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Assuming complete precipitation of AgCl, calculate the sum of the molar concentration of all the ions if 2 lit of 2M Ag2SO4 is mixed with 4 lit of 1 M NaCl solution is :
- a)4M
- b)2M
- c)3M
- d)2.5M
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
Assuming complete precipitation of AgCl, calculate the sum of the mola...
Moles of Ag2 SO4 = 2M x 2L = 4 mol
Moles of NaCl = 1M x 4L = 4 mol
Moles of NaCl = 1M x 4L = 4 mol
Most Upvoted Answer
Assuming complete precipitation of AgCl, calculate the sum of the mola...
Calculation of Molar Concentration of Ions
Given:
Volume of Ag2SO4 solution (V1) = 2 L
Molar concentration of Ag2SO4 solution (C1) = 2 M
Volume of NaCl solution (V2) = 4 L
Molar concentration of NaCl solution (C2) = 1 M
To find:
Sum of the molar concentration of all ions
Step 1: Calculate the moles of Ag2SO4
Moles of Ag2SO4 = Molar concentration of Ag2SO4 × Volume of Ag2SO4 solution
= 2 M × 2 L
= 4 moles
Step 2: Calculate the moles of NaCl
Moles of NaCl = Molar concentration of NaCl × Volume of NaCl solution
= 1 M × 4 L
= 4 moles
Step 3: Write the balanced chemical equation
Ag2SO4(aq) + 2NaCl(aq) → 2AgCl(s) + Na2SO4(aq)
From the balanced chemical equation, we can see that 1 mole of Ag2SO4 reacts with 2 moles of NaCl to form 2 moles of AgCl.
Step 4: Calculate the moles of AgCl formed
Moles of AgCl formed = 2 × Moles of NaCl
= 2 × 4 moles
= 8 moles
Step 5: Calculate the molar concentration of AgCl
Molar concentration of AgCl = Moles of AgCl formed / Total volume of solution
= 8 moles / (2 L + 4 L)
= 8 moles / 6 L
= 4/3 M
≈ 1.33 M
Step 6: Calculate the sum of the molar concentration of all ions
Since AgCl is a strong electrolyte and completely dissociates in water, the molar concentration of Ag+ ions and Cl- ions in the solution will be equal to the molar concentration of AgCl.
Sum of the molar concentration of all ions = Molar concentration of Ag+ ions + Molar concentration of Cl- ions
= 1.33 M + 1.33 M
= 2.66 M
Therefore, the correct answer is option 'B', 2.66 M.
Given:
Volume of Ag2SO4 solution (V1) = 2 L
Molar concentration of Ag2SO4 solution (C1) = 2 M
Volume of NaCl solution (V2) = 4 L
Molar concentration of NaCl solution (C2) = 1 M
To find:
Sum of the molar concentration of all ions
Step 1: Calculate the moles of Ag2SO4
Moles of Ag2SO4 = Molar concentration of Ag2SO4 × Volume of Ag2SO4 solution
= 2 M × 2 L
= 4 moles
Step 2: Calculate the moles of NaCl
Moles of NaCl = Molar concentration of NaCl × Volume of NaCl solution
= 1 M × 4 L
= 4 moles
Step 3: Write the balanced chemical equation
Ag2SO4(aq) + 2NaCl(aq) → 2AgCl(s) + Na2SO4(aq)
From the balanced chemical equation, we can see that 1 mole of Ag2SO4 reacts with 2 moles of NaCl to form 2 moles of AgCl.
Step 4: Calculate the moles of AgCl formed
Moles of AgCl formed = 2 × Moles of NaCl
= 2 × 4 moles
= 8 moles
Step 5: Calculate the molar concentration of AgCl
Molar concentration of AgCl = Moles of AgCl formed / Total volume of solution
= 8 moles / (2 L + 4 L)
= 8 moles / 6 L
= 4/3 M
≈ 1.33 M
Step 6: Calculate the sum of the molar concentration of all ions
Since AgCl is a strong electrolyte and completely dissociates in water, the molar concentration of Ag+ ions and Cl- ions in the solution will be equal to the molar concentration of AgCl.
Sum of the molar concentration of all ions = Molar concentration of Ag+ ions + Molar concentration of Cl- ions
= 1.33 M + 1.33 M
= 2.66 M
Therefore, the correct answer is option 'B', 2.66 M.
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Assuming complete precipitation of AgCl, calculate the sum of the molar concentration of all the ions if 2 lit of 2M Ag2SO4is mixed with 4 lit of 1 M NaCl solution is :a)4Mb)2Mc)3Md)2.5MCorrect answer is option 'B'. Can you explain this answer?
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Assuming complete precipitation of AgCl, calculate the sum of the molar concentration of all the ions if 2 lit of 2M Ag2SO4is mixed with 4 lit of 1 M NaCl solution is :a)4Mb)2Mc)3Md)2.5MCorrect answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Assuming complete precipitation of AgCl, calculate the sum of the molar concentration of all the ions if 2 lit of 2M Ag2SO4is mixed with 4 lit of 1 M NaCl solution is :a)4Mb)2Mc)3Md)2.5MCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Assuming complete precipitation of AgCl, calculate the sum of the molar concentration of all the ions if 2 lit of 2M Ag2SO4is mixed with 4 lit of 1 M NaCl solution is :a)4Mb)2Mc)3Md)2.5MCorrect answer is option 'B'. Can you explain this answer?.
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