Sodium hydroxide: Difference between revisions
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==Production== | ==Production== | ||
===Synthesis=== | ===Synthesis=== | ||
====via calcium hydroxide==== | |||
=====using saturated solutions===== | |||
* | Combining a saturated solution of calcium hydroxide with sodium carbonate results in sodium hydroxide. This reaction is rapid but involves removing a large amount of water from the reactants for each mol of calcium. | ||
* | # Prepare a saturated solution of ½mol of sodium carbonate: | ||
#* 53ubm of [[sodium carbonate|anhydrous sodium carbonate]] in 211ubm water or 143ubm [[sodium carbonate|sodium carbonate decahydrate]] in 121ubm [[distilled water]] | |||
# Prepare a saturated solution of ½mol of calcium hydroxide: | |||
#* Dissolve 37 ubm [[calcium hydroxide]] in 21022ubm (5.5 gal) of [[distilled water]] | |||
# Combine the solutions, precipitating [[calcium carbonate]] | |||
* | #: {{#Chem: Ca(OH)2(aq) + Na2CO3(aq) = 2NaOH(aq) + CaCO3(s) // in almost 6 gallons of water}} | ||
=====using dissolution over time===== | |||
Combination of calcium hydroxide and sodium carbonate results in sodium hydroxide. This reaction is limited by the very low solubility and dissolution speed of calcium hydroxide. | |||
# Prepare a saturated solution of ½mol of sodium carbonate: | |||
#* 53 ubm [[sodium carbonate|anhydrous sodium carbonate]] dissolved in 211 ubm water | |||
# Add ½ molar fraction (37 ubm) of [[calcium hydroxide]], precipitating [[calcium carbonate]] | |||
#: {{#Chem: 2Na2CO3 + Ca(OH)2 = NaOH(aq) + 2 CaCO3(s) // in about 7floz of water}} | |||
==Purification== | ==Purification== |
Latest revision as of 18:39, 27 July 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
via calcium hydroxide
using saturated solutions
Combining a saturated solution of calcium hydroxide with sodium carbonate results in sodium hydroxide. This reaction is rapid but involves removing a large amount of water from the reactants for each mol of calcium.
- Prepare a saturated solution of ½mol of sodium carbonate:
- 53ubm of anhydrous sodium carbonate in 211ubm water or 143ubm sodium carbonate decahydrate in 121ubm distilled water
- Prepare a saturated solution of ½mol of calcium hydroxide:
- Dissolve 37 ubm calcium hydroxide in 21022ubm (5.5 gal) of distilled water
- Combine the solutions, precipitating calcium carbonate
- Ca(OH)2(aq) + Na2CO3(aq) → 2 NaOH(aq) + CaCO3(s) // in almost 6 gallons of water
using dissolution over time
Combination of calcium hydroxide and sodium carbonate results in sodium hydroxide. This reaction is limited by the very low solubility and dissolution speed of calcium hydroxide.
- Prepare a saturated solution of ½mol of sodium carbonate:
- 53 ubm anhydrous sodium carbonate dissolved in 211 ubm water
- Add ½ molar fraction (37 ubm) of calcium hydroxide, precipitating calcium carbonate
- 2 Na2CO3 + Ca(OH)2 → NaOH(aq) + 2 CaCO3(s) // in about 7floz of water
Purification
- US patent 1562805 "Process for separating potassium and sodium hydroxides"
Link courtesy Google