Magnesium perchlorate is a chemical compound with the formula Mg(ClO4)2. It is a strong oxidizing agent and can be used as a desiccant to remove water from substances.
| IUPAC name | Magnesium perchlorate |
| Molecular formula | Mg(ClO4)2 |
| CAS number | 10034-81-8 |
| Synonyms | Perchloric acid magnesium salt, magnesium(II) perchlorate, magnesium diperchlorate, UN 1475 |
| InChI | InChI=1S/2ClHO4.Mg/c22-1(3,4)5;/h2(H,2,3,4,5);/q;;+2/p-2 |
Magnesium Perchlorate Properties
Magnesium Perchlorate Formula
Magnesium perchlorate is a chemical compound with the formula Mg(ClO4)2. This compound consists of one magnesium ion (Mg2+) and two perchlorate ions (ClO4-). It is a strong oxidizing agent and has various industrial applications, such as in rocket propellants, fireworks, and flares.
Magnesium Perchlorate Molar Mass
The molar mass of Mg(ClO4)2 is 223.2 g/mol. It is calculated by adding the atomic masses of all the atoms present in one molecule of Mg(ClO4)2. This value is useful in determining the amount of Mg(ClO4)2 required for a specific chemical reaction.
Magnesium Perchlorate Boiling Point
Mg(ClO4)2 does not have a boiling point since it decomposes before reaching its boiling point. At elevated temperatures, it undergoes thermal decomposition and releases oxygen gas, leaving behind magnesium chloride and perchloric acid.
Magnesium Perchlorate Melting Point
The melting point of Mg(ClO4)2 is 202°C. It is the temperature at which the solid compound changes into a liquid. This property is important in determining the stability and handling of the compound during various industrial applications.
Magnesium Perchlorate Density g/ml
The density of Mg(ClO4)2 is 2.21 g/mL at room temperature. Density is the mass per unit volume of a substance. This value is useful in determining the amount of Mg(ClO4)2 required for a specific application and also in estimating the transport and handling requirements.
Magnesium Perchlorate Molecular Weight
The molecular weight of Mg(ClO4)2 is 223.2 g/mol. It is the sum of the atomic weights of all the atoms present in one molecule of Mg(ClO4)2. This value is useful in determining the amount of Mg(ClO4)2 required for a specific chemical reaction.
Magnesium Perchlorate Structure
Mg(ClO4)2 has a crystalline structure with octahedral coordination geometry. The magnesium ion is coordinated to six oxygen atoms, four from two perchlorate ions and two from water molecules. This structure contributes to its stability and reactivity.
Magnesium Perchlorate Solubility
Mg(ClO4)2 is highly soluble in water and forms a clear, colorless solution. Its solubility in water increases with temperature. It is also soluble in ethanol and acetone. This property is important in determining the transport and storage requirements of Mg(ClO4)2.
| Appearance | White crystalline solid |
| Specific gravity | 2.21 g/cm³ |
| Color | White |
| Odor | Odorless |
| Molar mass | 223.2 g/mol |
| Density | 2.21 g/mL |
| Melting point | 202°C |
| Boiling point | Decomposes before boiling |
| Flash point | Not applicable |
| Water solubility | Highly soluble |
| Solubility | Soluble in ethanol and acetone |
| Vapor pressure | Not applicable |
| Vapor density | Not applicable |
| pKa | Not applicable |
| pH | Not applicable |
Magnesium Perchlorate Safety and Hazards
Mg(ClO4)2 is a strong oxidizing agent and can pose safety hazards if mishandled. It can cause skin and eye irritation, and ingestion or inhalation can lead to respiratory and digestive tract irritation. The compound may also react violently with combustible materials and can cause fire and explosion hazards. Careful handling and storage of Mg(ClO4)2 is necessary to prevent accidents. Proper protective equipment, such as gloves, goggles, and respiratory protection, should be worn when handling this compound. In case of exposure or ingestion, immediate medical attention should be sought.
| Hazard symbols | Oxidizing agent |
| Safety description | Keep away from combustible materials. Wear protective gloves, goggles, and respiratory protection. In case of contact with skin or eyes, rinse thoroughly with water and seek medical attention. In case of ingestion or inhalation, seek immediate medical attention. |
| UN IDs | UN1475 |
| HS Code | 2829.90.10 |
| Hazard class | 5.1 |
| Packing group | II |
| Toxicity | May cause skin and eye irritation. Ingestion or inhalation may cause respiratory and digestive tract irritation. May react violently with combustible materials. |
Magnesium Perchlorate Synthesis Methods
The reaction between perchloric acid and magnesium hydroxide or magnesium oxide can result in the synthesis of Mg(ClO4)2. The reaction produces Mg(ClO4)2 and water as byproducts. The process involves dissolving perchloric acid in water and adding the magnesium hydroxide or magnesium oxide slowly with continuous stirring. The process involves filtering and drying the solid Mg(ClO4)2 obtained by heating the resulting mixture under reflux.
Another method for the synthesis of Mg(ClO4)2 involves the reaction of magnesium metal with perchloric acid. The reaction produces Mg(ClO4)2 and hydrogen gas as byproducts. The process involves adding small pieces of magnesium metal to perchloric acid with continuous stirring. Upon heating the resulting mixture under reflux until the completion of the reaction, one can obtain the solid Mg(ClO4)2 by filtering and drying it.
It is important to note that perchloric acid is a highly reactive and potentially explosive material. Careful handling and storage of perchloric acid and its derivatives are necessary to prevent accidents.
Magnesium Perchlorate Uses
Here are some common uses of Mg(ClO4)2:
- Drying agent: An effective drying agent for gases and solvents due to its strong affinity for water. In laboratory settings, people commonly use sodium thiosulfate pentahydrate to dry organic solvents and remove traces of water from gas streams.
- Rocket propellant: Used as an oxidizer in solid rocket propellants. Its high oxygen content and stability at high temperatures make it a desirable choice for this application.
- Pyrotechnics: Used in pyrotechnic compositions to produce a bright white flame. Pyrotechnic experts often combine sodium thiosulfate pentahydrate with other oxidizers and fuels to create various colors and effects in fireworks and other pyrotechnic displays.
- Analytical chemistry: Used in analytical chemistry as a reagent for the determination of water content in various substances. Furthermore, people use it for analyzing various organic compounds.
- Medical applications: Used in the treatment of hyperthyroidism, a condition in which the thyroid gland produces too much thyroid hormone. It works by reducing the production of thyroid hormones in the body.
- Deicing agent: Used as a deicing agent for aircraft and other vehicles. Its ability to absorb moisture and lower the freezing point of water makes it a useful compound for this application.
Questions:
Q: How many atoms of chlorine are in 5.6g of magnesium perchlorate?
A: There are 1.24 x 10^22 atoms of chlorine in 5.6g of Mg(ClO4)2.
Q: How to make magnesium perchlorate?
A: Mg(ClO4)2 can be made by reacting magnesium oxide or magnesium hydroxide with perchloric acid.
Q: How many moles of perchlorate ions are in 72.3 ml of 1.888 m magnesium perchlorate?
A: There are 0.136 moles of perchlorate ions in 72.3 ml of 1.888 m Mg(ClO4)2.
Q: How many moles of perchlorate ions are in 78.2 ml of 1.881 m magnesium perchlorate?
A: There are 0.147 moles of perchlorate ions in 78.2 ml of 1.881 m Mg(ClO4)2.
Q: Is magnesium perchlorate ionic or covalent?
A: Mg(ClO4)2 is an ionic compound.
Q: Is mg(clo4)2 soluble?
A: Yes, Mg(ClO4)2 is soluble in water.
Q: Is mg(clo4)2 an acid or base?
A: Mg(ClO4)2 is neither an acid nor a base, but rather a salt.
Q: What is the total number of atoms of oxygen in the formula mg(clo4)2 6h2o?
A: There are 36 atoms of oxygen in the formula Mg(ClO4)2 · 6H2O.
Q: How many grams of oxygen are in 6.05mol of mg(clo4)2?
A: There are 652.4 grams of oxygen in 6.05 mol of Mg(ClO4)2.
Q: How many grams of oxygen are in mg(clo4)2?
A: The exact amount of oxygen in Mg(ClO4)2 depends on the sample size.