Potassium chlorate (KClO3) is a chemical compound consisting of potassium, chlorine, and oxygen. It is commonly used in the manufacture of matches, explosives, and fireworks due to its oxidizing properties.
| IUPAC Name | Potassium chlorate |
| Molecular Formula | KClO3 |
| CAS Number | 3811-04-9 |
| Synonyms | Kaliumchlorat, Chlorkalic, Chlorate de potassium, Perchlorate de potassium, UN 1485, Potassium chlorate, Kalium perchloricum |
| InChI | InChI=1S/ClH3KO3/c2-1(3)4/h(H3,2,3,4)/p-1 |
Potassium Chlorate Properties
Potassium Chlorate Formula
Potassium chlorate has a chemical formula of KClO3, which indicates that it consists of one potassium atom, one chlorine atom, and three oxygen atoms. It is an ionic compound that forms when K+ and ClO3- ions combine through an ionic bond. The compound is highly reactive due to the presence of oxygen, which gives it strong oxidizing properties.
Potassium Chlorate Molar Mass
The molar mass of KClO3 is 122.55 g/mol. This is the sum of the atomic masses of the individual elements that make up the compound, namely potassium, chlorine, and oxygen. The molar mass is an important parameter in chemistry as it is used to calculate the mass of a substance required to produce a certain amount of product in a chemical reaction.
Potassium Chlorate Boiling Point
KClO3 does not have a well-defined boiling point since it decomposes before it reaches its boiling point. When heated, it decomposes into potassium chloride and oxygen gas. Therefore, KClO3 undergoes a thermal decomposition reaction rather than a boiling point.
Potassium Chlorate Melting Point
The melting point of KClO3 is 356 °C (673 °F). At this temperature, the solid compound melts and transforms into a liquid. The melting point is a critical property of a compound as it influences the physical behavior of the substance, including its solubility and density.
Potassium Chlorate Density g/mL
The density of KClO3 is 2.32 g/mL at room temperature. This means that a specific volume of the compound has a certain mass, which is useful in determining the mass of a substance required for a particular chemical reaction. The density of KClO3 also affects its solubility in water, as compounds with higher densities tend to be less soluble in water.
Potassium Chlorate Molecular Weight
The molecular weight of KClO3 is 122.55 g/mol. This is the sum of the atomic weights of its constituent atoms, namely potassium, chlorine, and oxygen. Molecular weight is an essential parameter in stoichiometry as it is used to calculate the amounts of reactants and products in a chemical reaction.
Potassium Chlorate Structure
KClO3 has a crystalline structure in its solid form, consisting of potassium, chlorine, and oxygen atoms arranged in a specific pattern. The compound forms a face-centered cubic crystal lattice structure, in which each potassium ion is surrounded by six oxygen atoms and each oxygen ion is surrounded by four potassium atoms and two chlorine atoms.
Potassium Chlorate Solubility
KClO3 is moderately soluble in water, with a solubility of 7 g/100 mL of water at room temperature. The solubility of the compound increases with temperature, as the water molecules have more kinetic energy and can dissolve more of the compound. KClO3 is also soluble in other polar solvents such as ethanol and acetone.
| Appearance | White crystalline solid |
| Specific Gravity | 2.32 g/cm³ |
| Color | White |
| Odor | Odorless |
| Molar Mass | 122.55 g/mol |
| Density | 2.32 g/cm³ |
| Melting Point | 356 °C (673 °F) |
| Boiling Point | Decomposes before boiling |
| Flash Point | Not applicable |
| Water Solubility | 7 g/100 mL at 20 °C |
| Solubility | Soluble in ethanol and acetone |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| pKa | 1.8 (Ka = 1.6 × 10⁻⁵) |
| pH | pH of a 0.1 M solution is around 6.5-7.5 |
Potassium Chlorate Safety and Hazards
KClO3 is a highly reactive and potentially dangerous substance, so it should be handled with extreme care. It can cause severe skin and eye irritation and can be toxic if ingested or inhaled. When heated, it can undergo a violent reaction and even explode. KClO3 can also react strongly with other chemicals, such as sulfuric acid and organic compounds, and can produce toxic gases like chlorine and chlorate dioxide. It is important to follow proper safety protocols when working with KClO3, including wearing protective gear and working in a well-ventilated area.
| Hazard Symbols | O, Xi, N |
| Safety Description | Avoid contact with combustible material. Toxic if ingested. Causes severe skin burns and eye damage. |
| UN IDs | UN1485 |
| HS Code | 2829.90.10 |
| Hazard Class | 5.1 |
| Packing Group | II |
| Toxicity | Highly toxic |
Potassium Chlorate Synthesis Methods
There are several methods for synthesizing KClO3.
One method involves the reaction between potassium chloride and bleach. This method involves adding a solution of bleach to a solution of potassium chloride and stirring the mixture. To yield KClO3, filter and wash the resulting precipitate.
Another method involves the electrolysis of a solution containing potassium chloride, water, and a source of oxygen. An electrolytic cell, a specialized apparatus, carries out this process by separating potassium and chloride ions and producing oxygen gas. The oxygen reacts with the potassium ions to form KClO3.
A third method involves the reaction between potassium hydroxide and chlorine gas, which yields KClO3 along with potassium chloride and water. This method requires careful control of the temperature and concentration of the reactants to ensure optimal yields.
Potassium Chlorate Uses
KClO3 has a wide range of uses in various industries, including:
- Pyrotechnics: Commonly used as an oxidizing agent in fireworks and other pyrotechnic devices.
- Matches: Used in the heads of safety matches, which ignite when struck against a rough surface.
- Fertilizers: Used as a source of potassium for plant fertilizers.
- Bleaching agent: Used as a bleaching agent for textiles, paper, and other materials.
- Laboratory reagent: Also used as a laboratory reagent for a variety of chemical reactions.
- Medical applications: Used in medicine to treat some types of skin conditions, such as eczema.
- Explosives: Common ingredient in some types of explosives, such as blasting caps and dynamite.
- Oxidizer: Used as an oxidizing agent in the production of some chemicals, such as perchlorates.
Questions:
Q: How many grams of potassium chloride are produced if 25g of potassium chlorate decomposes?
A: When 25g of KClO3 decomposes, it produces 13.47g of potassium chloride.
Q: How to make potassium chlorate?
A: KClO3 can be made by reacting potassium chloride with bleach, by electrolysis of a solution containing potassium chloride, or by reacting potassium hydroxide with chlorine gas.
Q: How many moles of oxygen are produced when 2 mol of potassium chlorate (kclo3) decomposes?
A: When 2 mol of KClO3 decomposes, it produces 3 mol of oxygen gas.
Q: A 0.70 m solution contains 3.0 g of potassium chlorate (kclo3). What is the volume of the solution?
A: The volume of the 0.70 m solution containing 3.0 g of KClO3 is 51.4 mL.
Q: Is potassium chlorate volatile?
A: KClO3 is not considered to be a volatile substance, as it has a relatively high melting and boiling point.
Q: How much kcl is produced if you decompose 2.50 g of kclo3?
A: When 2.50 g of KClO3 decomposes, it produces 1.35 g of potassium chloride.
Q: Is kclo3 soluble in water?
A: Yes, KClO3 is highly soluble in water, with a solubility of 7 g/100 mL at room temperature.
Q: How many grams of oxygen can be produced from the decomposition of 100 g of kclo3?
A: When 100 g of KClO3 decomposes, it produces 45.02 g of oxygen gas.