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Question:Its used in an experiment about adsorptionmof oxalic acid using acitivated charcoal and its really important!
Answers:2(MnO4)- + 5C2O4H2 + 6H+ -------> 2Mn2+ + 10CO2 + 8H2O
Answers:In basic solution, you get a different reaction (formation of MnO4-2 or MnO2) instead of the formation of Mn+2.
Question:It doesn't really matter what the aldehyde is, I just want to see a full equation for one and potassium permanganate, because my chemistry textbook says that KMNO4 is used to oxidise an aldehyde and form an carboxylic acid, but it doesn't show the whole equation. I especially need to see what happens to the potassium permangate, and all the products. A short explination would be awesome. Thanks :)
Answers:The half-equation for MnO4- is given below (K+ is a spectator ion)
MnO4- + 8H+ + 5e --> Mn2+ + 4H2O
The aldehyde would be oxidized to a carboxylic acid, you're right. Thus a carboxylic acid would be one of your products.
As seen from my equation above, you should also get Mn2+ (a faint pink solution) as well as H2O (water).
However, in general, it is not necessary for students to give the equation for KMnO4 when discussing the oxidation of carbonyl compounds. It is sufficient to denote the oxidation by the general equation:
aldehyde + [O] --> carboxylic acid
where [O] represents oxygen (oxidation here being the basic addition of oxygen to the aldehyde)
Hope I was of help!
Episode 5: Potassium Permanganate (KMnO4)Hello Chemists. Today I will be showing you some reactions involving Potassium Permanganate. This compound is a powerful oxidizing agent and this propriety makes it useful in qualitative analytical chemistry in redox titration. It is also used as a disinfectant and in water treatment. In this video I will be doing three well known reactions with KMnO4. The chemical chameleon. KMnO4 + Sucrose (Sugar) and NaOH KMnO4 + Glycerol (Glycerin) Spontaneous combustion Manganese Heptoxide.
Glycerin Reacting With Potassium Permanganate And Magnesium Powder!I put 4 drops of glycerin(glycerine, glycerol) onto a mix of 2 pars potassium permanganate powder, and one part magnesium powder, as the exothermic reaction got hotter and hotter, it ignited the glycerin, and soon after the mix of powders. The purple flame you can see right before the flash is the glycerine burning(it is purple from potassium ions)
Oxidation state of potassium permanganate/chemical chameleonSorry for unclear subtitles,here I write it again: 0:07-To perform this reaction,dissolve spatula of sodium hydroxide in 100ml of water. 0:18-This is to provide alkaline environment for the reaction. 0:30-Ok,let dissolve this thing. 1:08 And now,dissolve 3 spatula of sucrose in 100ml of water 1:14-sucrose act as reducing agent in this experiment 1:19-depending on your sodium hydroxide and sucrose concentration,the duration of each stages in this experiment can be vary. 1:37-let me dissolve this thing too. 2:13-the deep violet solution of potassium permanganate is quickly reduced to green species (manganate ions) 2:25-after that the colour of the solution will change to olive green and lastly to amber (suspension of hydrous MnO2) 2:32-with a higher concentration, it will quickly precipitate MnO2 out of the solution. 2:37-With a higher concentration also,the reaction is not visible as the change of colour cannot be seen. Permanganate ions is slowly reduced in an alkaline environment by sugar.Sugar is organic compound,having many -OH group,attached to carbon atoms,which also have hydrogen atom attached directly to it.Such compound,containing -C(H)(OH)- structure (secondary alcohols group) are easily oxidized. The oxidation of the --C(H)(OH)-- structure is as follows, where the alcohol-group is oxidized to a ketone-group: --C(H)(OH)-- + 2OH-- --C(=O)-- + 2H2O + 2e This reaction requires hydroxide ions. The observed speed of the reaction indeed is strongly depending on the ...
Barium Peroxide, Sulfuric Acid: Iron, Potassium PermanganateNote: the "poor explanation" of my video is strictly due to the fact that this experiment corresponds to a university class. I can't just give out reactions and answers. The video can be used to analyse the reaction. Were there bubbles (ie, evolution of a gas)? If so, what gas is it? Does the permanganate solution simply dilute in colour, or is there a colour change? This would clearly indicate a reaction. Is there precipitate formation? Again, very indicative of a reaction, if there is. Think about what you observe to help answer questions on the experiment, such as chemical equations. In my "Chemistry of the Main Group Elements" lab at the University of Manitoba in Winnipeg, we synthesised the barium peroxide. This video shows the experimentation with the substance, involving barium peroxide in sulfuric acid, with experimentation involving iron and potassium permanganate (separately). A solution was made, with about 0.3 grams of barium peroxide (synthesised earlier in the experiment) placed into about 20 millilitres of sulfuric acid solution. The solution was split into two. One portion had about 0.1 grams of iron powder added to it. This is the first re ction. The second portion had a solution of 2 crystals of potassium permanganate dissolved in about 5 millilitres of water added to it. This is the second re ction.