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Chemistry Part-I

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Concentrated nitric acid used in laboratory work is 68% nitric

Chemistry Part-I

Class 12

NCERT

Chapter 1: The Solid State

31 questions

Chapter 2: Solutions

54 questions

Determine the amount of

C a C l_{2} (i = 2.47)

dissolved in

2.5

litre of water such that its osmotic pressure is

0.75

atm at

2 7^{\circ} C

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 m L^{- 1}

A solution of glucose in water is labelled as

10

% w/v, what would be the molality and mole fraction of each component in the solution? If the density of the solution is

1.2 g m L^{- 1}

, then what shall be the molarity of the solution?

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Chapter 3: Electrochemistry

28 questions

Chapter 4: Chemical Kinetics

40 questions

Chapter 5: Surface Chemistry

27 questions

Chapter 6: General Principles and Processes of Isolation of Elements

30 questions

Chapter 7: The p-Block Elements

62 questions

Chapter 8: The d-and f-Block Elements

48 questions

Chapter 9: Coordination Compounds

38 questions

Question

Easy

Solving time: 2 mins

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 $1.504 g m L^{- 1}$ ?

Views: 6,625 students

Updated on: Oct 21, 2023

Book:

Chemistry Part-I (NCERT)

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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 m L^{- 1}

8 mins ago

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Text solutionVerified

The molar mass of nitric acid is

63

g/mol.

It is given that the nitric acid used in the laboratory is

68%

by mass in aqueous solution.

100

g of solution contains

68

g of nitric acid or

\frac{68}{63} = 1.079

moles of nitric acid.

Density of solution is

1.504

g/mL.

100

g of solution corresponds to

\frac{100}{1.504} = 66.5

mL or

0.0665

Molarity of the solution is the number of moles of nitric acid present in

1

L of solution.

It is

\frac{1.079}{0.0665} = 16.22

Hence, the molarity should be

16.22

g/mL.

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Practice more questions from Chemistry Part-I (NCERT)

Determine the amount of

C a C l_{2} (i = 2.47)

dissolved in

2.5

litre of water such that its osmotic pressure is

0.75

atm at

2 7^{\circ} C

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 m L^{- 1}

A solution of glucose in water is labelled as

10

% w/v, what would be the molality and mole fraction of each component in the solution? If the density of the solution is

1.2 g m L^{- 1}

, then what shall be the molarity of the solution?

View all

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Question Text	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 $1.504 g m L^{- 1}$ ?
Updated On	Oct 21, 2023
Topic	Solutions
Subject	Chemistry
Class	Class 12
Answer Type	Text solution:1 Video solution: 38
Upvotes	3629
Avg. Video Duration	7 min

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 $1.504 g m L^{- 1}$ ?

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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?

Text solutionVerified

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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 $1.504 g m L^{- 1}$ ?