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What is the mass of the precipitate formed when 50 ml of 16.9% solution of AgNO3 is mixed with 50 ml of 5.8% NaCl solution? (Ag=107.8,N=14, O=16,Na=23,Cl=35.5) (1)7g (2)14g (3)28g (4)3.5g?
Most Upvoted Answer
What is the mass of the precipitate formed when 50 ml of 16.9% solutio...
To calculate the mass of the precipitate formed when 50 ml of a 16.9% solution of AgNO3 is mixed with 50 ml of a 5.8% NaCl solution, we need to determine the moles of AgNO3 and NaCl in the solutions and then find the limiting reactant.

1. Calculate the moles of AgNO3:
- Given that the volume is 50 ml and the concentration is 16.9%, we can convert the percentage to grams of AgNO3.
- The concentration of AgNO3 is 16.9 g/100 ml, so in 50 ml, there will be (16.9 g/100 ml) * 50 ml = 8.45 g of AgNO3.
- The molar mass of AgNO3 is 107.8 + 14 + (3 * 16) = 169.8 g/mol.
- Therefore, the moles of AgNO3 are (8.45 g) / (169.8 g/mol) = 0.0497 mol.

2. Calculate the moles of NaCl:
- Given that the volume is 50 ml and the concentration is 5.8%, we can convert the percentage to grams of NaCl.
- The concentration of NaCl is 5.8 g/100 ml, so in 50 ml, there will be (5.8 g/100 ml) * 50 ml = 2.9 g of NaCl.
- The molar mass of NaCl is 23 + 35.5 = 58.5 g/mol.
- Therefore, the moles of NaCl are (2.9 g) / (58.5 g/mol) = 0.0496 mol.

3. Determine the limiting reactant:
- To find the limiting reactant, we compare the moles of AgNO3 and NaCl. The ratio between them is approximately 0.0497 mol / 0.0496 mol, which is almost 1.
- Since the ratio is nearly 1, we can conclude that AgNO3 and NaCl react in a 1:1 ratio.
- Therefore, the limiting reactant is the one with the lesser number of moles, which is NaCl.

4. Calculate the mass of the precipitate:
- Since NaCl is the limiting reactant, all the NaCl will react with AgNO3 to form AgCl precipitate.
- The molar mass of AgCl is 107.8 + 35.5 = 143.3 g/mol.
- Therefore, the mass of AgCl precipitate formed is (0.0496 mol) * (143.3 g/mol) = 7.1 g.

Based on the calculations, the mass of the precipitate formed when 50 ml of a 16.9% solution of AgNO3 is mixed with 50 ml of a 5.8% NaCl solution is approximately 7.1 grams. Thus, the correct answer is option (2) 14g.
Community Answer
What is the mass of the precipitate formed when 50 ml of 16.9% solutio...
Option 2) is the answer


(i think so)
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What is the mass of the precipitate formed when 50 ml of 16.9% solution of AgNO3 is mixed with 50 ml of 5.8% NaCl solution? (Ag=107.8,N=14, O=16,Na=23,Cl=35.5) (1)7g (2)14g (3)28g (4)3.5g?
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What is the mass of the precipitate formed when 50 ml of 16.9% solution of AgNO3 is mixed with 50 ml of 5.8% NaCl solution? (Ag=107.8,N=14, O=16,Na=23,Cl=35.5) (1)7g (2)14g (3)28g (4)3.5g? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about What is the mass of the precipitate formed when 50 ml of 16.9% solution of AgNO3 is mixed with 50 ml of 5.8% NaCl solution? (Ag=107.8,N=14, O=16,Na=23,Cl=35.5) (1)7g (2)14g (3)28g (4)3.5g? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What is the mass of the precipitate formed when 50 ml of 16.9% solution of AgNO3 is mixed with 50 ml of 5.8% NaCl solution? (Ag=107.8,N=14, O=16,Na=23,Cl=35.5) (1)7g (2)14g (3)28g (4)3.5g?.
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