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To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,
MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).
Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.
(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)
MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).
Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.
(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)
Correct answer is '126'. Can you explain this answer?
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Verified Answer
To measure the quantity of MnCl2 dissolved in an aqueous solution, it ...
The given reactions are.
Number of millimoles of oxalic acid are calculated below,
The number of millimoles of KMnO4 that react with oxalic acid is 1.
The number of millimoles of MnCl2 that are required initially is 1.
Thus, calculate the mass of MnCl2 that is required initially.
M=1x126 mg
= 126 mg
Number of millimoles of oxalic acid are calculated below,
The number of millimoles of KMnO4 that react with oxalic acid is 1.
The number of millimoles of MnCl2 that are required initially is 1.
Thus, calculate the mass of MnCl2 that is required initially.
M=1x126 mg
= 126 mg
Most Upvoted Answer
To measure the quantity of MnCl2 dissolved in an aqueous solution, it ...
2KMnO4(aq) + 16HCl(aq) → 2MnCl2(aq) + 2KCl(aq) + 8H2O(l) + 5Cl2(g)
In this reaction, 2 moles of KMnO4 react with 16 moles of HCl to produce 2 moles of MnCl2.
To measure the quantity of MnCl2 dissolved in the aqueous solution, you can follow these steps:
1. Take a known volume of the aqueous solution containing MnCl2.
2. Add excess K2S2O8 and H2O to the solution.
3. Titrate the resulting solution with a standardized solution of KMnO4.
4. The endpoint of the titration is reached when the pink color of KMnO4 persists after swirling the solution.
5. Record the volume of KMnO4 solution required to reach the endpoint.
6. Use stoichiometry to calculate the moles of MnCl2 present in the solution.
- Since 2 moles of KMnO4 react with 2 moles of MnCl2, the moles of MnCl2 can be calculated using the equation:
Moles of MnCl2 = (volume of KMnO4 solution used) * (molarity of KMnO4 solution) / 2
7. Finally, the quantity of MnCl2 dissolved in the aqueous solution can be determined by converting moles to grams using the molar mass of MnCl2.
In this reaction, 2 moles of KMnO4 react with 16 moles of HCl to produce 2 moles of MnCl2.
To measure the quantity of MnCl2 dissolved in the aqueous solution, you can follow these steps:
1. Take a known volume of the aqueous solution containing MnCl2.
2. Add excess K2S2O8 and H2O to the solution.
3. Titrate the resulting solution with a standardized solution of KMnO4.
4. The endpoint of the titration is reached when the pink color of KMnO4 persists after swirling the solution.
5. Record the volume of KMnO4 solution required to reach the endpoint.
6. Use stoichiometry to calculate the moles of MnCl2 present in the solution.
- Since 2 moles of KMnO4 react with 2 moles of MnCl2, the moles of MnCl2 can be calculated using the equation:
Moles of MnCl2 = (volume of KMnO4 solution used) * (molarity of KMnO4 solution) / 2
7. Finally, the quantity of MnCl2 dissolved in the aqueous solution can be determined by converting moles to grams using the molar mass of MnCl2.
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To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer?
Question Description
To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer?.
To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer?.
Solutions for To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer?, a detailed solution for To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? has been provided alongside types of To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4 using the reaction,MnCl2 + K2S2O8 + H2O → KMnO4 + H2SO4 + HCl (equation not balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of MnCl2 (in mg) present in the initial solution is ____.(Atomic weights in g mol-1: Mn = 55, Cl = 35.5)Correct answer is '126'. Can you explain this answer? tests, examples and also practice JEE tests.
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