Ammonium hydroxide: Difference between revisions
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* Feedstock for [[ammonium chloride]] and most amines. | * Feedstock for [[ammonium chloride]] and most amines. | ||
* Solvent | * Solvent | ||
===Secondary=== | |||
* Antibacterial | * Antibacterial | ||
* Fertilizer | * Fertilizer | ||
==Natural occurrence== | ==Natural occurrence== | ||
* Occurs naturally in the effluent of birds, fish, and rodents. | * Occurs naturally in the effluent of birds, fish, and rodents. | ||
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* Directly from excrement | * Directly from excrement | ||
===Synthesis=== | ===Synthesis=== | ||
====From urea==== | |||
* Action of [[urease]] upon [[urea]], usually in an aqueous environment at raised temperature. | * Action of [[urease]] upon [[urea]], usually in an aqueous environment at raised temperature. | ||
*: {{#Chem: (NH2)2CO + 3H2O → CO2 + 2NH3OH}} | *: {{#Chem: (NH2)2CO + 3H2O → CO2 + 2NH3OH}} | ||
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* Airtight containers | * Airtight containers | ||
==Disposal== | ==Disposal== | ||
* Small | * Small amounts of dilute [[ammonium hydroxide]] may be disposed of directly into soil. | ||
* Disposal directly into waterways is hazardous to indigenous aquatic life. | * Disposal directly into waterways is hazardous to indigenous aquatic life. | ||
==See Also== | ==See Also== | ||
* [[Ammonia]] | |||
==References== | ==References== | ||
<references/> | <references/> | ||
Latest revision as of 05:41, 12 December 2019
| Chemical formula | NH4OH |
|---|---|
| OTP appearance | colorless liquid |
| Molar Mass(g/mol) | 35.04 |
| Enthalpy of Formation(kJ/mol) | -80 |
| Density(g/cc) | 0.88-0.91 |
| Melting Point(°C) | -57.5 |
| Boiling Point(°C) | 37.7 |
| Solubility in water(g/L) | misc |
| NFPA 704 |  0
0
0
|
Uses
Primary
- Feedstock for ammonium chloride and most amines.
- Solvent
Secondary
- Antibacterial
- Fertilizer
Natural occurrence
- Occurs naturally in the effluent of birds, fish, and rodents.
Hazards
- Inhalation or consumption can be hazardous
Production
Extraction
- Directly from excrement
Synthesis
From urea
- Action of urease upon urea, usually in an aqueous environment at raised temperature.
- (NH2)2CO + 3 H2O → CO2 + 2 NH3OH
Testing
Purification
Ammonium hydroxide has a relatively high vapor pressure. Like all such compounds, it can be purified by air stripping to a suitable solvent. Solutions of ammonium hydroxide will "boil off" small amounts of pure ammonia into the environment. Open containers of pure distilled water will absorb the ammonia, producing ammonium hydroxide. Thus a container of ammonium hydroxide and a container of distilled water, both in a sealed environment, will approach an equilibrium of concentrations of ammonium hydroxide. Although this decreases the concentration, it also increases the purity by restricting impurities to those that can be dissolved in air. The balance can be further driven by increasing the alkalinity and/or temperature of the source material relative to the absorbing material.
Storage
- Airtight containers
Disposal
- Small amounts of dilute ammonium hydroxide may be disposed of directly into soil.
- Disposal directly into waterways is hazardous to indigenous aquatic life.