Zinc hydroxide

Zinc hydroxide
	Zinc hydroxide
Names
	IUPAC name Zinc hydroxide
Identifiers
CAS Number	20427-58-1 ;
3D model (JSmol)	Interactive image;
ChemSpider	7988510 ;
ECHA InfoCard	100.039.816
PubChem CID	9812759;
UNII	OXK3V8KJ7L ;
CompTox Dashboard (EPA)	DTXSID7042516 ;
	InChI InChI=1S/2H2O.Zn/h21H2;/q;;+2/p-2 Key: UGZADUVQMDAIAO-UHFFFAOYSA-L ; InChI=1/2H2O.Zn/h21H2;/q;;+2/p-2 Key: UGZADUVQMDAIAO-NUQVWONBAV;
	SMILES [Zn+2].[OH-].[OH-];
Properties
Chemical formula	Zn(OH)2
Molar mass	99.424 g/mol
Appearance	white powder
Density	3.053 g/cm3, solid
Melting point	125 °C (257 °F; 398 K) (decomposition)
Solubility in water	slightly soluble
Solubility product (Ksp)	1.8×10−14
Solubility in alcohol	insoluble
Acidity (pKa)	3.12, 3.39
Magnetic susceptibility (χ)	−67.0·10−6 cm3/mol
Thermochemistry
Std enthalpy of; formation (ΔfH⦵298)	−642 kJ·mol−1
Hazards
Flash point	Non-flammable
Related compounds
Other anions	Zinc oxide
Other cations	Cadmium hydroxide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Zinc hydroxide is an inorganic chemical compound with the formula Zn(OH)₂. It occurs naturally as 3 rare minerals: wülfingite (orthorhombic), ashoverite, and sweetite (both tetragonal).

Like the hydroxides of other metals (such as lead, aluminium, beryllium, tin and chromium), zinc hydroxide (as well as zinc oxide) is amphoteric. It thus dissolves readily in a dilute solution of a strong acid, such as HCl, as well as in a solution of an alkali such as sodium hydroxide.

Preparation

Zinc hydroxide can be prepared by first dissolving zinc oxide in concentrated aqueous solution of sodium hydroxide. The resulting solution is strongly diluted.

Zn²⁺ + 2 OH⁻ → Zn(OH)₂.

The initial colorless solution contains the zincate ion:

Zn(OH)₂ + 2 OH⁻ → Zn(OH)₄²⁻.

Zinc hydroxide will dissolve because the ion is normally surrounded by water ligands; when excess sodium hydroxide is added to the solution, the hydroxide ions will reduce the complex to a −2 charge and make it soluble. When excess ammonia is added, it sets up an equilibrium which provides hydroxide ions; the formation of hydroxide ions causes a similar reaction as sodium hydroxide and creates a +2 charged complex with a coordination number of 4 with the ammonia ligands, making the complex soluble so that it dissolves.

Unlike the hydroxides of aluminium and lead, zinc hydroxide also dissolves in excess aqueous ammonia to form a colorless, water-soluble ammine complex.

Applications

One major use is as an absorbent in surgical dressings. It is also used to find zinc salts by mixing sodium hydroxide with the suspect salt.

References

↑ Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 265. ISBN 0-08-029214-3. LCCN 82-16524.
↑ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
↑ F. Wagenknecht; R. Juza (1963). "Zinc Sulfide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1074. NY, NY: Academic Press.

Chemistry in Context - By Graham Hill, John Holman (pp. 283,284)

[P82db-1] Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 265. ISBN 0-08-029214-3. LCCN 82-16524.

[b1-2] Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.

[3] F. Wagenknecht; R. Juza (1963). "Zinc Sulfide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1074. NY, NY: Academic Press.