Zinc acetate

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Zinc acetate
Zinc acetate crystals
IUPAC name
Zinc acetate
Other names
Acetic acid, Zinc salt
Acetic acid, Zinc(II) salt
Zinc diacetate
  • 557-34-6 ☑Y
  • 5970-45-6 ☑Y
3D model (JSmol)
  • Interactive image
  • ChEMBL1200928 ☒N
  • 10719 ☑Y
ECHA InfoCard 100.008.338
E number E650 (flavour enhancer)
PubChem CID
  • 11192
RTECS number ZG8750000
  • H2ZEY72PME ☑Y
Zn(CH3COO)2(H2O)2 (dihydrate)
Molar mass 219.50 g/mol (dihydrate)
183.48 g/mol (anhydrous)
Appearance White solid (all forms)
Density 1.735 g/cm3 (dihydrate)
Melting point Decomposes at 237 °C (459 °F; 510 K) (dihydrate loses water at 100 °C)
Boiling point decomposes
43 g/100 mL (20 °C, dihydrate)
Solubility 1.5 g/100 mL (methanol)
−101.0·10−6 cm3/mol (+2 H2O)
octahedral (dihydrate)
A16AX05 (WHO)
Main hazards mildly toxic
R-phrases (outdated) R22 R36 R50/53
S-phrases (outdated) S26 S60 S61
Related compounds
Other anions
Zinc chloride
Other cations
Copper(II) acetate
Related compounds
Basic beryllium acetate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Zinc acetate is a salt with the formula Zn(CH3CO2)2, which commonly occurs as the dihydrate Zn(O2CCH3)2(H2O)2. Both the hydrate and the anhydrous forms are colorless solids that are commonly used in chemical synthesis and as dietary supplements. Zinc acetates are prepared by the action of acetic acid on zinc carbonate or zinc metal. When used as a food additive, it has the E number E650.


Dietary and medicinal applications

Zinc acetate has been used in lozenges for treating the common cold. Pooling the results of three high dose zinc acetate trials indicates an average 42% reduction in the duration of colds (see figure).[1] A 2016 meta-analysis on three studies on zinc acetate-lozenges and the common cold found that colds were 2.7 days shorter by zinc lozenge usage. This estimate is to be compared with the 7 day average duration of colds in the three trials [2]

This forest plot shows the effect of high dose zinc (>75 mg/day) as zinc acetate lozenges on common cold duration in three randomized placebo-controlled trials. Constructed from data in Table 3 of Hemilä 2011: http://www.ncbi.nlm.nih.gov/pmc/articles/PMC3136969.The three horizontal lines indicate the three studies, and the diamond shape at the bottom indicates the pooled effect of zinc: decrease in the duration of colds by 42% (95%CI: 35 to 48%).

Zinc acetate is a particularly useful salt in lozenges since acetate has relatively low affinity for zinc, with the result that essentially all zinc from the lozenges is freely released upon solvation in the saliva.[3][4][unreliable medical source?]

Although zinc acetate lozenges appear to be able to shorten the duration of colds, some zinc lozenges may be more effective than others. Among the factors affecting the usefulness of a zinc lozenge are the total dose of zinc provided as well as the presence of substances like citric acid which may bind up much of the zinc that the lozenge is providing.[5]

Zinc acetate can also be used to treat zinc deficiencies. As an oral daily supplement it is used to inhibit the body's absorption of copper as part of the treatment for Wilson's disease. Zinc acetate is also sold as an astringent in the form of an ointment, a topical lotion, or combined with an antibiotic such as erythromycin for the topical treatment of acne. It is commonly sold as a topical anti-itch ointment.

In chewing gum, zinc acetate is a breath freshener[6][self-published source?][7][self-published source?] and, when combined with hexetidine, a plaque inhibitor.[8]

Industrial applications

Industrial applications include wood preservation, manufacturing other zinc salts, polymers, manufacture of ethyl acetate, as a dye mordant, and analytical reagent. It is used in commercial nuclear power plants as a plating inhibitor on primary water piping.

Basic properties and structures

In anhydrous zinc acetate the zinc is coordinated to four oxygen atoms to give a tetrahedral environment, these tetrahedral polyhedra are then interconnected by acetate ligands to give a range of polymeric structures.[9][10][11] In contrast, most metal diacetates feature metals in octahedral coordination with bidentate acetate groups.

In zinc acetate dihydrate the zinc is octahedral, wherein both acetate groups are bidentate.[12][13]

Basic zinc acetate

Heating Zn(CH3CO2)2 in a vacuum results in a loss of acetic anhydride, leaving a residue of basic zinc acetate, with the formula Zn4O(CH3CO2)6. This cluster compound has the tetrahedral structure shown below. This species closely resembles the corresponding beryllium compound, although it is slightly expanded with Zn-O distances ~1.97 vs ~1.63 Å for Be4O(OAc)6.[14]


See also


  1. ^ Hemilä, Harri (23 June 2011). "Zinc Lozenges May Shorten the Duration of Colds: A Systematic Review". The Open Respiratory Medicine Journal. 5 (1): 51–58. doi:10.2174/1874306401105010051. PMC 3136969. PMID 21769305.
  2. ^ Hemila, H.; Petrus, E.; Fitzgerald, J.; Prasad, A. (2016). "Zinc acetate lozenges for treating the common cold: an individual patient data meta-analysis". British Journal of Clinical Pharmacology. 82: 1393–1398. doi:10.1111/bcp.13057. PMC 5061795. PMID 27378206.
  3. ^ Eby, George A. "Zinc Lozenges: Cold Cure or Candy? Solution Chemistry Determinations". Bioscience Reports. 24 (1): 23–39. doi:10.1023/B:BIRE.0000037754.71063.41.
  4. ^ Eby, George A. (Mar 2010). "Zinc lozenges as cure for the common cold – A review and hypothesis". Medical Hypotheses. 74 (3): 482–492. doi:10.1016/j.mehy.2009.10.017. PMID 19906491.
  5. ^ Eby G (2009) Zinc Lozenges as a Common Cold Treatment
  6. ^ US 7087255 
  7. ^ US 6592849 
  8. ^ Giertsen E, Svatun B, Saxton A (February 1987). "Plaque inhibition by hexetidine and zinc". Scand J Dent Res. 95 (1): 49–54. doi:10.1111/j.1600-0722.1987.tb01392.x. PMID 3470899.
  9. ^ Clegg, W.; Little, I. R.; Straughan, B. P. (15 December 1986). "Monoclinic anhydrous zinc(II) acetate". Acta Crystallographica Section C. 42 (12): 1701–1703. doi:10.1107/S010827018609087X.
  10. ^ He, Hongshan (15 November 2006). "A new monoclinic polymorph of anhydrous zinc acetate". Acta Crystallographica Section E. 62 (12): m3291–m3292. doi:10.1107/S1600536806046678.
  11. ^ Capilla, A. V.; Aranda, R. A. (1979). "Anhydrous Zinc(II) Acetate (CH3-COO)2Zn". Crystal Structure Communications. 8: 795–797.
  12. ^ van Niekerk, J. N.; Schoening, F. R. L.; Talbot, J. H. (10 September 1953). "The crystal structure of zinc acetate dihydrate, Zn(CH3COO)2.2H2O". Acta Crystallographica. 6 (8): 720–723. doi:10.1107/S0365110X53002015.
  13. ^ Ishioka, T.; Murata, A.; Kitagawa, Y.; Nakamura, K. T. (15 August 1997). "Zinc(II) Acetate Dihydrate". Acta Crystallographica Section C. 53 (8): 1029–1031. doi:10.1107/S0108270197004484.
  14. ^ Koyama, H.; Saito, Y. (1954). "The Crystal Structure of Zinc Oxyacetate, Zn4O(CH3COO)6". Bull. Chem. Soc. Japan. 27 (2): 112–114. doi:10.1246/bcsj.27.112.
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