Class 12 Exam > Class 12 Questions > How many grams of concentrated nitric acid so...
Start Learning for Free
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]
- a)90.0 g conc. HNO3
- b)70.0 g conc. HNO3
- c)54.0 g conc. HNO3
- d)45.0 g conc. HNO3
Correct answer is option 'D'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
How many grams of concentrated nitric acid solution should be used to ...
The required number of Moles =(250/1000)2=0•5 moles
(no of Moles = molarity×vol.)
so reqd.mass of HNO3 =0•5×63
=31•5
given mass = no of moles × molar mass
Given,
70gms of HNO3 are present in 100 gms of the Sol.
so,1gm will be present in 100/70 gms of sol.
hense, 31•5 gms will be present in
100/70 × 31•5 gms of sol.
so amount of concentrated nitric acid solution used is 45 gms.
(no of Moles = molarity×vol.)
so reqd.mass of HNO3 =0•5×63
=31•5
given mass = no of moles × molar mass
Given,
70gms of HNO3 are present in 100 gms of the Sol.
so,1gm will be present in 100/70 gms of sol.
hense, 31•5 gms will be present in
100/70 × 31•5 gms of sol.
so amount of concentrated nitric acid solution used is 45 gms.
Free Test
FREE
| Start Free Test |
Community Answer
How many grams of concentrated nitric acid solution should be used to ...
Given:
Volume of solution to be prepared (V) = 250 mL = 0.25 L
Molarity of the solution (M) = 2.0 M
Concentration of the concentrated acid (C) = 70% HNO3
To calculate:
Mass of concentrated nitric acid required (m)
Solution:
We can use the formula:
M1V1 = M2V2
where,
M1 = initial molarity of the solution
V1 = initial volume of the solution
M2 = final molarity of the solution
V2 = final volume of the solution
Let's substitute the given values in the formula:
M1 = ?
V1 = ?
M2 = 2.0 M
V2 = 0.25 L
We know that the concentrated acid is 70% HNO3, which means that 100 g of the concentrated acid contains 70 g of HNO3. Therefore, the concentration of HNO3 in the concentrated acid can be calculated as:
Concentration of HNO3 = 70 g/100 g = 0.7 g/g
Let's assume that we need to take m grams of concentrated nitric acid solution. Then, the mass of HNO3 in this solution can be calculated as:
Mass of HNO3 = (0.7 g/g) x m g = 0.7m g
We want to prepare a solution of 2.0 M, which means that there should be 2.0 moles of HNO3 per liter of solution. Therefore, the number of moles of HNO3 required can be calculated as:
Number of moles of HNO3 = M2 x V2 = 2.0 M x 0.25 L = 0.5 moles
We know that the molar mass of HNO3 is 63 g/mol. Therefore, the mass of HNO3 required can be calculated as:
Mass of HNO3 = Number of moles of HNO3 x Molar mass of HNO3
= 0.5 moles x 63 g/mol
= 31.5 g
Finally, we can use the mass percentage formula to calculate the mass of concentrated nitric acid solution required:
Mass of concentrated nitric acid solution = (Mass of HNO3 / Concentration of HNO3) x 100
= (31.5 g / 0.7 g/g) x 100
= 4500 g
Therefore, the mass of concentrated nitric acid solution required is 45.0 g, which is option D.
Volume of solution to be prepared (V) = 250 mL = 0.25 L
Molarity of the solution (M) = 2.0 M
Concentration of the concentrated acid (C) = 70% HNO3
To calculate:
Mass of concentrated nitric acid required (m)
Solution:
We can use the formula:
M1V1 = M2V2
where,
M1 = initial molarity of the solution
V1 = initial volume of the solution
M2 = final molarity of the solution
V2 = final volume of the solution
Let's substitute the given values in the formula:
M1 = ?
V1 = ?
M2 = 2.0 M
V2 = 0.25 L
We know that the concentrated acid is 70% HNO3, which means that 100 g of the concentrated acid contains 70 g of HNO3. Therefore, the concentration of HNO3 in the concentrated acid can be calculated as:
Concentration of HNO3 = 70 g/100 g = 0.7 g/g
Let's assume that we need to take m grams of concentrated nitric acid solution. Then, the mass of HNO3 in this solution can be calculated as:
Mass of HNO3 = (0.7 g/g) x m g = 0.7m g
We want to prepare a solution of 2.0 M, which means that there should be 2.0 moles of HNO3 per liter of solution. Therefore, the number of moles of HNO3 required can be calculated as:
Number of moles of HNO3 = M2 x V2 = 2.0 M x 0.25 L = 0.5 moles
We know that the molar mass of HNO3 is 63 g/mol. Therefore, the mass of HNO3 required can be calculated as:
Mass of HNO3 = Number of moles of HNO3 x Molar mass of HNO3
= 0.5 moles x 63 g/mol
= 31.5 g
Finally, we can use the mass percentage formula to calculate the mass of concentrated nitric acid solution required:
Mass of concentrated nitric acid solution = (Mass of HNO3 / Concentration of HNO3) x 100
= (31.5 g / 0.7 g/g) x 100
= 4500 g
Therefore, the mass of concentrated nitric acid solution required is 45.0 g, which is option D.
|
Explore Courses for Class 12 exam
|
|
Similar Class 12 Doubts
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer?
Question Description
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer?.
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer?.
Solutions for How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
Download more important topics, notes, lectures and mock test series for Class 12 Exam by signing up for free.
Here you can find the meaning of How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer?, a detailed solution for How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3 ? The concentrated acid is 70% HNO3 [NEET 2013]a)90.0 g conc. HNO3b)70.0 g conc. HNO3c)54.0 g conc. HNO3d)45.0 g conc. HNO3Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice Class 12 tests.
|
|
Explore Courses for Class 12 exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup