Manganate and Permanganate - Chemistry Stack Exchange However, permanganate is $\ce {MnO4-}$ and manganate is $\ce {MnO4^2-}$ The charges are different but there are still four oxygen atoms in each, so it seems to violate the convention
The Role of Acidified Potassium Manganate (VII) in Oxidation of . . . The chemical equation for the oxidation of ethanol is given as: $$\ce {C2H5OH + 2 [O] -> CH3COOH + H2O} $$ Acidified potassium manganate (VII) solution $\ce {KMnO4}$ is added as the oxidising agent My question is how does the $\ce {KMnO4}$ help in the oxidation?
How does the reaction of HCl and KMnO4 proceed? I'm assuming that you were expecting a double replacement Clearly that doesn't happen here, and it's because of the permanganate ion $\ce {KMnO4}$ is a powerful oxidizing agent That means that it likes to steal electrons from other species, ultimately producing $\ce {Mn^2+}$ ions and water If we look at the species in solution with it, $\ce {K^ {+}}$, $\ce {H^ {+}}$, and $\ce {Cl
The hydrogen ion in acidified potassium manganate (VII) 2 Recently, I am playing with redox reaction and I come over a compound acidified potassium manganate (VII) ($\ce {KMnO4 H^+}$) I get confused that why they put $\ce {H^+}$ beside $\ce {KMnO4}$ Doesn't the hydrogen ions flow freely in the solution or something else