Potassium Hypochlorite Formula: Properties, Structure & Uses

Ans: The formula of potassium hypochlorite is KClO, salt hypochlorous acid. 

Ans: Some of the uses of potassium hypochlorite are as follows:

• The chemical compound is used for disinfecting water and sanitizing the surface
• It is also used as a bleaching agent
• Then, it is used as an industrial oxidizer
• Used in agriculture field

Ans: Potassium hypochlorite is prepared by the reaction of chlorine with a solution of potassium hydroxide.

Cl₂ + 2 KOH → KCl + KClO + H₂O

Another production method of this potassium hypochlorite is electrolysis of potassium chloride solution. The reaction mixture with both methods must be kept cold to prevent the formation of potassium chlorate.

Ans: Potassium Chlorate is often viewed as a unique inorganic compound that was first discovered by a French Chemist, by the name of, Louis Berthollet at the end of the 18th Century. It is also known as a pot crate and has various trade names such as Fegabit or Fekabit. In its purest form, it is found as a white crystalline powder at room temperature.

Ans: The formula of this compound is KClO₃ which indicates, that in its most empirical form the compound has 1 potassium, 1 chlorine, and 3 oxygen atoms.

Ans: The physical properties of KClO₃ are:

• The chemical compound is a crystalline solid that is white.
• The molar mass of KClO₃ is 122.55 g/mol.
• The density is often mentioned as 2.32 g/cm³.
• The melting point is calculated to be 629.15 K.
• The boiling point is estimated to be 673.15 K.
• It is hygroscopic which means that it readily absorbs moisture from the air.
• The crystal structure of this compound is monoclinic.

Ans: It is soluble in glycerol. It is partially soluble in liquid ammonia and acetone.

Ans: This process turns out to be the most feasible one for the industrial production of potassium chlorate. This is due to its high industry applications. In this method, chlorine gas is passed through hot calcium hydroxide. Then, potassium chloride is added. This is how potassium chlorate is produced in this process.

The reactions involved are as follows:

6Ca(OH)₂ + 6Cl₂ à Ca(ClO₃)₂ + 5CaCl₂ + 6H₂O

Ca(ClO₃)₂ + 2KCl à 2KClO₃ + CaCl₂

Ans: Electrolysis of potassium chloride helps to make potassium chlorate. The anode here will be carbon, platinum, or mixed metal oxide and the cathode here is made of titanium. The aqueous solution is of potassium chloride and a current is then passed through the whole setup. Potassium chlorate is obtained as a precipitate in this reaction. It is obtained in the form of crystals as the reaction progresses. These crystals can be obtained by emptying the cell contents and filtering them.

Ans: This process is extremely useful if we need potassium chlorate in small amounts. Sodium chloride and sodium chlorate are formed by the disproportionation of sodium hypochlorite post which sodium chlorate undergoes metathesis with potassium chloride.

Ans: There is a very logical reason behind the use of potassium chlorate in firecrackers. This is related to its property of being a strong oxidizing agent. It produces oxygen on decomposition. This extreme amount of heat excites the colors in the firecrackers and causes their consumption. However, its usage had to be banned due to its application in anti-social and illegal activities.

Ans: It is suitable for ignition due to its oxidizing properties.

Potassium Chlorate immediately decomposes if heated in the presence of a catalyst such as MnO₂. The reaction is given below –

2KClO₃(s) à 3O₂(g) + 2KCl(s)

If it is heated in the absence of a catalyst, then on decomposition it gives potassium perchlorate and Potassium Chloride. The reaction is given below –

4KClO₃ --> 3KClO₄ + KCl

On further heating, potassium perchlorate decomposes into oxygen and Potassium Chloride. The reaction is as follows –

KClO₄ à KCl + 2O₂

Ans: It can be used as a disinfectant.

It has its application in safety matches in very small quantities.

It is used in laboratories for experiments.

It is used for making pesticides.

It is found in smoke grenades.