14866-68-3

Basic information

• Product Name: chloric acid
• Synonyms: Chlorate(1-);Chlorine oxide (clo3(1-))
• CAS NO: 14866-68-3
• Molecular Formula: ClO₃
• Molecular Weight: 83.45
• EINECS: 232-233-0
• Mol File: 14866-68-3.mol
• Article Data: 27

Chemical Properties

• Boiling Point: °Cat760mmHg
• Flash Point: °C
• Appearance: /
• Density: g/cm³
• CAS DataBase Reference: chloric acid(CAS DataBase Reference)
• NIST Chemistry Reference: chloric acid(14866-68-3)
• EPA Substance Registry System: chloric acid(14866-68-3)

Safety Data

• Hazardous Substances Data: 14866-68-3(Hazardous Substances Data)

Usage

Description

Chloric acid, also known as chlorate, is an inorganic compound that appears as a white crystalline substance. It is soluble in water and exhibits noncombustible properties. However, it can form a highly flammable mixture with combustible materials, which may become explosive if the combustible material is finely divided. The mixture can be ignited by friction, and contact with strong sulfuric acid can lead to fires or explosions. When mixed with ammonium salts, spontaneous decomposition and ignition may occur. Prolonged exposure to heat or fire can result in an explosion.

Uses

Used in Chemical Industry:
Chloric acid is used as a strong oxidizing agent for various chemical reactions, taking advantage of its ability to form explosive mixtures with combustible materials when finely divided. This property makes it useful in the production of certain chemicals and compounds.
Used in Fireworks Industry:
Due to its explosive nature when mixed with combustible materials, chloric acid can be used as a component in the manufacturing of fireworks and pyrotechnics. The controlled use of its explosive properties contributes to the visual and auditory effects of these products.
Used in Mining Industry:
Chloric acid's strong oxidizing properties make it suitable for use in the mining industry, particularly in the extraction of certain metals. Its ability to react with other substances can aid in the separation and purification processes of valuable minerals.
Used in Water Treatment:
Chloric acid can be utilized in water treatment processes as a disinfectant and oxidizing agent. Its ability to react with contaminants can help purify water and make it safe for various applications.
Used in Safety and Security:
The explosive properties of chloric acid can be harnessed for safety and security purposes, such as in the development of explosive devices for controlled demolitions or in the creation of safety systems that rely on controlled explosions to prevent accidents or protect against threats.

Air & Water Reactions

They are soluble in water.

Reactivity Profile

Metal chlorates are oxidants in the presence of strong acid; liberates explosive chlorine dioxide gas; liberates chlorine dioxide and carbon dioxide by heating a moist metal chlorate and a dibasic organic acid; mixtures of perchlorates with sulfur or phosphorus are explosives [Bretherick 1979 p. 100]; mixtures of the chlorate with ammonium salts, powdered metals, silicon, sulfur, or sulfides are readily ignited and potentially explosive [Bretherick 1979 p. 806]. A combination of finely divided aluminum with finely divided bromates (also chlorates and iodates) of barium, calcium, magnesium, potassium, sodium, or zinc can explode by heat, percussion, or friction [Mellor 2:310 1946-47].

Health Hazard

Inhalation, ingestion or contact (skin, eyes) with vapors or substance may cause severe injury, burns or death. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may cause pollution.

Fire Hazard

These substances will accelerate burning when involved in a fire. Some may decompose explosively when heated or involved in a fire. May explode from heat or contamination. Some will react explosively with hydrocarbons (fuels). May ignite combustibles (wood, paper, oil, clothing, etc.). Containers may explode when heated. Runoff may create fire or explosion hazard.

InChI:InChI=1/ClHO3/c2-1(3)4/h(H,2,3,4)/p-1

Upstream product

• 7758-19-2 sodium chlorite 
• 10028-15-6 ozone 
• 7601-90-3 perchloric acid 
• 3811-04-9 potassium chlorate 
• 7647-14-5 sodium chloride 
• 14336-71-1 calcium chloride 
• 16887-00-6 chloride 
• 7791-07-3 sodium perchlorate monohydrate 
• 14989-30-1 hypochloric acid 
• 7681-52-9 sodium hypochlorite 
• 10049-04-4 chlorine dioxide 
• 7553-56-2 iodine 
• 7732-18-5 water 
• 14265-45-3 sulfite^(2-) 

Downstream Products

• 16887-00-6 chloride 
• 15454-31-6 iodate 
• 7789-31-3 bromic acid 
• 7601-90-3 perchloric acid 
• 7790-93-4 chloric acid 
• 7782-50-5 chlorine 
• 7553-56-2 iodine 
• 7790-99-0 Iodine monochloride 
• 13598-36-2 phosphonic Acid 
• 10028-15-6 ozone 
• 14797-73-0 perchlorate^(1-) 
• 14362-44-8 iodide 
• 865-44-1 iodine trichloride 
• 10049-04-4 chlorine dioxide 

Relevant articles and documents

Hypohalite ion catalysis of the disproportionation of chlorine dioxide

The disproportionation of chlorine dioxide in basic solution to give ClO2- and ClO3- is catalyzed by OBr- and OCl-. The reactions have a first-order dependence in both [ClO2] and [OX-] (X = Br, Cl) when the ClO2- concentrations are low. However, the reactions become second-order in [ClO2] with the addition of excess ClO2-, and the observed rates become inversely proportional to [ClO2-]. In the proposed mechanisms, electron transfer from OX- to ClO2 (k1OBr- = 2.05 ± 0.03 M-1 s-1 for OBr-/ClO2 and k1OCl- = 0.91 ± 0.04 M-1 s-1 for OCl-/ClO2) occurs in the first step to give OX and ClO2-. This reversible step (k1OBr-/k-1OBr- = 1.3 × 10-7 for OBr-/ClO2, k1OCl-/k-1OCl = 5.1 × 10-10 for OCl-/ClO2) accounts for the observed suppression by ClO2-. The second step is the reaction between two free radicals (XO and ClO2) to form XOClO2. These rate constants are k2OBr = 1.0 × 108 M-1 s-1 for OBr/ClO2 and k2OCl = 7 × 109 M-1 s-1 for OCl/ClO2. The XOClO2 adduct hydrolyzes rapidly in the basic solution to give ClO3- and to regenerate OX-. The activation parameters for the first step are ΔH1? = 55 ± 1 kJ mol-1, ΔS1? = - 49 ± 2 J mol-1 K-1 for the OBr-/ClO2 reaction and ΔH1? = 61 ± 3 kJ mol-1, ΔS1? = - 43 ± 2 J mol-1 K-1 for the OCl-/ClO2 reaction.

Kinetics and mechanism of catalytic decomposition and oxidation of chlorine dioxide by the hypochlorite ion

The oxidation of ClO2 by OCl-is first order with respect to both reactants in the neutral to alkaline pH range: -d[ClO2]/dt = 2kOCl[ClO2][OCl-]. The rate constant (T = 298 K, μ = 1.0 M NaCl

Two-dimensional cluster catalysts with superior thermal stability and catalytic activity for AP

The preparation of catalysts with small particle size, large specific surface area and high atomic utilization has always been the focus of research in the field of catalysis. As for energetic materials, catalysts are always used to improve the thermal decomposition performance of ammonium perchlorate (AP) as it has significant effect on the power of engine. In this work, a two-dimensional metal clusters catalyst has been successfully prepared by solvothermal and heat treatment to improve thermal decomposition performance of AP. In detail, the transition metal ions were supported on the graphene oxide (GO) surface by organic ligands linking, followed by heat treatment to obtain two-dimensional rGO based metal clusters catalyst. The morphology and structure of the catalysts at different temperatures and their effect on AP decomposition were studied, the results show that catalyst at 300 °C has a particle size of 20 nm and uniformly distributed on rGO. The catalyst promotes the high temperature decomposition of AP by 73.7 °C with improved stability, and increases the heat release from 652.73 J/g to 1392.11 J/g. This may be attributed to good conductivity of GO and the strong gain-loss electron ability of the metal clusters. The presence of GO increased the active sites for cluster catalysis, additional, the metal clusters have a positive synergistic effect with GO. Thus, the thermal decomposition performance of AP was enhanced meanwhile thermal stability can also be improved.

Kinetics and Mechanism of the Chlorite-Periodate System: Formation of a Short-Lived Key Intermediate OClOIO3 and Its Subsequent Reactions

The chlorite-periodate reaction has been studied spectrophotometrically in acidic medium at 25.0 ± 0.1 °C, monitoring the absorbance at 400 nm in acetate/acetic acid buffer at constant ionic strength (I = 0.5 M). We have shown that periodate was exclusive