Potassium permanganate

What is potassium permanganate?
Potassium permanganate is an oxidising agent with disinfectant, deodorising and astringent properties. Its chemical formula is KMnO4. It is sometimes called by its common name, Condy’s crystals.
In its raw state, potassium permanganate is an odourless dark purple or almost black crystal or granular powder.

How is potassium permanganate solution prepared?

A potassium permanganate solution is made by dissolving crystals or powder in water aiming for a 1-in-10,000 solution. Potassium permanganate tablets can also be used. If using 400 mg tablets, add one to each 4 L of water. The tablets should be dissolved in hot water before pouring into the bath.
The potassium permanganate solution should be a pink colour.

From Wikipedia
Potassium permanganate is an inorganic compound with the chemical formula KMnO4 and composed of K+ and It is a purplish-black crystalline salt, that dissolves in water to give intensely pink or purple solutions.
Potassium permanganate is widely used in chemical industry and laboratories as a strong oxidizing agent, and also as a medication for dermatitis, for cleaning wounds, and general disinfection.

Almost all applications of potassium permanganate exploit its oxidizing properties.[6] As a strong oxidant that does not generate toxic byproducts, KMnO4 has many niche uses.

Water treatment
Potassium permanganate is used extensively in the water treatment industry. It is used as a regeneration chemical to remove iron and hydrogen sulfide (rotten egg smell) from well water via a “Manganese Greensand” Filter. “Pot-Perm” is also obtainable at pool supply stores and is used additionally to treat waste water. Historically it was used to disinfect drinking water and can turn the water pink.[11] It currently finds application in the control of nuisance organisms such as zebra mussels in fresh water collection and treatment systems.
Reaction with acids

The reaction of permanganate with concentrated hydrochloric acid gives chlorine. The Mn-containing products from redox reactions depend on the pH. Acidic solutions of permanganate are reduced to the faintly pink manganese(II) ion (Mn2+) and water. In neutral solution, permanganate is only reduced by three electrons to give manganese dioxide (MnO2), wherein manganese is in a +4 oxidation state. This is the material that stains one’s skin when handling KMnO4. KMnO4 spontaneously reduces in an alkaline solution to green K2MnO4, wherein manganese is in the +6 oxidation state.
A curious reaction occurs upon addition of concentrated sulfuric acid to potassium permanganate. Concentrated sulfuric acid reacts with KMnO4 to give Mn2O7, which can be explosive.[41] Although no reaction may be apparent, the vapor over the mixture will ignite paper impregnated with alcohol. Potassium permanganate and sulfuric acid react to produce some ozone, which has a high oxidizing power and rapidly oxidizes the alcohol, causing it to combust. As the reaction also produces explosive Mn2O7, this should only be attempted with great care.

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