There is a redox reaction between oxalic acid being oxidised by acidic permanganate ions (MnO4-). Products are H2O(l) and CO2(g) and Mn2+ ions.
we add sulpheric acid with oxalic acid to stable the ions when titrated against KMNO4
The balanced chemical equation would be K4FeC6N6 + KMnO4 + H2SO4 = KHSO4 + Fe2SO43 + MnSO4 + HNO3 + CO2 + H2O.
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Yes; the chemical reaction is:2 KMnO4 + 2 H2SO4 → Mn2O7 + H2O + 2 KHSO4
KMnO4 and H2SO4 are oxidising agents. Oxidising agents are hungry for electrons...
consider the balance chemical equation, suppose the reaction with oxalic acid 2MnO4- + 16H+ + 5C2O4 --> 2Mn+2 + 8H2O + 10CO2 Above reaction shows that the reaction requires a number of protons to occur, H2SO4 is the source of these protons.
we add sulpheric acid with oxalic acid to stable the ions when titrated against KMNO4
Oxalic acid is generally warmed slightly because it is not completely soluble and heat helps this. It aids in accuracy of the titration.
The balanced chemical equation would be K4FeC6N6 + KMnO4 + H2SO4 = KHSO4 + Fe2SO43 + MnSO4 + HNO3 + CO2 + H2O.
Kbr
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Potassium Permanganate (KMnO4) reacts with Sulphuric acid (H2SO4) to produce Manganese Heptoxide (MnO7), water (H20) and Potassium Hydrogen Sulphate (KHSO4)2. The reactive species produced is Manganese Heptoxide (which is a very powerful oxidiser). The Manganese Heptoxide will oxidise the Oxalic acid (COOH)2 to Carbon dioxide (CO2).
Potassium permanganate solutions due to the strong oxiding nature readily forms MnO2 on contact with impurities. Traditionally sources of KMnO4 always contained traces of MnO2 . KMnO4 solutions "go off" when they stand for a period.
KMno4 is reduced to Mn^2+ Salt and the pink colour is discharged by the nascent hydrogen produced when zinc reacts with h2so4
FeCl2 + 2KMnO4 --> Fe(MnO4)2 + 2KCl
The answer is: 4 KMnO4=2 K2O+4 MnO+5 O2