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To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)Correct answer is '126'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.

Here you can find the meaning of To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)Correct answer is '126'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of To measure the quantity of MnCl2 dissolved in an aqueous solution, it was completely converted to KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)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 KMnO4using the reaction, MnCl2 + K2S2O8 + H2O -->KMnO4 + H2SO4 + HCl (equation not balanced). Few dropsof concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) wasadded 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)a)b)c)d)Correct answer is '126'. Can you explain this answer? tests, examples and also practice JEE tests.