Jump to content

Calcium lactate

From Wikipedia, the free encyclopedia
(Redirected from E327)
Calcium lactate

Calcium L-lactate
Names
Preferred IUPAC name
Calcium bis(2-hydroxypropanoate)
Other names
  • calcium lactate 5-hydrate
  • calcium lactate
  • 2-hydroxypropanoic acid
  • calcium salt pentahydrate
Identifiers
3D model (JSmol)
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.011.278 Edit this at Wikidata
EC Number
  • 212-406-7
E number E327 (antioxidants, ...)
UNII
  • InChI=1S/2C3H6O3.Ca/c2*1-2(4)3(5)6;/h2*2,4H,1H3,(H,5,6);/q;;+2/p-2 checkY
    Key: MKJXYGKVIBWPFZ-UHFFFAOYSA-L checkY
  • InChI=1/2C3H6O3.Ca/c2*1-2(4)3(5)6;/h2*2,4H,1H3,(H,5,6);/q;;+2/p-2
    Key: MKJXYGKVIBWPFZ-NUQVWONBAM
  • [Ca+2].[O-]C(=O)C(O)C.[O-]C(=O)C(O)C
Properties
C6H10CaO6
Molar mass 218.22 g/mol
Appearance white or off-white powder, slightly efflorescent
Density 1.494 g/cm3
Melting point 240 °C (464 °F; 513 K) (anhydrous)
120 °C (pentahydrate)
L-lactate, anhydrous, g/100 mL: 4.8 (10 °C), 5.8 (20 °C), 6.7 (25 °C), 8.5 (30 °C);[1][2] 7.9 g/100 mL (30 °C)[citation needed]
Solubility very soluble in methanol, insoluble in ethanol
Acidity (pKa) 6.0-8.5
1.470
Pharmacology
A12AA05 (WHO)
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H319
P264, P280, P305+P351+P338, P337+P313
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Flash point Not applicable
No data
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Calcium lactate is a white crystalline salt with formula C
6H
10CaO
6, consisting of two lactate anions H
3C(CHOH)CO−
2 for each calcium cation Ca2+
. It forms several hydrates, the most common being the pentahydrate C
6H
10CaO
6·5H
2O.

Calcium lactate is used in medicine, mainly to treat calcium deficiencies; and as a food additive with E number of E327. Some cheese crystals consist of calcium lactate.[3][4]

Properties

[edit]

The lactate ion is chiral, with two enantiomers, D (−,R) and L (+,S). The L isomer is the one normally synthesized and metabolized by living organisms, but some bacteria can produce the D form or convert the L to D. Thus calcium lactate also has D and L isomers, where all anions are of the same type.[5]

Some synthesis processes yield a mixture of the two in equal parts, resulting in the DL (racemic) salt. Both the L and the DL forms occur as crystals on the surface of aging Cheddar cheese.[5]

The solubility of calcium L-lactate in water increases significantly in presence of d-gluconate ions, from 6.7 g/dl) at 25 °C to 9.74 g/dl or more.[1][2] Paradoxically, while the solubility of calcium L-lactate increases with temperature from 10 °C (4.8 g/dl) to 30 °C (8.5 g/dl), the concentration of free Ca2+
 ions decreases by almost one half. This is explained as the lactate and calcium ions becoming less hydrated and forming a complex C
3H
5O
3Ca+
.[2]

The DL (racemic) form of the salt is much less soluble in water than the pure L or D isomers, so that a solution that contains as little as 25% of the D form will deposit racemic DL-lactate crystals instead of L-lactate.[6]

The pentahydrate loses water in a dry atmosphere between 35 and 135 °C, being reduced to the anhydrous form and losing its crystalline character. The process is reversed at 25 °C and 75% relative humidity.[7]

In aqueous solutions, calcium lactate partially dissociates into calcium ions (Ca2+) and lactate ions (C3H5O3-). The lactate ion, being the conjugate base of lactic acid (a weak acid), can undergo slight hydrolysis, making the solution mildly alkaline. This reaction increases the concentration of hydroxide ions (OH-), resulting in a solution with a pH slightly above 7, that is, basic.[8][9][10] Here are approximate pH values for calcium lactate solutions at various concentrations:[9]

Approximate pH Values of Aqueous Calcium Lactate Solutions at Different Concentrations
Concentration of Calcium Lactate (mol/L) Approximate pH
0.01 7.4 – 7.6
0.05 7.6 – 7.8
0.10 7.8 – 8.0
0.20 8.0 – 8.2

Calcium lactate pentahydrate has solubility in water of or 79 g/L at 25°C. That property makes calcium lactate readily available for absorption when consumed. It is more soluble than some other calcium salts, such as citrate (which has solubility of 0.85 g/L at 25°C).[11][8]

Preparation

[edit]

Calcium lactate can be prepared by the reaction of lactic acid with calcium carbonate or calcium hydroxide.

Since the 19th century, the salt has been obtained industrially by fermentation of carbohydrates in the presence of calcium mineral sources such as calcium carbonate or calcium hydroxide.[12]: p200 [13][14] Fermentation may produce either D or L lactate, or a racemic mixture of both, depending on the type of organism used.[15]

Uses

[edit]

Medicine

[edit]

Calcium lactate has several uses in human and veterinary medicine.

Calcium lactate is used in medicine as an antacid.[16]

It is also used to treat hypocalcaemia (calcium deficiencies). It can be absorbed at various pHs, thus it does not need to be taken with food. However, in this use it has been found to be less convenient than calcium citrate. Calcium lactate contains 13% elemental calcium.[17]

In the early 20th century, oral administration of calcium lactate dissolved in water (but not in milk or tablets) was found to be effective in prevention of tetany in humans and dogs with parathyroid insufficiency or who underwent parathyroidectomy.[18][19]

The compound is also found in some mouth washes and toothpaste as an anti-tartar agent.[16]

Calcium lactate (or other calcium salts) is an antidote for soluble fluoride ingestion[20]: p165  and hydrofluoric acid.

While aqueous solutions of calcium lactate exhibit a slightly basic (above 7) pH due to the slight hydrolysis of lactate ions, calcium lactate is not used as an antacid. The reasons lie in its chemical properties and physiological behavior in the gastrointestinal tract. Calcium lactate has insufficient acid-neutralizing capacity caused by its weak base formation. The lactate ion (C3H5O3-) is the conjugate base of lactic acid, which is a weak acid. When calcium lactate dissolves in water, it releases lactate ions that can slightly increase the pH of the aqueous solution. The degree of hydroxide ion (OH-) generation through lactate ion hydrolysis is minimal, making the solution only mildly basic. Calcium lactate is more soluble in water compared to other calcium salts such as calcium citrate or carbonate, leading to quicker absorption in the small intestine rather than reacting in the stomach. The slight increase in pH from calcium lactate is rapidly buffered by the stomach's acidic environment, as such, it does not provide the rapid pH shift needed to relieve symptoms of hyperacidity.[21][22][23] As such, the role of calcium lactate is to supply calcium ions to the body—a source of bioavailable calcium. Calcium lactate is a well-absorbed and generally safe form of calcium supplementation[24] that does not interfere with digestion.[17] Its properties allow it to be used effectively without disrupting normal gastrointestinal function, making it suitable for individuals seeking to increase their calcium intake without affecting their digestive processes.[17] Calcium lactate does not interact significantly with digestive enzymes or other components of the gastrointestinal tract. It dissolves and releases calcium ions that are absorbed in the small intestine without affecting the digestion of proteins, carbohydrates, or fats.[17]

Food industry

[edit]

The compound is a food additive classified by the United States FDA as generally recognized as safe (GRAS), for uses as a firming agent, a flavor enhancer or flavoring agent, a leavening agent, a nutritional supplement, and a stabilizer and thickener.[25]

Calcium lactate is also known as cheese lactate because it coagulates milk, making the chhena used in the production of paneer cheese.[16] Chhena is also used to make various sweets and other milk proteins.

Calcium lactate is an ingredient in some baking powders containing sodium acid pyrophosphate. It provides calcium in order to delay leavening.[26]: p933 

Calcium lactate is added to sugar-free foods to prevent tooth decay. When added to chewing gum containing xylitol, it increases the remineralization of tooth enamel.[27]

The compound is also added to fresh-cut fruits, such as cantaloupes, to keep them firm and extend their shelf life, without the bitter taste caused by calcium chloride, which can also be used for this purpose.[28]

Calcium lactate is used in molecular gastronomy as a flavorless fat-soluble agent for plain and reverse spherification. It reacts with sodium alginate to form a skin around the food item.

Animal feeds

[edit]

Calcium lactate may be added to animal rations as a source of calcium.[29]

Chemistry

[edit]

The compound was formerly an intermediate in the preparation of lactic acid for food and medical uses. The impure acid from various sources was converted to calcium lactate, purified by crystallization, and then converted back to acid by treatment with sulfuric acid, which precipitated the calcium as calcium sulfate. This method yielded a purer product than would be obtained by distillation of the original acid.[12]: p180  Recently ammonium lactate has been used as an alternative to calcium in this process.[14]

Water treatment

[edit]

Calcium lactate has been considered as a coagulant for removing suspended solids from water, as a renewable, non-toxic, and biodegradable alternative to aluminum chloride AlCl
3.[30]

Bioconcrete

[edit]

Addition of calcium lactate substantially increases the compressive strength and reduces water permeability of bioconcrete, by enabling bacteria such as Enterococcus faecalis, Bacillus cohnii, Bacillus pseudofirmus and Sporosarcina pasteurii to produce more calcite.[31][32]

See also

[edit]

References

[edit]
  1. ^ a b Martina Vavrusova, Merete Bøgelund Munk, and Leif H. Skibsted (2013): "Aqueous Solubility of Calcium l-Lactate, Calcium d-Gluconate, and Calcium d-Lactobionate: Importance of Complex Formation for Solubility Increase by Hydroxycarboxylate Mixtures". Journal of Agriculture and Food Chemistry, volume 61 issue 34, pages 8207–8214. doi:10.1021/jf402124n
  2. ^ a b c Martina Vavrusova, Ran Liang, and Leif H. Skibsted (2014): "Thermodynamics of Dissolution of Calcium Hydroxycarboxylates in Water". Journal of Agriculture and Food Chemistry, volume 62, issue 24, pages 5675–5681. doi:10.1021/jf501453c
  3. ^ Stephie Clark & Shantanu Agarwal (April 27, 2007). "Chapter 24: Cheddar and Related Hard Cheeses. 24.6: Crystal Formation". In Y. H. Hui (ed.). Handbook of Food Products Manufacturing (1st ed.). Wiley-Interscience. p. 589. ISBN 978-0470049648.
  4. ^ Phadungath, Chanokphat (2011). The Efficacy of Sodium Gluconate as a Calcium Lactate Crystal Inhibitor in Cheddar Cheese (Thesis). University of Minnesota. Archived from the original on May 5, 2021. Retrieved October 12, 2013.
  5. ^ a b G.F. Tansman, P.S. Kindstedt, J.M. Hughes (2014): "Powder X-ray diffraction can differentiate between enantiomeric variants of calcium lactate pentahydrate crystal in cheese". Journal of Dairy Science, volume 97, issue 12, pages 7354–7362. doi:10.3168/jds.2014-8277
  6. ^ Gil Fils Tansman (2014): Exploring the nature of crystals in cheese through X-ray diffraction Masters Dissertation, University of Vermont
  7. ^ Yukoh Sakata, Sumihiro Shiraishi, Makoto Otsuka (2005): "Characterization of dehydration and hydration behavior of calcium lactate pentahydrate and its anhydrate". Colloids and Surfaces B: Biointerfaces, volume 46, issue 3, pages 135–141. doi:10.1016/j.colsurfb.2005.10.004
  8. ^ a b Williams, Michael (April 2013). The Merck Index: An Encyclopedia of Chemicals, Drugs, and Biologicals, 15th Edition Edited by M.J.O'Neil, Royal Society of Chemistry, Cambridge, UK. Drug Development Research. Vol. 74. p. 2708. doi:10.1002/ddr.21085. ISBN 9781849736701.
  9. ^ a b Sheskey, Paul J.; Hancock, Bruno C.; Moss, Gary P.; Goldfarb, David J. (1 October 2020). Handbook of Pharmaceutical Excipients. Pharmaceutical Press. ISBN 978-0857113757.
  10. ^ Remington: The Science and Practice of Pharmacy. Pharmaceutical Press. 3 September 2012. p. 3056. ISBN 978-0857110626.
  11. ^ Rumble, John R. (4 June 2024). CRC Handbook of Chemistry and Physics. CRC Press. ISBN 978-1032655628.
  12. ^ a b H. Benninga (1990): "A History of Lactic Acid Making: A Chapter in the History of Biotechnology". Volume 11 of Chemists and Chemistry. Springer, ISBN 9780792306252
  13. ^ Kook Hwa Choi, Yong Keun Chang, and Jin-Hyun Kim (2011) "Optimization of Precipitation Process for the Recovery of Lactic Acid". KSBB Journal, volume 26, pages 13-18. (Abstract Archived 2017-04-16 at the Wayback Machine)
  14. ^ a b "A gypsum-free, energy-saving route to lactic acid" Chemical Engineering, July 1, 2009.
  15. ^ Rojan P. John, K. Madhavan Nampoothiri, Ashok Pandey (2007): "Fermentative production of lactic acid from biomass: an overview on process developments and future perspectives" Applied Microbiology and Biotechnology, volume 74, issue 3, pages 524–534 doi:10.1007/s00253-006-0779-6
  16. ^ a b c "Calcium Lactate Uses". www.tripurabiotech.com. Archived from the original on 2021-05-13. Retrieved 2020-08-04.
  17. ^ a b c d Straub DA (June 2007). "Calcium supplementation in clinical practice: a review of forms, doses, and indications". Nutr Clin Pract. 22 (3): 286–96. doi:10.1177/0115426507022003286. PMID 17507729.
  18. ^ Sloan J. Wilson (1938): "Postoperative Parathyroid Insufficiency and Calcium Lactate". Archives of Surgery, volume 37, issue 3, pages 490-497. doi:10.1001/archsurg.1938.01200030139008
  19. ^ A.B. Luckhardt and B. Goldberg (1923): "Preservation of the Life of Completely Parathyroidectomized Dogs by Means of the Oral Administration of Calcium Lactate." Journal of the American Medical Association, volume 80, issue 2, pages 79-80. doi:10.1001/jama.1923.02640290009002
  20. ^ Carolyn A. Tylenda (2011): "Toxicological Profile for Fluorides, Hydrogen Fluoride, and Fluorine (Update)". DIANE Publishing. ISBN 9781437930771
  21. ^ Emkey, Ronald D.; Emkey, Gregory R. (2012). "Calcium Metabolism and Correcting Calcium Deficiencies". Endocrinology and Metabolism Clinics of North America. 41 (3): 527–556. doi:10.1016/j.ecl.2012.04.019. PMID 22877428.
  22. ^ Brunton, Laurence L.; Knollmann, Björn C. (7 November 2022). Goodman Gilman's Pharmacological Basis T: Herapeutics 14e (Ie). McGraw-Hill Education. p. 1664. ISBN 978-1265016982.
  23. ^ "Office of Dietary Supplements - Calcium". Archived from the original on 2018-03-17. Retrieved 2024-11-17.
  24. ^ Program, Human Foods (10 October 2024). "Food Additive Status List". FDA. Archived from the original on 12 November 2020. Retrieved 17 November 2024.
  25. ^ U. S. Food and Drug Administration (2016): Code of Federal Regulations: Title 21 Volume 3, section 21CFR184.1207 "Calcium lactate" Archived 2017-04-15 at the Wayback Machine, revised April 1, 2016
  26. ^ E.J. Pyler (1988), Baking Science and Technology, Sosland Publishing
  27. ^ Sudaa, R.; T. Suzukia; R. Takiguchib; K. Egawab; T. Sanob; K. Hasegawa (2006). "The Effect of Adding Calcium Lactate to Xylitol Chewing Gum on remineralization of Enamel Lesions". Caries Research. 40 (1): 43–46. doi:10.1159/000088905. PMID 16352880. S2CID 45316316.
  28. ^ Luna-Guzman, Irene; Diane M. Barrett (2000). "Comparison of calcium chloride and calcium lactate effectiveness in maintaining shelf stability and quality of fresh-cut cantaloupes". Postharvest Biology and Technology. 19: 16–72. doi:10.1016/S0925-5214(00)00079-X.
  29. ^ B.N. Paul, S. Sarkar, S. S. Giri, S. N Mohanty, P. K. Mukhopadhyay (2006): "Dietary calcium and phosphorus requirements of rohu Labeo rohita fry". Animal Nutrition and Feed Technology, volume 6, issue 2, pages 257-263
  30. ^ R. Devesa-Rey, G. Bustos, J. M. Cruz, A. B. Moldes (2012): "Evaluation of Non-Conventional Coagulants to Remove Turbidity from Water". Water, Air, & Soil Pollution, volume 223, issue 2, pages 591–598. doi:10.1007/s11270-011-0884-8
  31. ^ Irwan, J.M.; Anneza, L.H.; Othman, Norzila; Faisal Alshalif, A. (2016). "Compressive Strength and Water Penetration of Concrete with Enterococcus faecalis and Calcium Lactate". Key Engineering Materials. 705: 345–349. doi:10.4028/www.scientific.net/KEM.705.345.
  32. ^ Moneo, Shannon (11 September 2015). "Dutch scientist invents self-healing concrete with bacteria". Journal Of Commerce. Archived from the original on 22 March 2018. Retrieved 21 March 2018.
Retrieved from "https://wiki.riteme.site/w/index.php?title=Calcium_lactate&oldid=1259153948"