Difference between revisions of "Potassium bifluoride"
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Potassium bifluoride can be purchased from glass Manufacturers and chemical companies. | Potassium bifluoride can be purchased from glass Manufacturers and chemical companies. | ||
==Preparation== | ==Preparation== | ||
| − | Reaction of | + | Reaction of anhydrous [[Hydrogen fluoride]] with [[Potassium hydroxide]] yields Potassium bifluoride. Concentrated [[Hydrofluoric acid]] can also be reacted with [[Potassium hydroxide]] to produce Potassium bifluoride but an extra purification step is required to remove Potassium fluoride formed as a reaction product. |
| − | + | ||
==Projects== | ==Projects== | ||
*Make elemental [[Fluorine]] | *Make elemental [[Fluorine]] | ||
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===Disposal=== | ===Disposal=== | ||
| − | Potassium bifluoride should not be poured down the drain because fluoride ions are quite toxic | + | Potassium bifluoride should not be poured down the drain because fluoride ions at higher concentrations are quite toxic for the environment. It can be recycled for fluoride ions or should be given to a specific authority for its safe disposal. |
==References== | ==References== | ||
Revision as of 21:19, 19 August 2025
| Names | |
|---|---|
| IUPAC name
Potassium hydrogen difluoride
| |
| Properties | |
| K[HF2] | |
| Molar mass | 78.103 g/mol |
| Appearance | White crystalline solid |
| Odor | Slightly acidic |
| Density | 2.37 g/cm3 |
| Melting point | 238.7 °C (461.7 °F; 511.8 K) |
| 39.2 g/100 ml (20 °C) | |
| Solubility | Soluble in ethanol |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Flash point | Non-flammable |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Potassium bifluoride is a salt with the formula K[HF2]. It is a white crystalline solid, it is hygroscopic in nature, and has slight acidic odour to it.
Contents
Properties
Potassium bifluoride (KHF₂) is a white, crystalline solid that is highly soluble in water. It has a melting point of 238.7°C and decomposes before boiling. It is mildly acidic in solution due to the release of hydrofluoric acid.
Availability
Potassium bifluoride can be purchased from glass Manufacturers and chemical companies.
Preparation
Reaction of anhydrous Hydrogen fluoride with Potassium hydroxide yields Potassium bifluoride. Concentrated Hydrofluoric acid can also be reacted with Potassium hydroxide to produce Potassium bifluoride but an extra purification step is required to remove Potassium fluoride formed as a reaction product.
Projects
- Make elemental Fluorine
- Etching glass
Handling
Safety
Potassium bifluoride should be handled carefully with gloves and a suitable respirator as this substance is quite irritating to the nose and the skin. If ingested fluoride ions can become quite poisonous. Potassium bifluoride should not be heated above its melting point as this may lead to decomposition of the salt and formation of highly corrosive Hydrogen fluoride gas and Potassium fluoride.
Storage
Potassium bifluoride should be stored in an airtight container (preferably a desiccator) since its hygroscopic.
Disposal
Potassium bifluoride should not be poured down the drain because fluoride ions at higher concentrations are quite toxic for the environment. It can be recycled for fluoride ions or should be given to a specific authority for its safe disposal.
