Difference between revisions of "Perchloric acid"
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===Disposal=== | ===Disposal=== | ||
| − | Perchloric acid and its compounds should not be released in the environment. | + | Perchloric acid and its compounds should not be released in the environment. Perchloric acid is best precipitated to the insoluble potassium perchlorate, which can then be mixed with a combustible material and burned. |
| + | |||
| + | Perchlorate salts can also be neutralized by using iron powder and UV light, under anaerobic conditions. | ||
==References== | ==References== | ||
Revision as of 14:41, 5 August 2018
| Names | |
|---|---|
| IUPAC name
Perchloric acid
| |
| Systematic IUPAC name
Chloric(VII) acid | |
| Other names
Hyperchloric acid
Hydrogen tetraoxochlorate(VII) Hydroperchlorate | |
| Properties | |
| HClO4 | |
| Molar mass | 100.46 g/mol |
| Appearance | Colorless liquid |
| Odor | Odorless |
| Density | 1.7703 g/cm3 (at 20 °C) |
| Melting point | −112 °C (−170 °F; 161 K) (anhydrous) −17 °C (1 °F; 256 K) (azeotrope) |
| Boiling point | 203 °C (397 °F; 476 K) (azeotrope) |
| Miscible | |
| Solubility | Reacts with amines Readily soluble in trifluoroacetic acid Insoluble in carbon tetrachloride |
| Vapor pressure | 29.35 mmHg (at 20 °C) |
| Acidity (pKa) | -15.2 (±2.0) ≈ −10 |
| Thermochemistry | |
| Std molar
entropy (S |
160-180 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-40.6 kJ/mol |
| Hazards | |
| Safety data sheet | BioExpress |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Hypochlorous acid Chlorous acid Chloric acid |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Perchloric acid is a strong inorganic acid with formula HClO4. At high concentrations it is a dangerously strong oxidizer, but at low concentrations it has little oxidizing potential.
Contents
Properties
Chemical
Perchloric acid is one of several strong acids, and is a potent oxidizer at high concentrations. It reacts with bases to form perchlorates. The addition of perchloric acid to a solution containing potassium ions will precipitate the poorly soluble potassium perchlorate out of the solution.
Physical
Perchloric acid is an oily liquid at room temperature. Like many other concentrated acids, samples of perchloric acid that are highly concentrated are also hygroscopic, absorbing moisture from the air. Perchloric acid forms an azeotrope with water at approximately 72.5% concentration that boils at 203°C. Its density is 1.67 g/cm3.
Perchloric acid, like many other mineral acids, comes in three typical concentrations: dilute (below 70%), concentrated (72.5%), and fuming (80-100%). Anhydrous (pure) perchloric acid is also used, although it is a very dangerous chemical. Each of these concentrations comes with its own set of hazards, although dilute is the safest.
Availability
Perchloric acid is available to concentrations up to ~70%, but its purchase requires paperwork and sometimes a business license, due to its strong explosive potential. Small amounts can be purchased from HMS Beagle.
Perchloric acid and its salts are restricted in the EU countries.
Preparation
Perchloric acid can be prepared by mixing a saturated solution of sodium perchlorate and hydrochloric acid. Sodium chloride will precipitate and perchloric acid will remain in solution. The acid can be concentrated up to its azeotrope by distillation. Silver perchlorate, if available can also be used.
Alternatively, a mixture of potassium perchlorate or calcium perchlorate, sulfuric acid, and water can be distilled. However, care must be taken to not let the concentration of perchloric acid in the distillate rise too high, especially since perchloric acid forms a negative azeotrope with water.
If you cannot or won't want to perform distillation, you can get perchloric acid by using barium perchlorate instead. Filter the insoluble barium sulfate to obtain conc. perchloric acid.
Perchloric acid can also be made by boiling down a solution of chloric acid. Heat and dehydration decompose chloric acid, cause it to release toxic fumes of hydrochloric and perchloric acid, which condense on a cold surface.
Projects
- Make bis(ethylenediamine)copper(II) perchlorate
- Ammonium perchlorate synthesis
- Dichlorine heptoxide preparation
- Ammonium perchlorate preparation
- Chromium etching[1]
Handling
Safety
Perchloric acid is a strong acid, and when concentrated is a dangerous oxidizer capable of exploding violently in contact with organic compounds. Anhydrous or fuming perchloric acid is known to spontaneously detonate. Aqueous solutions up to 70% are safe to handle and store however. The azeotropic (concentrated) acid is mostly safe under normal conditions. Additionally, perchlorate is toxic to the thyroid.
The biggest hazard in working with perchloric acid are its fumes. Normal fume hoods are insufficient in dealing with them, as the vapors will react with the construction materials and when they build up, there is a serious risk of explosion. Special fume hoods with washing down capabilities are mandatory when working with perchloric acid, to prevent accumulation of perchlorates in the ductwork.
Storage
Perchloric acid is safe to store at concentrations lower than 70%. It must be kept away from any organic vapors and metals. Glass bottles with Teflon seal cap are suitable for storing this dangerous reagent.
Disposal
Perchloric acid and its compounds should not be released in the environment. Perchloric acid is best precipitated to the insoluble potassium perchlorate, which can then be mixed with a combustible material and burned.
Perchlorate salts can also be neutralized by using iron powder and UV light, under anaerobic conditions.
