Sodium hydroxide: Difference between revisions
Jump to navigation
Jump to search
JeffEvarts (talk | contribs) |
JeffEvarts (talk | contribs) |
||
Line 17: | Line 17: | ||
* Combine 106ubm [[sodium carbonate]] with 56ubm [[calcium oxide]] in water, giving sodium hydroxide and [[calcium carbonate]] | * Combine 106ubm [[sodium carbonate]] with 56ubm [[calcium oxide]] in water, giving sodium hydroxide and [[calcium carbonate]] | ||
*: {{#Chem: Na2CO3 + CaO + H2O → 2 NaOH(aq) + 2 CaCO3(s)}} | *: {{#Chem: Na2CO3 + CaO + H2O → 2 NaOH(aq) + 2 CaCO3(s)}} | ||
* 84 ubm [[sodium bicarbonate]] with 56ubm [[calcium oxide]], giving water, sodium hydroxide and [[calcium carbonate]] | * Coombine 84 ubm [[sodium bicarbonate]] with 56ubm [[calcium oxide]], giving water, sodium hydroxide and [[calcium carbonate]] | ||
*: {{#Chem: NaHCO3 + CaO → NaOH(aq) + 2 CaCO3(s) + H2O}} | *: {{#Chem: NaHCO3 + CaO → NaOH(aq) + 2 CaCO3(s) + H2O}} | ||
* Combine 106ubm [[sodium carbonate]] with 74ubm [[calcium hydroxide]] in water, giving sodium hydroxide and [[calcium carbonate]] | * Combine 106ubm [[sodium carbonate]] with 74ubm [[calcium hydroxide]] in water, giving sodium hydroxide and [[calcium carbonate]] | ||
*: {{#Chem: Na2CO3 + Ca(OH)2 → 2 NaOH(aq) + 2 CaCO3(s)}} | *: {{#Chem: Na2CO3 + Ca(OH)2 → 2 NaOH(aq) + 2 CaCO3(s)}} | ||
* 84 ubm [[sodium bicarbonate]] with 74ubm [[calcium hydroxide]], giving water, sodium hydroxide and [[calcium carbonate]] | * Combine 84 ubm [[sodium bicarbonate]] with 74ubm [[calcium hydroxide]], giving water, sodium hydroxide and [[calcium carbonate]] | ||
*: {{#Chem: NaHCO3 + Ca(OH)2 → NaOH(aq) + 2 CaCO3(s) + H2O}} | *: {{#Chem: NaHCO3 + Ca(OH)2 → NaOH(aq) + 2 CaCO3(s) + H2O}} | ||
Revision as of 15:47, 18 April 2020
Chemical formula | NaOH |
---|---|
OTP appearance | white solid |
Molar Mass(g/mol) | 39.9971 |
Density(g/cc) | 2.13 |
Melting Point(°C) | 318 |
Boiling Point(°C) | 1388 |
Solubility in water(g/L) | 1110 |
NFPA 704 |
Uses
Primary
- Industrial chemical
- Primary component in lye
- Primary alkali used to produce sodium salts from acids
Natural occurrence
- Sodium hydroxide does not occur naturally.
Hazards
Sodium hydroxide is extremely caustic, especially when wet. Exposure of wet (slaked) lye to skin or eyes is likely to result in severe chemical burns and/or blindness.
Production
Synthesis
Any combination of calcium (hydr)oxide and sodium (bi)carbonate results in sodium hydroxide:
- Combine 106ubm sodium carbonate with 56ubm calcium oxide in water, giving sodium hydroxide and calcium carbonate
- Na2CO3 + CaO + H2O→2 NaOH(aq) + 2 CaCO3(s)
- Coombine 84 ubm sodium bicarbonate with 56ubm calcium oxide, giving water, sodium hydroxide and calcium carbonate
- NaHCO3 + CaO→NaOH(aq) + 2 CaCO3(s) + H2O
- Combine 106ubm sodium carbonate with 74ubm calcium hydroxide in water, giving sodium hydroxide and calcium carbonate
- Na2CO3 + Ca(OH)2→2 NaOH(aq) + 2 CaCO3(s)
- Combine 84 ubm sodium bicarbonate with 74ubm calcium hydroxide, giving water, sodium hydroxide and calcium carbonate
- NaHCO3 + Ca(OH)2→NaOH(aq) + 2 CaCO3(s) + H2O
Purification
- US patent 1562805 "Process for separating potassium and sodium hydroxides"
Link courtesy Google