Strontium hydroxide

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Strontium hydroxide
18480-07-4 YesY
1311-10-0 (octahydrate) N
ChEBI CHEBI:35105 YesY
ChemSpider 79094 YesY
EC Number 242-367-1
Jmol 3D model Interactive image
PubChem 87672
Molar mass 121.63 g/mol (anhydrous)
139.65 g/mol (monohydrate)
265.76 g/mol (octahydrate)
Appearance prismatic colourless crystals
Density 3.625 g/cm3 (anhydrous)
1.90 g/cm3 (octahydrate)
Melting point 535 °C (995 °F; 808 K) (anhydrous, 375K for octahydrate)
Boiling point 710 °C (1,310 °F; 983 K) decomposes (anhydrous)
0.41 g/100 mL (0 °C)
1.77 g/100 mL (40 °C)
21.83 g/100 mL (100 °C) [1]
Solubility insoluble in acetone
soluble in acid, NH4Cl
Basicity (pKb) −2.19
tetragonal (octahydrate)
Flash point Non-flammable
Related compounds
Other anions
Strontium oxide
Strontium peroxide
Other cations
Beryllium hydroxide
Magnesium hydroxide
Calcium hydroxide
Barium hydroxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Strontium hydroxide, Sr(OH)2, is a caustic alkali composed of one strontium ion and two hydroxide ions. It is synthesized by combining a strontium salt with a strong base. Sr(OH)2 exists in anhydrous, monohydrate, or octahydrate form.


Because Sr(OH)2 is very slightly soluble in water, its preparation can be easily carried out by the addition of a strong base such as NaOH or KOH, drop by drop to a solution of any strontium salt, most commonly Sr(NO3)2 (strontium nitrate). The Sr(OH)2 will precipitate out as a fine white powder. From here, the solution is filtered, and the Sr(OH)2 is washed with cold water and dried.[2]


Strontium hydroxide is used chiefly in the refining of beet sugar and as a stabilizer in plastic. It may be used as a source of strontium ions when the chlorine from strontium chloride is undesirable. Strontium hydroxide absorbs carbon dioxide from the air to form strontium carbonate.


Strontium hydroxide is a severe skin, eye and respiratory irritant. It is harmful if swallowed.


  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ Brauer, Georg (1963). Handbook Of Preparative Inorganic Chemistry. Academic Press. p. 935. 

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