Sodium carbonate: Difference between revisions
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===Synthesis=== | ===Synthesis=== | ||
====From sodium bicarbonate==== | ====From sodium bicarbonate==== | ||
* Heat [[sodium bicarbonate]] to | * Heat [[sodium bicarbonate]] to 200°C to rapidly decompose it to sodium carbonate and water | ||
*: {{#Chem: 2NaHCO3 { ≥ | *: {{#Chem: 2NaHCO3 { ≥200°C --> } Na2CO3 + CO2 + H2O}} | ||
==Purification== | ==Purification== | ||
==Testing== | ==Testing== | ||
Revision as of 09:46, 22 April 2020
| Chemical formula | Na2CO3 |
|---|---|
| Molar Mass(g/mol) | 106 |
| Density(g/cc) | 2.54 |
| Melting Point(°C) | 851 |
| Boiling Point(°C) | 1600 |
| Solubility in water(g/L) | 251 |
| Solubility in ethanol(g/L) | insoluble |
| NFPA 704 |  0
1
1
|
| Thermal decomposition of Sodium carbonate | |
| 33.5 | 10-hydrate
33.5°C 7-hydrate |
| 40 | 7-hydrate
40°C hydrate |
| 100 | hydrate
100°C anhydrous |
Uses
Primary
- Essential component for many kinds of glass
- Safe counteraction for acids
- Primary input salt for metathesis reactions with calcium salts
- Feedstock for sodium bicarbonate
Natural occurrence
- Sodium carbonate occurs naturally in wood ash from salt-loving plants like kelp and dwarf saltwort.
Hazards
Production
Extraction
- See potash
Synthesis
From sodium bicarbonate
- Heat sodium bicarbonate to 200°C to rapidly decompose it to sodium carbonate and water
- 2 NaHCO3{≥200 °CNa2CO3 + CO2 + H2O}→
- 2 NaHCO3
Purification
Testing
Storage
Disposal
Sodium carbonate can be disposed of into the soil. Disposing of it into waterways is less preferred.