The brown precipitate is MnO2, it is the product of the following redox in neutral environment:
For each half reaction:
MnO4- + 4H++ 3e- → MnO2 + 2H2O REDUCTION
HSO3- + H2O → SO42- + 3H+ + 2e- OXIDATION
Overall: Permanaganate half reaction x2 + Bisulfite half reactionx3
2MnO4- + 3HSO3- + 8H+ + 3H2O + 6e- → 2MnO2 + 3SO42- + 4H2O + 9H+ + 6e-
Cancelling like terms:
2MnO4- + 3HSO3- → 2MnO2 + 3SO42- + H3O+
Note that all species are balanced, all charges are balanced and the brown precipitate MnO2 is accounted for. The reaction also predicts that acid is formed in the process.
Potassium permanganate and sulfite:2MnO4-(aq) + 5SO32-(aq) + 6H+(aq) --> 5SO42- + 2Mn2+(aq) + 3H2O(l)Note:Potassium and sodium ions do NOT react, they are tribune-ions
sodium permanganate
They are not soluble, therefore they do not precipitate or form a color....a.k.a....no reaction...
Melting point of Sodium bisulfite NaHSO3 150 °C, 423 K, 302 °F
1.928
Potassium permanganate and bisulfite in stronger acid environment:2MnO4-(aq) + 5HSO3-(aq) + H+(aq) --> 5SO42- + 2Mn2+(aq) + 3H2O(l)Note:Potassium and sodium ions do NOT react, they are tribune-ions.
Alkaline potassium permanganate solution is a solution of potassium permanganate containing an alkali. The alkali can be sodium hydroxide or potassium hydroxide.
KMnO4 is potassium permanganate.
Yes. Sodium permanganate is an ionic compound comprising mono-atomic sodium cations and polyatomic permanganate anions.
nope
Examples: sodium chloride, potassium chloride, calcium chloride, sodium hydrogen carbonate, sodium citrate, potassium permanganate, magnesium sulfate etc.
Examples: sodium chloride, potassium chloride, calcium chloride, sodium hydrogen carbonate, sodium citrate, potassium permanganate, magnesium sulfate etc.
Potassium permanganate and sulfite:2MnO4-(aq) + 5SO32-(aq) + 6H+(aq) --> 5SO42- + 2Mn2+(aq) + 3H2O(l)Note:Potassium and sodium ions do NOT react, they are tribune-ions
Sodium hydrogen sulphite: Sodium bisulfite, not sodium "meta" bisulfite
sodium permanganate
KMnO4 + NaNO2 -> KNO2 + NaMnO4
"Hard scrubbing with water or scrubbing with Sodium Bisulfite solution." Good answer! It worked like a charm. I used saturated sodium bisulfite, aqueous. I've gotten the habit of first trying Nochromix in concentrated sulfuric acid for cleaning laboratory glassware. This doesn't work at all for glass bottles which have contained an aqueous solution of 1% potassium permanganate for many years. So I doubt that the other answer here, namely, to use lemon juice, would work at all since this is a much weaker acid than sulfuric. Caution: If you don't rinse out the sulfuric acid before trying sodium bisulfite, you must do this in a fume hood or a well-ventilated area since SO2 gas (or some other nasty respiratory irritant) evolves.