Acidified Potassium Permanganate

One of the chemical compounds of potassium is called as potassium permanganate. The chemical formula of potassium permanganate is KMnO4. It acts as a strong oxidizing agent which was discovered in 1659. This compound has ability to add oxygen or remove hydrogen or remove electrons from an element or compound. KMnO4 (potassium permanganate) is composed of 1-Mn atom is surrounded by 4-O-atoms.

The molecular weight of KMnO4 is 158.04 g/mol with tetrahedral structure. The oxidation of iron can be done in the presence of potassium permanganate to form an insoluble manganese dioxide and iron oxide which can be removed by filtration. It has dark colour purple solid which form pink colour solution in water.

The colour of solution depends on the concentration of compound in solution. This compound has very useful for various applications such as for the treatment of water in pharmaceutical manufacture. It is used to oxidize Fe, Mn, H2S and ‘As’ impurities. 

The treatment of water with it also improves taste and odour. It is used as a pre-oxidant for disinfection by-product control. KMnO4 can help to produce high quality water which can easily meet drinking water standards. It mainly involves in the oxidation of functional groups like aromatic side chains to RCOOH, organic sulphides to sulphones which is used to produce antibiotics and tranquilizers.

The oxidation reaction of KMnO4 is effected by the pH of the solution as Mn can exist from 2+ to 7+ oxidation state. Out of that Mn7+ is the most potent oxidation state in both acid and alkaline medium. This oxidation process is widely used in organic synthesis such as phase transfer catalysis. For example the oxidation of ferrous sulphate with acidified potassium permanganate results the formation of ferric sulphate with manganese sulphate and potassium sulphate. The oxidation reaction can be written as given below;

8H2SO4 + 2KMnO4 + 10FeSO4  â†’ 2MnSO4 + 5Fe2(SO4)3 + 8H2O + K2SO4

The 0.1 M acidified potassium permanganate solution can be prepared with 1.6g of KMnO4 in 100mL water which is acidified by the addition of 5 mL of 1 M solution of sulphuric acid.  The acidification cannot be done with the help of hydrochloric acid as it gets oxidised to chlorine gas. On the contrary, the alkaline solution of KMnO4 can be prepared with the help of potassium permanganate and 2% sodium carbonate solution.
We cannot write one formula for acidified potassium permanganate as it is a mixture, not a pure compound.  Manganese exists in 7+ oxidation state in potassium permanganate which is reduced to colourless or pink Mn2+ ion in acidic medium. The ionic reaction can be written as given below;

MnO4- +  8H+  +   5e-  â†’  Mn2+  +  4H2O


In the titration of KMnO4 with iron (II) solution, we have to take permanganate solution in the burette and add slowly to the solution of iron (II) which acts as reducing agent. As the purpel colour solution is added to iron(II) solution, the purpel colour is discharged. The addition of excess of permanganate solution makes the solution pink.

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Question:what is the full chemical equation for oxalic acid added to potassium permanganate acidified with a few drops of concentrated sulfuric acid?

Answers:Write the unbalanced equation first: H2C2O4 + (MnO4)-(aq) ---> CO2(g) + Mn2+(aq) You can determine the products simply by looking up tables of standard electrode potentials such as http://www.jesuitnola.org/upload/clark/r Now, write the half-reactions and balanced them based on redox rules: H2C2O4 ---> 2 CO2(g) + 2 H+(aq) + 2 e- (MnO4)-(aq) + 8 H+(aq) + 5 e- ----> Mn2+(aq) + 4 H2O(l) 5 H2C2O4 ---> 10 CO2(g) + 10 H+(aq) + 10 e- 2 (MnO4)-(aq) + 16 H+(aq) + 10 e- ----> 2 Mn2+(aq) + 8 H2O(l) -------------------------------------- 5 H2C2O4 + 2 (MnO4)-(aq) + 6 H+(aq) ----> 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)

Question:what is the full chemical equation for oxalic acid added to potassium permanganate acidified with a few drops of concentrated sulfuric acid?

Answers:Write the unbalanced equation first: H2C2O4 + (MnO4)-(aq) ---> CO2(g) + Mn2+(aq) You can determine the products simply by looking up tables of standard electrode potentials such as http://www.jesuitnola.org/upload/clark/refs/red_pot.htm Now, write the half-reactions and balanced them based on redox rules: H2C2O4 ---> 2 CO2(g) + 2 H+(aq) + 2 e- (MnO4)-(aq) + 8 H+(aq) + 5 e- ----> Mn2+(aq) + 4 H2O(l) At this point, balance the number of electrons on both equations by cross-multiplying each equation by the number of electrons of their counterpart equation and then add the equations together: 5 H2C2O4 ---> 10 CO2(g) + 10 H+(aq) + 10 e- 2 (MnO4)-(aq) + 16 H+(aq) + 10 e- ----> 2 Mn2+(aq) + 8 H2O(l) ----------------------------------------------------------------------------------------- 5 H2C2O4 + 2 (MnO4)-(aq) + 6 H+(aq) ----> 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) Notice that the charge on both sides of the equation is +4: 2(-1) + 6(1) = 2(2) -2 + 6 = 4 4 = 4 This implies that are redox equation has been balanced correctly. Cheers.

Question:What observation would be present if the above So2 was reacted with acidified potassium Permanganate? And can you tell me why you assume this observation would occur? Please

Answers:Potassium permanganate has a purple colour. Sulphur dioxide is a reducing agent. Potassium permanganate is an oxidizing agent. When sulphur dioxide reacts with potassium permanganate the solution decolourizes. colour changes from Purple to transparent(Colourless). Reason : Potassium permanganate gets reduces by sulphur dioxide. Hope this helped!

Question:acid is sulphuric acid and I would also like to know the word equation is well!!! it says that the product will be adipic acid, I think it's hexanoic acid not sure but what are the formulaes??

Answers:Close, but not quite. The product (adipic acid) is hexane-dicarboxylic acid (there is a carboxylic acid group on both ends of the hexane chain). The KMnO4 (potassium permanganate) is fully oxidizing the cyclohexene olefin to the point of severing the double bond (opening the ring up to acyclic chain) and oxidizing the ends all the way up to carboxylic acids. So: cyclohexene [-CH(CH2)4)CH-] (cyclic) + KMn04 + H2SO4 (probably with some water H2O) -> HO2C(CH2)4CO2H. The byproducts of this reaction is a bit more complex to elucidate. KMnO4 itself reacts with sulfuric acid to form Mn2O7 initially, but ultimately probably winds up as something like MnO2 (reduced state)

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