62-54-4 Usage
Chemical properties
Calcium acetate, also known as acetate of lime or vinegar salts, is the calcium salt of acetic acid. It is an odorless powder. Calcium has an important role in the nutrition of humans and animals. Hormonal mechanisms control absorption of dietary calcium (including added calcium salts) allowing adaptation to a range of calcium intakes while maintaining a relatively constant blood calcium concentration of about 10 mg/100 mL. Major functions of calcium inside the body include the formation and maintenance of bones and teeth, the physiology of muscle contraction, the cell membrane integrity, the activity of several enzymes that have specific requirement for it, the coagulation of blood, and the regulation of acid-base balance.*
Uses
Different sources of media describe the Uses of 62-54-4 differently. You can refer to the following data:
1. Calcium acetate [Ca(CH3COO)2.H2O] is used as a food additive and a mordant to fix dyes in the textile industry. It is used as an alkali (base) in the manufacture of soaps, to improve some lubricants, and as an antimold to preserve baked goods for a longer shelf life.
2. Calcium Acetate is the calcium salt of acetic acid which functions
as a sequestrant and mold control agent. it contains approximately
25% calcium. it is a white odorless powder which is readily soluble
in water with a solubility of approximately 37 g in 100 g water at
0°c. its solubility decreases with increasing temperature, with a sol-
ubility of approximately 29 g in 100 g of water at 100°c.
3. Calcium Acetate is the salt of acetic acid which is used as a preservative and sequestrant.
4. Calcium Acetate is a salt of acetic acid (A167640), a common chemical reagent used in a multitude of organic reactions. It is the primary constituent of vinegar, contributing to its distinct taste and odor. It is used in the synthesis of dye-sensitized solar cells.
Toxicity
ADI is not subject to restrictive regulations (FAO/WHO, 2001).
GRAS (FDA, §181.29, §182.6197, § 184.1185, 2000).
LD50: 52 mg/kg (mouse, subcutaneous).
Usage limit
GB 14880 a 94: cereals and their products, beverages 8~16g/kg.
GB 2760-2001: vinegar, 6~8g/kg (in terms of Ca).
FAO/WHO (1984): Edible caseinate, GMP.
FDA, § 184.1185 (2000): baked goods, gelatin, pudding, fillings, 0.2%; sweet sauce, top materials and poured, 0.15%;
EEC can be used for packaging cheese powder, quick-setting jelly powder.
FEMA (mg/kg): soft drinks 200; baked goods 500.
Production method
It is obtained by the reaction between calcium carbonate and acetic acid. Preparation method of anhydrous calcium acetate: the refined powder of calcium carbonate is added to the water, stirred into a suspension; added separately of a small amount of glacial acetic acid. After completion of the reaction, the filtrate was concentrated in a water bath and a white solid, anhydrous calcium acetate, was precipitated from the viscous filtrate.
It is obtained by the neutralization between coke acid (wood acetic acid) and calcium hydroxide, followed by the evaporation of the filtrate and recrystallization.
It is obtained by the reaction between the reaction between acetic acid and calcium hydroxide or calcium carbonate. Filter, concentrate and cool to obtain the dihydrate (colorless crystal), heated to 84 °C in a water salt (colorless crystal), heated to 100 °C to obtain the anhydrous salt.
Shellfish can be taken as raw materials, washed, crushed and dried for 1 h, subjecting to barbecue for 2 hour at 900~l000 ℃, then being added water to make a 1.3~1.5mol/L lime milk. And then neutralized with acetic acid to clarify, filter with the filtrate concentrated, and finally dried at 120~140 °C to get the final product with a yield of 91.28%.
To a 20% acetic acid solution, add calcium carbonate powder to until there is no longer any CO2 gas escaping, then add a small amount of calcium carbonate, heated? 80 ° C for reaction of 2-3h. The filtrate was heated and concentrated with water bath while adding a small amount of 80% acetic acid at the same time to precipitate the calcium acetate monohydrate (what precipitated after the cooling of the solution is dihydrate), and finally dried at 60~70 ℃to derive the products.
Hazards & Safety Information
Category:? Toxic substances
Toxicity classification:? highly toxic
Acute toxicity:? intravenous-mouse LD50: 52 mg/kg; celiac-mouse LD50: 75 mg/kg
Flammability and Hazardous characteristics:? Thermal decomposition releases Pungent irritation Smoke
Storage and transportation characteristics:Treasury: ventilated, low temperature drying; store it separately from food raw materials
Fire extinguishing agent:? water, dry powder, foam, carbon dioxide
Chemical Properties
Calcium acetate occurs as a white or almost white, odorless or
almost odorless, hygroscopic powder.
Production Methods
Calcium acetate can be prepared by soaking calcium carbonate (found in eggshells, or in common carbonate rocks such as lime stone or marble) in vinegar: CaCO3 + 2CH3COOH → Ca(CH3COO)2 + H2O + CO2 Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then.
Preparation
Produced by calcium hydroxide neutralization of acetic acid.
Definition
ChEBI: The calcium salt of acetic acid. It is used, commonly as a hydrate, to treat hyperphosphataemia (excess phosphate in the blood) in patients with kidney disease: the calcium ion combines with dietary phosphate to form (insoluble) calcium phosphate, which is
excreted in the faeces.
General Description
Calcium Acetate belongs to the group of calcium salts, widely used as phosphorus binders in patients with chronic renal failure.Pharmaceutical secondary standards for application in quality control, provide pharma laboratories and manufacturers with a convenient and cost-effective alternative to the preparation of in-house working standards.
Pharmaceutical Applications
Calcium acetate is used as a preservative in oral and topical
formulations.
Therapeutically, parenteral calcium acetate acts as a source of
calcium ions for hypocalcemia or electrolyte balance. Oral
calcium acetate is used as a complexing agent for hyperphosphatemia
in dialysis patients. Calcium acetate is also used in the
food industry as a stabilizer, buffer and sequestrant.
Clinical Use
Phosphate binding agent
Safety Profile
Poison by intravenous
and intraperitoneal routes. Mutation data
reported. See also CALCIUM
COMPOUNDS. When heated to
decomposition it emits acrid smoke and
fumes.
Safety
Calcium acetate is used in oral and topical formulations. The pure
form of calcium acetate is toxic by IP and IV routes.
LD50 (mouse, IP): 0.075 g/kg
LD50 (mouse, IV): 0.052 g/kg
LD50 (rat, oral): 4.28 g/kg
Veterinary Drugs and Treatments
Calcium acetate can be used for oral administration to treat hyperphosphatemia
in patients with chronic renal failure. Secondary to its
phosphorus binding efficiency and lower concentration of elemental
calcium, calcium acetate is considered the most effective and having
the lowest potential for causing hypercalcemia of the calcium-based
phosphorus-binding agents. When compared to calcium carbonate,
calcium acetate binds approximately twice as much phosphorus per gram of elemental calcium administered. Unlike calcium citrate, calcium
acetate does not promote aluminum absorption.
Metabolism
The residual acetate will be metabolised through
bicarbonate, which will be further excreted via normal
metabolic routes.
Any unbound calcium not involved in the binding
of phosphate will be variable and may be absorbed.
Calcium is absorbed mainly from the small intestine by
active transport and passive diffusion. About one-third
of ingested calcium is absorbed although this can vary
depending upon dietary factors and the state of the small
intestine. 1,25-Dihydroxycholecalciferol (calcitriol), a
metabolite of vitamin D, enhances the active phase of
absorption.
Excess calcium is mainly excreted renally. Unabsorbed
calcium is eliminated in the faeces, together with that
secreted in the bile and pancreatic juice. Minor amounts
are lost in the sweat, skin, hair, and nails.
storage
Calcium acetate is stable although very hygroscopic, and so the
monohydrate is the common form. It decomposes on heating (above
1608℃) to form calcium carbonate and acetone.
Store in well-closed airtight containers.
Incompatibilities
Calcium acetate is incompatible with strong oxidizing agents and
moisture.
Regulatory Status
GRAS listed. Accepted for use as a food additive in Europe.
Included in the FDA Inactive Ingredients Database (oral suspensions
and tablets; topical emulsions, lotions, and creams). Included
in nonparenteral medicines (oral tablets) licensed in the UK.
Check Digit Verification of cas no
The CAS Registry Mumber 62-54-4 includes 5 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 2 digits, 6 and 2 respectively; the second part has 2 digits, 5 and 4 respectively.
Calculate Digit Verification of CAS Registry Number 62-54:
(4*6)+(3*2)+(2*5)+(1*4)=44
44 % 10 = 4
So 62-54-4 is a valid CAS Registry Number.
InChI:InChI=1/C2H4O2.Ca/c1-2(3)4;/h1H3,(H,3,4);/q;+2/p-1
62-54-4Relevant articles and documents
Synthesis of CaCu3Ti4O12, Study of Physicochemical and Photocatalytic Properties
Ivanov,Alekseeva,Agafonov
, (2020)
Abstract: Precursor CaCu3Ti4O12 has been obtained using solution method in acetic acid medium, it was annealed at 100, 200, 400, 600 800, and 1100°C. Sintered powders have been studied by physicochemical methods of analysi
Synthesis, characterization and the thermal decomposition of calcium(II)bis(oxalato)calcium(II)dihydrate
Deb,Baruah,Dass
, p. 301 - 308 (1996)
Calcium(II)bis(oxalato)calcium(II)dihydrate, Ca[Ca(C2O4)2]·2H2O, has been synthesized and characterized by elemental analysis, and reflectance and IR spectral studies. Thermal decomposition studies (TG, DTG, and DTA) in air showed that the final end product was CaO at 865°C through the intermediate formation of a mixture of CaCO3 and CaO at approx. 818°C. At around 424°C a mixture of CaO and Ca(C2O4)1.2 is formed by partial decomposition of oxalate which is stable up to 670°C. DSC studies up to 700°C in nitrogen at 10°C min-1 showed both endothermic and exothermic peaks with activation energies of 190 and 458 kJ mol-1, respectively, and compared with values calculated from TG. Some of the decomposition products were identified by spectral, analytical and X-ray powder diffraction studies and a tentative mechanism for the decomposition is proposed.
Dissolution of calcium carbonate in aqueous solutions of acetic acid
Blinkova,Eliseev
, p. 1064 - 1066 (2005)
A kinetic equation for the calcium carbonate dissolution, fitting the experimental data to within 8.1%, was obtained. The additional diffusion hindrance caused by the CO2 evolution in the course of the dissolution was considered.
DIRECT CONVERSION OF ESTERS TO CARBOXYLATES
-
Paragraph 0041, (2022/03/22)
A calcium carboxylate is prepared by reacting water, calcium oxide, and a compound of formula (I): wherein R is a C1-C3 alkyl and R1 is a C1 or C2 alkyl. The reaction solution is heated to remove an amount of a co-product from the reaction solution. The calcium carboxylate may be recovered in a solid form from the reaction solution.
On the nature of calcium magnesium acetate road deicer
Miller, Jennifer R.,LaLama, Matthew J.,Kusnic, Rachel L.,Wilson, Darian E.,Kiraly, Paije M.,Dickson, Samuel W.,Zeller, Matthias
, p. 1 - 10 (2018/11/20)
CMA (calcium magnesium acetate) road deicers have gained popularity in recent years as an environmentally friendly alternative to traditional rock salt, and as an industrial adsorbent for removing H2S and other odorous acid gases from gas streams. Despite its increasing commercial use, its exact composition and crystalline structure remained unknown, with subsequent problems in evaluating properties of commercial CMA. Various synthetic routes towards formation of crystalline calcium magnesium acetates were investigated. From aqueous solutions preferential formation of calcium monohydrates or calcium monohydrate acetic acid solvates is observed. Crystals of genuine mixed metal calcium-magnesium acetate were obtained from hot glacial acetic acid. Material suitable for analysis by single crystal X-ray diffraction, SC-XRD, was obtained by slight reduction of solvent volume at 80 °C for several hours. CMA crystallizes in the orthorhombic space group Pnma with a formula of Mg2Ca(OAc)6 (OAc = acetate anion), with a magnesium to calcium ratio of two to one. Under the same conditions, but in the absence of magnesium, the acetic acid solvate of calcium acetate, Ca(OAc)2(HOAc), is obtained, which is also described. Multicrystalline XRD and EDS analysis data of ground CMA samples match those of commercial CMA. Single crystal structural analysis finds an unusually large unoccupied void space of 9.4% of the unit cell volume. Thermal gravimetric analysis, TGA, gives an upper limit of one water molecule per formula unit of CMA, leaving the void space at least partially unoccupied. This helps to better understand CMAs unusually low density, which had been an issue when used as a commercial road deicer, having been described as being easily blown off road surfaces when applied in crystalline or powder form.
RECOVERY OF ORGANIC ACID USING A COMPLEX EXTRACTION SOLVENT
-
Page/Page column 34-35, (2012/05/05)
A method is disclosed for the recovery of an organic acid from a dilute salt solution in which the cation of the salt forms an insoluble carbonate salt. An amine, C02 and a water immiscible solvent are introduced to the solution to form the insoluble carbonate salt and a complex between the acid and the amine that is soluble in both an aqueous and a solvent phase. The complex is extracted into the solvent phase which is than distilled to recover the acid or an ester of the acid in a concentrated form.
CALCIUM ABSORPTION ENHANCER
-
, (2010/06/16)
The present invention provides a calcium absorption enhancer that places no burden on the body of a human or a domestic animal to which a calcium compound is administered and can increase the efficiency with which a calcium content is absorbed into the body by supplying calcium ions in the stomach or the like of the human or the domestic animal in a sustained-release manner after administration of the calcium compound. The calcium absorption enhancer of the present invention contains, as an active ingredient, water-soluble calcium particles that can release calcium ions in an aqueous solution in a sustained-release manner.
Preservative and Additive for Food and Feed
-
, (2009/05/28)
A preservative and additive for food and feed. One aspect of the invention concerns various acidified clays and minerals as food or feed additive to kill, or inhibit the growth of, harmful microorganisms and to inactivate mycotoxins, such as aflatoxins, present as contaminants in human foods and animal feeds. Another aspect of the present invention relates to a clay of hydrated sodium calcium aluminosilicate with relatively uniform particle size distribution.
Precursors for mixed metal oxide nanoparticles: Synthesis and characterization of μ-oxoalkoxides of some bivalent metals and their β-diketonates
Sharma, Malti,Bhagi, Ajay K.,Sharma, Harish K.,Priti, Ritu Kansal,Kumar, Ram,Kapoor, Pramesh N.
, p. 256 - 260 (2007/10/03)
New heterobimetallic derivatives of the type M{OAl(OPri) 2}2 (M = Sn, Pb, Cd) have been prepared by the reactions of M(OAc)2 with Al(OPri)3 in 1:2 molar ratio in hydrocarbon solvent (xylene/toluene) with the continuous liberation of isopropyl acetate. Furthermore, reactions of M{OAl(OPri) 2}2 (M = Ca, Pb, Cd) with β-diketones (acetylacetone, benzoyl acetone) have also been carried out to obtain modified derivatives. These new derivatives have been characterized by elemental analyses and spectroscopic [IR, NMR (1H, 13C, 27Al and 119Sn)] studies.
Highly acidic metalated organic acid
-
Page/Page column 10, (2008/06/13)
A highly acidic metalated organic acid composition and its preparation. The acidic composition can be prepared by mixing a monovalent or polyvalent cation and an organic acid in the presence of a strong oxyacid, wherein the resultant acidic composition is less corrosive to a ferrous metal than a solution of a mineral acid having the same acidic pH value as that of the acidic composition, and where in the acid composition is more biocidal than a mixture of the organic acid and a metal salt of the organic acid which mixture has the same acid normality value as that of the acidic composition. The acidic composition can be prepared by mixing at least one regenerating acid, at least one metal base, and at least one organic acid, wherein the amount of the regenerating acid is in excess of the equivalent amount of the metal base.
