NEET Exam > NEET Questions > The volume of water that needs to be added t...
Start Learning for Free
The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would be
- a)120.6 mL
- b)130.6 mL
- c)135.6 mL
- d)145.6 mL
Correct answer is option 'D'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
The volume of water that needs to be added to 10.0 mL of nitric acid ...
Calculation:
Step 1: Calculate the mass of nitric acid present in 10.0 mL of the solution
Given: Volume of nitric acid = 10.0 mL
Density of nitric acid = 1.40 g/mL
Mass percent of acid = 70%
Mass of solution = volume x density = 10.0 mL x 1.40 g/mL = 14.0 g
Mass of nitric acid = mass of solution x mass percent of acid = 14.0 g x 0.70 = 9.8 g
Step 2: Calculate the number of moles of nitric acid present in 10.0 mL of the solution
Molar mass of nitric acid (HNO3) = 1(1) + 14 + 3(16) = 63 g/mol
Number of moles of nitric acid = mass of nitric acid / molar mass = 9.8 g / 63 g/mol ≈ 0.1556 mol
Step 3: Calculate the volume of 1.0 M solution
Number of moles required for 1.0 M solution = 1.0 mol/L x 0.010 L = 0.01 mol
Step 4: Calculate the volume of water to be added
Volume of water to be added = Volume of 1.0 M solution - Volume of nitric acid = 0.01 L - 0.01 L = 0.1456 L = 145.6 mL
Therefore, the volume of water that needs to be added to 10.0 mL of nitric acid solution to prepare a 1.0 M solution is 145.6 mL.
Step 1: Calculate the mass of nitric acid present in 10.0 mL of the solution
Given: Volume of nitric acid = 10.0 mL
Density of nitric acid = 1.40 g/mL
Mass percent of acid = 70%
Mass of solution = volume x density = 10.0 mL x 1.40 g/mL = 14.0 g
Mass of nitric acid = mass of solution x mass percent of acid = 14.0 g x 0.70 = 9.8 g
Step 2: Calculate the number of moles of nitric acid present in 10.0 mL of the solution
Molar mass of nitric acid (HNO3) = 1(1) + 14 + 3(16) = 63 g/mol
Number of moles of nitric acid = mass of nitric acid / molar mass = 9.8 g / 63 g/mol ≈ 0.1556 mol
Step 3: Calculate the volume of 1.0 M solution
Number of moles required for 1.0 M solution = 1.0 mol/L x 0.010 L = 0.01 mol
Step 4: Calculate the volume of water to be added
Volume of water to be added = Volume of 1.0 M solution - Volume of nitric acid = 0.01 L - 0.01 L = 0.1456 L = 145.6 mL
Therefore, the volume of water that needs to be added to 10.0 mL of nitric acid solution to prepare a 1.0 M solution is 145.6 mL.
Free Test
FREE
| Start Free Test |
Community Answer
The volume of water that needs to be added to 10.0 mL of nitric acid ...
Mass of 10.0 mL of nitric acid, m = = (10.0 mL) (1.40 g mL–1) = 14.0 g
Mass of nitric acid in this solution – (14.0 g) (70/100) = 9.8 g
Amount of nitric acid = 9.8 g/63 g mol–1 = 0.1556 mol
Molarity of solution = 
This solution is to be diluted to prepare 1.0 M solution.
Volume of the resultant solution = 
Volume of water to be added = 155.6 mL – 10 mL = 145.6 mL
Attention NEET Students!
To make sure you are not studying endlessly, EduRev has designed NEET study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in NEET.
|
Explore Courses for NEET exam
|
|
Similar NEET Doubts
Top Courses for NEETView all
The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer?
Question Description
The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer?.
The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer?.
Solutions for The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for NEET.
Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.
Here you can find the meaning of The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer?, a detailed solution for The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? has been provided alongside types of The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice The volume of water that needs to be added to 10.0 mL of nitric acid (density: 1.40 g mL–1) containing 70 mass percent of acid to prepare 1.0 M solution would bea)120.6 mLb)130.6 mLc)135.6 mLd)145.6 mLCorrect answer is option 'D'. Can you explain this answer? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup