Sodium hydroxide: Difference between revisions

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===Synthesis===
===Synthesis===
Any combination of calcium (hydr)oxide and sodium (bi)carbonate results in sodium hydroxide:
Any combination of calcium (hydr)oxide and sodium (bi)carbonate results in sodium hydroxide:
# Combine any sodium/calcium pair of these alternatives to produce 1 mol  of [[sodium hydroxide]]
* Combine any sodium/calcium pair of these alternatives to produce 1 mol  of [[sodium hydroxide]]
#* 53 ubm [[sodium carbonate|anhydrous sodium carbonate]] or 143ubm [[sodium carbonate decahydrate]] dissolved in 211 ubm water (½ molar {{#Chem:Na2CO3}})
** 53 ubm [[sodium carbonate|anhydrous sodium carbonate]] or 143ubm [[sodium carbonate decahydrate]] dissolved in 211 ubm water (½ molar {{#Chem:Na2CO3}})
#* 84 ubm [[sodium bicarbonate]] dissolved in 875ubm water (1 mol {{#Chem: NaHCO3}})
** 84 ubm [[sodium bicarbonate]] dissolved in 875ubm water (1 mol {{#Chem: NaHCO3}})
#* 28 ubm [[calcium oxide]]
** 28 ubm [[calcium oxide]]
#* 37 ubm [[calcium hydroxide]]
** 37 ubm [[calcium hydroxide]]
#: {{#Chem: Na2CO3 + CaO + H2O = 2 NaOH(aq) + CaCO3(s) // halve reactants (containing disodium compound) to get one mol of sodium hydroxide}}
*: {{#Chem: Na2CO3 + CaO + H2O = 2 NaOH(aq) + CaCO3(s) // halve reactants (containing disodium compound) to get one mol of sodium hydroxide}}
#: {{#Chem: NaHCO3 + CaO = NaOH(aq) + 2 CaCO3(s) + H2O}}
*: {{#Chem: NaHCO3 + CaO = NaOH(aq) + 2 CaCO3(s) + H2O}}
#: {{#Chem: 2Na2CO3 + Ca(OH)2 = NaOH(aq) + 2 CaCO3(s)}}
*: {{#Chem: 2Na2CO3 + Ca(OH)2 = NaOH(aq) + 2 CaCO3(s)}}
#: {{#Chem: NaHCO3 + Ca(OH)2 = NaOH(aq) + 2 CaCO3(s) + H2O}}
*: {{#Chem: NaHCO3 + Ca(OH)2 = NaOH(aq) + 2 CaCO3(s) + H2O}}


==Purification==
==Purification==

Revision as of 19:57, 20 April 2020

 
Sodium hydroxide
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
NFPA704.png
0
3
1
ALK

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 any sodium/calcium pair of these alternatives to produce 1 mol of sodium hydroxide
    Na2CO3 + CaO + H2O 2 NaOH(aq) + CaCO3(s) // halve reactants (containing disodium compound) to get one mol of sodium hydroxide
    NaHCO3 + CaO NaOH(aq) + 2 CaCO3(s) + H2O
    2 Na2CO3 + Ca(OH)2 NaOH(aq) + 2 CaCO3(s)
    NaHCO3 + Ca(OH)2 NaOH(aq) + 2 CaCO3(s) + H2O

Purification

Testing

Storage

Disposal

See Also

References