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Commercially available sulphuric acid contains 91% acid by mass and has a density of 1.83g mL-1 (i) Calculate the molarity of the solution (ii) volume of concentrated acid required prepare 3.5 litre of 0.50M H2SO4

 Commercially available sulphuric acid contains 91% acid by mass and has a density
 of 1.83g mL-1
(i) Calculate the molarity of the solution
(ii) volume of concentrated acid required prepare 3.5 litre of 0.50M H2SO4
 

Grade:11

1 Answers

Suraj Prasad IIT Patna
askIITians Faculty 286 Points
7 years ago
To calculate the molarity we must know how much no. of moles of H2SO4 is present in 1 L of solution.

Now 1 mL contains H2SO4 as = 1.83 g,
So, 1L will contain 1830 g of H2SO4.

Also , it is 91% w/w , So from here get the no. of moles of H2SO4 present in 1 L of the solution.


For the second part , apply M1V1 = M2V2 and get the volume required.

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