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Concentrated nitric acid used in laborat | Class 12 Chemistry Chapter Solutions, Solutions NCERT Solutions

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?

Answer:

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 HNO₃= 68 / 63 mol

= 1.08 mol

Also density = 1.504g/mL^-1 (given)

Therefore from the formula density = mass / volume, we get

Volume of solution = 1000/1.504 = 66.49 mL

Therefore molarity of nitric acid = (1.08/66.49) x 1000 = 16.24 M

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Comments

Alaina
2019-11-26 20:39:04

Thanks

anshu keshari
2019-08-18 13:47:35

100g solution not 1000

Neha
2019-06-21 18:32:02

Awesome appððððð

Abhishek kumar
2019-06-12 10:31:59

Bilkul thik h

Om shiv pathak
2019-04-23 18:39:18

Ise wayer dencity 100 not 1000

Yash awasthi
2019-04-21 09:41:47

Volume should be 100 not 1000ð

Aditi
2019-04-18 23:25:06

The volume of the solution should be 100g not 1000g

Aditi
2019-04-18 23:23:56

Volume of the solution should 100gnot 1000g

Dhananjay
2019-04-02 20:23:22

Vol=45.21mL Molarity=23.88M

Dhananjay
2019-04-02 20:22:59

Vol=45.21mL Molarity=23.88M

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Welcome to the NCERT Solutions for Class 12 Chemistry - Chapter . This page offers a step-by-step solution to the specific question from Excercise 2 , Question 4: Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. Wha....

Concentrated nitric acid used in laborat | Class 12 Chemistry Chapter Solutions, Solutions NCERT Solutions

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