Calcium chlorate (Ca(ClO3)2) is a chemical compound composed of calcium, chlorine, and oxygen. It is commonly used as an oxidizing agent in fireworks and matches. It can also be used to sterilize equipment in the food industry.
| IUPAC Name | Calcium chlorate |
| Molecular Formula | Ca(ClO3)2 |
| CAS Number | 10137-74-3 |
| Synonyms | Chloric acid, calcium salt; Calcium chlorate hydrate; Calciumperchlorate; Calciochlorite; UN1456 |
| InChI | InChI=1S/Ca.2ClHO3/c;22-1(3)4/h;2(H,2,3,4)/q+2;;/p-2 |
Calcium Chlorate Properties
Calcium Chlorate Formula
The formula for calcium chlorate is Ca(ClO3)2. It is composed of one Ca2+ ion and two ClO3- ions. Calcium chlorate is an ionic compound, meaning that it is held together by electrostatic attraction between the positive and negative ions.
Calcium Chlorate Molar Mass
The molar mass of Ca(ClO3)2 is 206.98 g/mol. This can be calculated by adding the atomic masses of calcium, chlorine, and oxygen, which make up the compound. The molar mass is important in calculating the amount of Ca(ClO3)2 needed for a given reaction.
Calcium Chlorate Boiling Point
Ca(ClO3)2 does not have a boiling point as it decomposes before it reaches its boiling point. When heated, Ca(ClO3)2 breaks down into calcium chloride (CaCl2) and oxygen gas (O2). This decomposition is exothermic and can be dangerous if not handled properly.
Calcium Chlorate Melting Point
The melting point of Ca(ClO3)2 is 135°C. This is the temperature at which the solid compound changes from a solid to a liquid. Ca(ClO3)2 is a white crystalline solid at room temperature and pressure.
Calcium Chlorate Density g/mL
The density of Ca(ClO3)2 is 2.4 g/mL. This means that one milliliter of Ca(ClO3)2 weighs 2.4 grams. The density is a measure of how tightly packed the molecules are in a substance. Ca(ClO3)2 is denser than water, which has a density of 1 g/mL.
Calcium Chlorate Molecular Weight
The molecular weight of Ca(ClO3)2 is 206.98 g/mol. This is the same as the molar mass and can be calculated by adding the atomic weights of the individual elements in the compound.
Calcium Chlorate Structure
Ca(ClO3)2 has a crystal lattice structure, which is typical for ionic compounds. In this structure, the Ca2+ ions and ClO3- ions are arranged in a regular, repeating pattern. Each Ca2+ ion is surrounded by six ClO3- ions, and each chlorate ion is surrounded by six calcium ions.
Calcium Chlorate Solubility
Ca(ClO3)2 is soluble in water and forms a clear, colorless solution. The solubility of Ca(ClO3)2 in water increases with temperature. However, it is less soluble in organic solvents such as ethanol and acetone. Ca(ClO3)2 is also hygroscopic, meaning that it absorbs moisture from the air. This can cause the compound to become damp or dissolve over time.
| Appearance | White crystalline solid |
| Specific Gravity | 2.4 |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 206.98 g/mol |
| Density | 2.4 g/mL |
| Melting Point | 135°C |
| Boiling Point | Decomposes before boiling point |
| Flash Point | Not applicable |
| Water Solubility | Soluble |
| Solubility | Soluble in water, less soluble in organic solvents |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| pKa | Not applicable |
| pH | Not applicable |
Calcium Chlorate Safety and Hazards
Ca(ClO3)2 is considered a hazardous substance and should be handled with care. It is an oxidizing agent and can react violently with organic materials, causing fires and explosions. Inhalation or ingestion of Ca(ClO3)2 can cause respiratory and gastrointestinal irritation. Prolonged exposure can lead to skin irritation, burns, and possible allergic reactions. It is important to wear appropriate personal protective equipment when handling Ca(ClO3)2, including gloves, goggles, and a respirator. In case of exposure, seek medical attention immediately. Store Ca(ClO3)2 in a cool, dry, well-ventilated area away from incompatible substances.
| Hazard Symbols | O, Xn |
| Safety Description | Keep away from organic materials. Wear personal protective equipment. Store in a cool, dry, well-ventilated area. |
| UN IDs | UN1458 |
| HS Code | 2829.11.00 |
| Hazard Class | 5.1 |
| Packing Group | II |
| Toxicity | Toxic if ingested or inhaled. May cause skin and eye irritation. May cause respiratory irritation. |
Calcium Chlorate Synthesis Methods
To synthesize Ca(ClO3)2, one can use various methods.
One common method involves the reaction of calcium hydroxide with chlorine gas. In this process, calcium chloride is first formed as a byproduct, which reacts with the remaining chlorine to form Ca(ClO3)2.
Another method involves the reaction of calcium carbonate with nitric acid and chlorine gas. To obtain Ca(ClO3)2, one evaporates and crystallizes the resulting solution.
Another approach involves the electrolysis of a solution containing calcium chloride and sodium chlorate. This process yields Ca(ClO3)2 and sodium chloride as the final products.
The reaction between calcium hypochlorite and sodium chlorate produces Ca(ClO3)2, which is then purified and crystallized.
Calcium Chlorate Uses
Ca(ClO3)2 has several important uses in various industries. Here are some of the most common applications of Ca(ClO3)2:
- Bleaching Agent: Used as a bleaching agent in the pulp and paper industry.
- Fireworks: A common oxidizing agent used in the production of fireworks.
- Matches: Also used in the production of safety matches, as it can be easily ignited.
- Herbicides: Used as a herbicide, as it can selectively kill certain weeds without harming crops.
- Oxidizing Agent: Used as an oxidizing agent in the production of other chemicals, such as perchlorates and chlorates.
- Pharmaceuticals: Also used in the production of pharmaceuticals, such as anti-infective drugs.
- Laboratory Reagent: Used as a laboratory reagent for analytical chemistry.
- Pigment Production: Used in the production of pigments, such as ultramarine blue.
Questions:
Q: What is the formula for calcium chlorate?
A: The chemical formula for calcium chlorate is Ca(ClO3)2.
Q: What is calcium chlorate used for?
A: Ca(ClO3)2 has various applications in industries, such as bleaching agent in the pulp and paper industry, oxidizing agent in the production of other chemicals, herbicide, pigment production, and laboratory reagent.
Q: Is calcium chlorate a solid?
A: Yes, Ca(ClO3)2 is a solid at room temperature.
Q: Where is sodium chlorate most commonly found and what is calcium chlorate used for?
A: Sodium chlorate is most commonly found in the chemical industry, where it is used as an oxidizing agent and a herbicide. Ca(ClO3)2, on the other hand, is used as a bleaching agent, oxidizing agent, and herbicide in various industries.
Q: What is the total number of atoms in the compound Ca(ClO3)2?
A: The compound Ca(ClO3)2 has a total of 13 atoms – 1 calcium atom, 2 chlorine atoms, and 6 oxygen atoms from the two ClO3- ions.
Q: What is the percent by mass of chlorine in Ca(ClO3)2?
A: The atomic mass of chlorine is 35.5 g/mol and the molar mass of Ca(ClO3)2 is 238.98 g/mol. Therefore, the percent by mass of chlorine in Ca(ClO3)2 is (2 x 35.5 g/mol) / 238.98 g/mol x 100% = 29.68%.
Q: How many chlorine atoms are in Ca(ClO3)2?
A: There are two chlorine atoms in Ca(ClO3)2, represented by the two ClO3 groups.
Q: What is the mass of each compound in the original mixture Ca(ClO3)2 and Ca(ClO)2?
A: It is impossible to determine the mass of each compound in the original mixture without additional information, such as the total mass or the mass ratio between the two compounds.