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Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition?
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Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they ...
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Introduction:
In acidic conditions, Mno4_ ions are reduced to Mn2+ ions whereas in neutral conditions they are reduced to Mno2. The oxidation of 25 ml of a solution x containing 20 ml of a solution y containing Mno4 ions. It is required to find the value of a solution y containing Mno4 ions to oxidize 25 ml of solution x containing Fe2+ ions in neutral conditions.
Calculations:
The balanced chemical equation for the oxidation of Fe2+ ions in neutral conditions is:
Mno4_ + 5Fe2+ + 8H+ → Mno2 + 5Fe3+ + 4H2O
From the equation, it is clear that for the oxidation of 5 moles of Fe2+ ions, 1 mole of Mno4_ ions is required. Therefore, the number of moles of Mno4_ ions required to oxidize 25 ml of solution x containing Fe2+ ions is:
Number of moles of Fe2+ ions in 25 ml of solution x = (20/25) * n, where n is the number of moles of Fe2+ ions in 20 ml of solution y.
Number of moles of Mno4_ ions required = (1/5) * (20/25) * n = (4/125) * n
In neutral conditions, Mno4_ ions are reduced to Mno2. The balanced chemical equation for the reduction of Mno4_ ions to Mno2 in neutral conditions is:
Mno4_ + 2H2O + 3e- → Mno2 + 4OH-
From the equation, it is clear that for the reduction of 1 mole of Mno4_ ions, 3 moles of electrons are required. Therefore, the number of moles of electrons required to reduce (4/125) * n moles of Mno4_ ions is:
Number of moles of electrons required = (4/125) * n * 3 = (12/125) * n
From the balanced chemical equation for the oxidation of Fe2+ ions in neutral conditions, it is clear that for the oxidation of 5 moles of Fe2+ ions, 8 moles of H+ ions are required. Therefore, the number of moles of H+ ions required to oxidize (20/25) * n moles of Fe2+ ions is:
Number of moles of H+ ions required = (8/5) * (20/25) * n = (32/25) * n
Conclusion:
To oxidize 25 ml of solution x containing Fe2+ ions in neutral conditions, a solution y containing (12/125) * n moles of electrons and (32/25) * n moles of H+ ions is required, where n is the number of moles of Fe2+ ions in 20 ml of solution y.
Introduction:
In acidic conditions, Mno4_ ions are reduced to Mn2+ ions whereas in neutral conditions they are reduced to Mno2. The oxidation of 25 ml of a solution x containing 20 ml of a solution y containing Mno4 ions. It is required to find the value of a solution y containing Mno4 ions to oxidize 25 ml of solution x containing Fe2+ ions in neutral conditions.
Calculations:
The balanced chemical equation for the oxidation of Fe2+ ions in neutral conditions is:
Mno4_ + 5Fe2+ + 8H+ → Mno2 + 5Fe3+ + 4H2O
From the equation, it is clear that for the oxidation of 5 moles of Fe2+ ions, 1 mole of Mno4_ ions is required. Therefore, the number of moles of Mno4_ ions required to oxidize 25 ml of solution x containing Fe2+ ions is:
Number of moles of Fe2+ ions in 25 ml of solution x = (20/25) * n, where n is the number of moles of Fe2+ ions in 20 ml of solution y.
Number of moles of Mno4_ ions required = (1/5) * (20/25) * n = (4/125) * n
In neutral conditions, Mno4_ ions are reduced to Mno2. The balanced chemical equation for the reduction of Mno4_ ions to Mno2 in neutral conditions is:
Mno4_ + 2H2O + 3e- → Mno2 + 4OH-
From the equation, it is clear that for the reduction of 1 mole of Mno4_ ions, 3 moles of electrons are required. Therefore, the number of moles of electrons required to reduce (4/125) * n moles of Mno4_ ions is:
Number of moles of electrons required = (4/125) * n * 3 = (12/125) * n
From the balanced chemical equation for the oxidation of Fe2+ ions in neutral conditions, it is clear that for the oxidation of 5 moles of Fe2+ ions, 8 moles of H+ ions are required. Therefore, the number of moles of H+ ions required to oxidize (20/25) * n moles of Fe2+ ions is:
Number of moles of H+ ions required = (8/5) * (20/25) * n = (32/25) * n
Conclusion:
To oxidize 25 ml of solution x containing Fe2+ ions in neutral conditions, a solution y containing (12/125) * n moles of electrons and (32/25) * n moles of H+ ions is required, where n is the number of moles of Fe2+ ions in 20 ml of solution y.
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Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition?
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Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition?.
Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition?.
Solutions for Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? in English & in Hindi are available as part of our courses for NEET.
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Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition?, a detailed solution for Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? has been provided alongside types of Mno4_ ions are reduced in acidic conditions to Mn2+ ions whereas they are reduced in neutral condition to Mno2. the oxidation of 25 ml of a solution x containing 20ml of a solution y containing Mno4 ions what value of a solution y containing Mno4 ions , what value of solution y would be required to oxidize 25ml of solution x containing fe2+ ions in neutral condition? theory, EduRev gives you an
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