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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?
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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.
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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
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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?
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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?.
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