Chloric acid (HClO3) is a strong and unstable acid that can be produced by mixing chlorine dioxide with water. It is used in bleaching and disinfecting agents, and in the production of explosives.
| IUPAC Name | Chloric acid |
| Molecular Formula | HClO3 |
| CAS Number | 7790-93-4 |
| Synonyms | Perchloric acid, chlorate; Chloric acid solution; Chloric(V) acid; Hydrogen chlorate; Hydrogen trichlorate |
| InChI | InChI=1S/ClHO3/c2-1(3)4/h(H,2,3,4) |
The properties of Chloric acid (HClO3) are of significant interest to chemists and engineers because of its many industrial applications.
HClO3 Lewis structure
The Lewis structure of HClO3 shows that chlorine is the central atom bonded to three oxygen atoms and one hydrogen atom. Chlorine has 7 valence electrons, and each oxygen has 6 valence electrons. The structure includes three single bonds and one double bond between chlorine and oxygen atoms.
Chloric acid (HClO3) formula
The chemical formula of Chloric acid (HClO3) is HClO3. It is an inorganic acid that contains one chlorine atom, one hydrogen atom, and three oxygen atoms. The formula of Chloric acid (HClO3) is used to calculate the stoichiometry and concentration of solutions containing the acid.
Chloric acid (HClO3) molar mass
The molar mass of Chloric acid (HClO3) is 84.46 g/mol. It is a relatively lightweight acid compared to other inorganic acids, such as sulfuric acid, which has a molar mass of 98.08 g/mol. The molar mass of Chloric acid (HClO3) is an important parameter in calculating the concentration and stoichiometry of solutions containing the acid.
Chloric acid (HClO3) boiling point
Chloric acid (HClO3) has a boiling point of 40.5°C. It is a highly volatile acid that can decompose at high temperatures, which makes it difficult to handle and store. The low boiling point of Chloric acid (HClO3) is an important consideration in designing equipment and processes that involve the use of the acid.
Chloric acid (HClO3) melting point
Chloric acid (HClO3) does not have a well-defined melting point. It can decompose before it reaches a melting point, releasing oxygen gas and leaving behind a residue of chlorates. The lack of a distinct melting point is due to the instability of Chloric acid (HClO3).
Chloric acid (HClO3) density g/ml
The density of Chloric acid (HClO3) is 1.97 g/cm³. It is a relatively dense acid compared to other inorganic acids, such as hydrochloric acid, which has a density of 1.18 g/cm³. The high density of Chloric acid (HClO3) is an important consideration in designing processes that involve the handling and transportation of the acid.
Chloric acid (HClO3) molecular weight
The molecular weight of Chloric acid (HClO3) is 84.46 g/mol. It is the sum of the atomic weights of its constituent elements: one chlorine atom, one hydrogen atom, and three oxygen atoms. The molecular weight of Chloric acid (HClO3) is an important parameter in calculating the concentration and stoichiometry of solutions containing the acid.
Chloric acid (HClO3) structure
The structure of Chloric acid is composed of one central chlorine atom bonded to three oxygen atoms and one hydrogen atom. The molecule has a tetrahedral geometry, with the chlorine atom at the center of the tetrahedron. The three oxygen atoms are arranged around the chlorine atom in a trigonal planar arrangement, while the hydrogen atom is bonded to one of the oxygen atoms. The structure of Chloric acid (HClO3) is important in understanding its chemical properties and reactivity.
| Appearance | Clear or yellowish liquid |
| Specific Gravity | 1.97 |
| Color | Colorless to yellow |
| Odor | Odorless |
| Molar Mass | 84.46 g/mol |
| Density | 1.68 g/cm³ |
| Melting Point | Decomposes before melting |
| Boiling Point | 40.5°C |
| Flash Point | Not applicable |
| Water Solubility | Miscible |
| Solubility | Soluble in most organic solvents |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| PKa | -0.6 |
| PH | <1 |
Chloric Acid (HClO3) Safety and Hazards
Chloric acid (HClO3) poses several safety hazards and should be handled with care. It is a strong oxidizer and can react violently with many organic materials, including fuels, reducing agents, and flammable liquids. It can cause severe burns to the skin and eyes upon contact and can be corrosive to metal surfaces. Inhaling its vapors can cause respiratory irritation and coughing. Due to its reactive nature, it should be stored and handled in a well-ventilated area away from other chemicals. Protective equipment, such as gloves, goggles, and a respirator, should be worn when handling chloric acid to prevent exposure. In case of skin or eye contact, immediate medical attention should be sought.
| Hazard Symbols | Oxidizing Agent |
| Safety Description | Avoid contact with skin and eyes; wear protective equipment |
| UN Ids | UN 3084 |
| HS Code | 2811.19 |
| Hazard Class | 5.1 |
| Packing Group | II |
| Toxicity | Corrosive; can cause severe burns to skin and eyes |
Chloric Acid (HClO3) Synthesis Methods
Chloric acid can be synthesized through several methods, including the reaction of chlorine gas with sodium hydroxide or sodium chlorate. One common method is the reaction of sodium chlorate with hydrochloric acid.
The synthesis reaction of chloric acid involves the reaction of sodium chlorate (NaClO3) with hydrochloric acid (HCl) in a two-step process. The first step involves the conversion of sodium chlorate to sodium chlorite (NaClO2) and chlorine dioxide (ClO2) gas in the presence of an acid catalyst. In the second step, the chlorine dioxide gas reacts with excess hydrochloric acid to form chloric acid and chlorine gas.
Another method for synthesizing chloric acid involves the electrolysis of a solution containing sodium chloride, nitric acid, and sulfuric acid. This process produces chlorine gas, which reacts with water to form chloric acid.
To produce chloric acid, one can react potassium chlorate with sulfuric acid and then distill the resulting mixture.
The synthesis of chloric acid requires careful handling of the reactants due to the potential for violent reactions and the corrosive nature of the acids involved. It is important to follow appropriate safety protocols and handle the materials in a well-ventilated area using proper protective equipment.
Chloric Acid (HClO3) Uses
Chloric acid (HClO3) has several applications in various industries due to its strong oxidizing properties. Some of its uses are:
- Other chemicals production: Chloric acid serves as an intermediate in producing other chemicals, including perchloric acid, chlorates, and perchlorates.
- Bleaching agent: The pulp and paper industry uses chloric acid as a bleaching agent.
- Disinfectant: Chloric acid acts as a disinfectant in the food and beverage industry to sanitize equipment and surfaces.
- Etching agent: The semiconductor industry uses chloric acid as an etching agent to remove unwanted material layers from semiconductor wafers.
- Laboratory reagent: Chloric acid is used as a laboratory reagent in analytical chemistry and organic synthesis.
- Oxidizing agent: Chloric acid is utilized as an oxidizing agent in organic chemistry reactions.
- Rocket propellant: Chloric acid serves as an oxidizer in rocket propellants.
- Water treatment: Chloric acid is used in water treatment to control the growth of algae and bacteria.
Questions:
Q: Is chloric acid a strong acid?
A: Yes, chloric acid (HClO3) is a strong acid.
Q: Which formula represents chloric acid?
A: The formula for chloric acid is HClO3.
Q: Explain why HCl is hydrochloric acid and HClO3 is chloric acid?
A: The names of binary acids (compounds that contain only two elements) are typically derived from the name of the anion, with the suffix -ic for the most common anion and -ous for the less common one. In the case of HCl, the anion is chloride (Cl-), so the acid is named hydrochloric acid. In the case of HClO3, the anion is chlorate (ClO3-), so the acid is named chloric acid.
Q: What is the formula for chloric acid?
A: The formula for chloric acid is HClO3.
Q: Is chloric acid ionic or molecular?
A: Chloric acid is molecular, as it consists of covalently bonded atoms of hydrogen, chlorine, and oxygen.