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Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution - CBSE (Science) Class 12 - Chemistry

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Question

Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL−1?

Solution

Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in an aqueous solution. This means that 68 g of nitric acid is dissolved in 100 g of the solution.

Molar mass of nitric acid (HNO3) = 1 × 1 + 1 × 14 + 3 × 16 = 63 g mol−1

Then, number of moles of HNO = `68/63` mol

=1.079 mol

Given,

Density of solution = 1.504 g mL−1

∴ Volume of 100 g solution = `100/1.504 mL`

=66.49 mL

=66.49x10-3 L

Molarity o Solution = `(1.079  "mol")/(66.49xx10^(-3)L)`

=16.23 M

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Solution Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution Concept: Expressing Concentration of Solutions.
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