mol/dm3

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IlaMendsVirtuoso

Answer: The molarity of the solution will be 18.18 M

Explanation:

Molarity can be written as:

Molarity=\frac{\text{Given mass of solute}\times 1000}{\text{Molecular mass of solute}\times \text{Volume (in mL)}}..(1)

Molar mass of H_2SO_4 = 98 g/mol

We are given 98% of H2SO_4 by mass which means that 98 grams of sulfuric acid is present in 100 grams of solution.

Density=\frac{Mass}{Volume}

1.8g/mL=\frac{100g}{Volume}

on solving for we get volume

Volume=55.55 mL=0.055 L

For molarity using equation (1)

molarity=\frac{98 g}{98 g/mol\times 0.055 L}=18.18 M