- Examples of reactions
- characteristics
- Preparation
- Driving
- Storage
- Provision
- Permanganates
- 1- Potassium permanganate
- Pharmacology and Biochemistry
- Indicators and reagents
- Industrial use
- Manufacturing methods
- Safety and hazards
- Health hazard
- Fire danger
- Chemical hazards
- First aid if you come into contact with potassium permanganate
- 2- Sodium permanganate
- Use and manufacture
- Manufacturing methods
- 3- Calcium permanganate
- characteristics
- Medical use
The manganic acid or permanganic is a dibasic acid of formula H2MnO4 formed manganese, analogous to sulfuric acid. It is found only in solution and in manganate salts.
- Systematic name: Dihydrogen (tetraoxidomanganate).
- Type of compound: Oxoacids (ternary combinations formed by hydrogen, a non-metal element and oxygen).
- Molecular Formula: H2MnO4
- Molecular mass: 120.9515
Examples of reactions
MnO3 + H2O = H2MnO4
KMnO4 + H2O2 = KO2 + H2MnO4
Permanganate ion
characteristics
Permanganic acid solutions (up to 20%) are purple liquids, with an ozone odor. Crystal hydrate (HMnO4 · 2H2O) is a purple crystalline solid that decomposes above 20 degrees Celsius.
Permanganic acid is a very strong oxidant, although milder than its anhydride. It decomposes spontaneously, engulfing oxygen and precipitating manganese dioxide, which catalyzes further decomposition of the acid.
By cooling the unstable concentrated solution of the acid close to the freezing point, and crystal hydrate can be prepared. Sources vary depending on the nature of this compound: according to some sources, it is a hydronium salt of permanganic acid, according to others, it is a polymanganic acid complex.
Excessively concentrated solutions of this acid can decompose spontaneously with the evolution of ozone. This enables ozone to be chemically prepared by reacting potassium permanganate with sulfuric acid of medium concentration (50-80%).
This reaction produces an excessively concentrated solution of permanganic acid, which decomposes rapidly, releasing ozone.
Sulfuric acid with a concentration above 80% should not be used for this reaction as this can lead to the formation of anhydride (manganese epoxide), which is extremely dangerous.
Preparation
Permanganic acid can be prepared by dissolving manganese epoxide in water, or by reacting barium permanganate with sulfuric acid. An impure solution can also be prepared by dissolving potassium permanganate in sulfuric acid of medium concentration (50-80%).
Driving
Not much is known about the dangers of permanganic acid, but it should be treated with caution as it is a strong acid and a very strong oxidant. Also, it can release ozone, which is toxic.
Storage
It is not practical to store this acid due to its instability. It should be used as soon as it is done. The hydrate can be stored as long as it is frozen (below the freezing point of water).
Provision
Permanganic acid can be discharged into the soil, as it causes the compound to decompose, oxidizing the soil and turning into manganese dioxide, which is safe and insoluble.
Permanganates
The univalent anionic group MnO4 derived from permanganic acid all being strong oxidizing agents. They are salts that contain the anion MnO4-, usually deep purplish red in color and with strong oxidizing properties.
1- Potassium permanganate
Molecular formula: KMnO4
Molecular weight: 158.032 g / mol
It is the best known of all the permanganates. Also known as Condy crystals, it is a highly oxidizing compound, odorless, soluble in water and in many organic solvents, has purple crystals, and a sweet taste. (Definition from the McGraw-Hill Dictionary of Scientific and Technical Information, 4th ed).
Potassium permanganate is not combustible but it accelerates the ignition of combustible material. If the combustible material is finely divided, the mixture may be explosive. When it comes into contact with liquid combustible materials it can cause spontaneous ignition. In contact with sulfuric acid, it may cause fire or explosion. It is used to make other chemicals and as a disinfectant.
Pharmacology and Biochemistry
Pharmacological classification: MeSH
Indicators and reagents
They are substances used for the detection, identification and analysis of chemical, biological or pathological processes or conditions.
Indicators are substances that change in physical appearance, for example color, when approaching the point where it passes between acidity and alkalinity. Reagents are substances used for the detection or determination of another substance by chemical or microscopic means, in particular analysis.
The types of reagents are precipitants, solvents, oxidants, reducers, fluxes, and colorimetric reagents. (Hackh's Chemical Dictionary, 5th edition, pg. 301, pg.499).
Industrial use
As bleaching agents, odor agents and oxidizing / reducing agents.
Manufacturing methods
They can be prepared by oxidizing manganese dioxide with potassium chlorate in potassium hydroxide solution, then completing the oxidation with chlorine or air and carbon dioxide.
Safety and hazards
-It can intensify the fire.
-It is harmful by ingestion.
- Causes severe skin burns.
- May cause eye damage.
-May cause irritation of the respiratory tract.
- Suspected of causing genetic defects.
- It is suspected that it may damage fertility and the fetus.
- Causes damage to organs through prolonged or repeated exposure.
- It is very toxic to aquatic organisms, with long-lasting harmful effects.
Health hazard
May cause burns and dark brown skin spots. If ingested, it severely affects the gastrointestinal system. It can be fatal if over 4 ounces are consumed.
Fire danger
It is not combustible but increases the combustion of other substances. Causes irritating or toxic gases or vapors in fire.
Behavior in Fire: May cause fire in contact with fuels causing containers to explode. May cause great risk of fire and explosion in contact with combustible substances or reducing agents.
Chemical hazards
It decomposes on heating and this produces toxic gases and irritating fumes. The substance is a strong oxidant. Reacts with combustible and reducing materials which generates fire and explosion hazard. Reacts violently with powdered metals, creating a fire hazard.
First aid if you come into contact with potassium permanganate
If ingested, induce vomiting and follow with a complete gastric lavage.
If inhaled, fresh air and rest are required. Artificial respiration may be necessary. It is necessary to consult a doctor.
If it comes in contact with skin, rinse with plenty of water for at least 15 minutes, then remove contaminated clothing and rinse again. It is also important to consult a doctor.
If it comes into contact with the eyes, rinse with plenty of water for several minutes. Seek medical attention.
2- Sodium permanganate
Molecular Formula: MnNaO4
Molecular Weight: 141.924 g / mol
Sodium permanganate is a purple crystalline solid. Non-combustible but accelerates the burning of combustible material. May spontaneously ignite in contact with liquid combustible materials. Contact with sulfuric acid can cause fire or explosion. Used in medicine, as a disinfectant, and for many other uses.
Use and manufacture
It is used in industry as an oxidizing and reducing agent. It is also used for water treatment, to whiten textiles
Manufacturing methods
The sodium manganate is dissolved in water and chlorine or ozone is introduced. The solution is concentrated and crystallized.
3- Calcium permanganate
Molecular formula: CaMn2O8
Molecular weight: 277.946 g / mol
characteristics
Calcium permanganate is a purple crystalline solid. It is used as a disinfectant and deodorizer, in water purification, and for many other uses.
Medical use
The manganic ion resulting from this permanganate is astringent which helps to suppress inflammation.