Calcium Hydroxide: Difference between revisions
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JeffEvarts (talk | contribs) (Created page with "{{Compound|chemf=Ca(OH)2 |stp_p=solid|stp_q=white |mm=74.093|density=2.211|sol_aq=1.73|sol_et=non |group=salts |nfpa_h=3 |decomp={{DecompRow|input=Calcium hydroxide|output={{#Chem: CaO, H2O}}|temp=580}} }} ==Uses== ===Primary=== * Feedstock for most hydroxides: sodium, potassium, etc * Production of mortar and plaster ===Secondary=== * Whitewash ==Hazards== Calcium hydroxide is alkaline. It can irritate the skin, eyes and...") |
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Latest revision as of 16:59, 18 October 2023
| Chemical formula | Ca(OH)2 |
|---|---|
| OTP appearance | white solid |
| Molar Mass(g/mol) | 74.093 |
| Density(g/cc) | 2.211 |
| Solubility in water(g/L) | 1.73 |
| Solubility in ethanol(g/L) | non |
| NFPA 704 |  0
3
0
|
| Thermal Decomposition | Calcium hydroxide
580°C CaO,H2O |
Uses
Primary
Secondary
- Whitewash
Hazards
Calcium hydroxide is alkaline. It can irritate the skin, eyes and lungs and should not be ingested in large quantities. Wash with fresh clean water after contact.
Synthesis
From calcium oxide
In ideal conditions (distilled water, pure calcium oxide) this works. Presuming a "part by mass" is 1g, this yields half a mol (37g) of calcium hydroxide.
- Gather a watertight container resistant to alkaline substances
- Gather 9 parts by mass of water
- Gather 28 parts by mass of calcium oxide
- Place the water in the container
- Slowly add the calcium oxide, allowing the water to cool in between additions
- The mixture is calcium hydroxide
Storage
- Calcium hydroxide is a caustic alkali, so glass and ceramic containers are excellent. Aluminum in particular is bad.
- Calcium hydroxide will absorb carbon dioxide from the air and precipitate as calcium carbonate, so keep in a sealed container
See Also
- lye