CALCIUM ACETATE

Calcium Acetate belongs to the group of calcium salts, widely used as phosphorus binders in patients with chronic renal failure.
Calcium acetate 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.
Calcium acetate is a chemical compound which is a calcium salt of acetic acid. 

CAS Number: 62-54-4
Molecular Formula: C4H6CaO4
Molecular Weight: 158.17
EINECS Number: 200-540-9

Synonyms:Calcium acetate, 62-54-4, Calcium diacetate, Acetic acid calcium salt, Lime acetate, PhosLo, Lime pyrolignite, Acetate of lime, Brown acetate, Gray Acetate of Lime, Brown Acetate of Lime, Phoslyra, Teltozan, Sorbo-calcion, Gray acetate, Phoslo Gelcaps, calcium ethanoate, FEMA No. 2228, Eliphos, Calcarea acetica, calcium(II) acetate, Calcium acetate anhydrous, Calcium acetate anhydrous, Acetic acid calcium salt (2:1), CHEBI:3310, INS NO.263, Y882YXF34X, INS-263, DTXSID0020234, E-263, Calphron, Everose, Renacet, Phosex, RefChem:5631, Calcium Acetate 667 mg, DTXCID00234, Calcium Acetate Capsules 667 mg, mineral supplement containing calcium acetate, 200-540-9, acetic acid calcium salt, calcium diacetate, MFCD00012448, Calcium di(acetate), Ca(OAc)2, Sanopan, CCRIS 4921, HSDB 928, EINECS 200-540-9, calciumacetate, Calcium acetate [USP:JAN], UNII-Y882YXF34X, AI3-02903, calcium acetate salt, Phoslo (TN), Calcium acetate (USP), C4H6CaO4, EC 200-540-9, SCHEMBL23872, CALCIUM ACETATE [II], CALCIUM ACETATE [MI], CALCIUM ACETATE [FCC], CALCIUM ACETATE [FHFI], CALCIUM ACETATE [HSDB], CALCAREA ACETICA [HPUS], CALCIUM ACETATE [VANDF], Calcium acetate (water <5%), CALCIUM ACETATE [MART.], CHEMBL1200800, CALCIUM ACETATE [USP-RS], CALCIUM ACETATE [WHO-DD], CALCIUM ACETATE [ORANGE BOOK], AKOS015904560, CALCIUM ACETATE [EP MONOGRAPH], CALCIUM ACETATE [USP MONOGRAPH], DB00258, E263, D00931, CALCIUM ACETATE ANHYDROUS [EP IMPURITY], Q409251., acetatedecalcium;Aceticacid,calciunsalt;teltozan;vinegarsalts;CALCIUM ACETATE EXTRA PURE, FCC, E 263;CALCIUM ACETATE HYDRATE PURE;CALCIUM ACETATE HYDRATE, 99.99%;CALCIUM ACETATE SIGMAULTRA

Calcium acetate, also known as acetate of lime or vinegar salts, is the calcium salt of acetic acid. 
Calcium acetate is an odorless powder. 
Calcium acetate has an important role in the nutrition of humans and animals. 

Calcium acetate 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 acetate 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.
Calcium acetate has the formula Ca(C2H3O2)2. 

Calcium acetate standard name is calcium acetate, while calcium ethanoate is the systematic name, an older name is acetate of lime. 
The anhydrous form is very hygroscopic; therefore the monohydrate (Ca(CH3COO)2•H2O) is the common form.
Calcium acetate is a phosphate binder used in patients with end-stage renal disease (ESRD) to prevent elevated phosphate levels and resulting ectopic calcification and secondary hyperparathyroidism.

Calcium acetate treats high phosphorus levels in people with kidney disease. 
It works by lowering the amount of phosphorus body absorbs from food. 
Calcium acetate belongs to a group of medications called phosphate binders.

Calcium acetate is an inorganic chemical compound with the formula Ca(C₂H₃O₂)₂, consisting of two acetate ions bound to one calcium ion.
It appears as a white crystalline solid that is highly soluble in water and slightly soluble in alcohol.
The compound is known for its mild vinegar-like odor, which comes from the acetic acid component in its structure.

It is commonly produced by the reaction of calcium carbonate or calcium hydroxide with acetic acid.
During this process, carbon dioxide is released, and a neutral salt is formed that can be crystallized or dried for industrial use.
This simple synthesis makes calcium acetate an easily accessible compound used across many chemical and biological fields.

Chemically, calcium acetate behaves as a neutral salt that dissociates completely in aqueous solution.
It releases calcium ions and acetate ions, both of which play important roles in biological and industrial systems.
The presence of acetate ions provides buffering capacity, allowing it to stabilize pH in various environments.

In the pharmaceutical and medical industries, calcium acetate is primarily used as a phosphate binder.
It helps patients with chronic kidney disease by preventing the absorption of excess phosphate from food into the bloodstream.
By binding dietary phosphate in the gastrointestinal tract, it reduces the risk of hyperphosphatemia and related complications.

Calcium acetate also serves as a food additive and acidity regulator under the designation E263.
In the food industry, it acts as a preservative and stabilizer, helping control microbial growth and maintain product texture.
Its calcium content also makes it a minor source of dietary supplementation in fortified foods and beverages.

In laboratory and industrial chemistry, calcium acetate is used as a reagent and stabilizer.
When heated, it decomposes to form calcium carbonate and acetone, which can be used in organic synthesis or as a precursor for other calcium compounds.
Its decomposition reaction also demonstrates its use in small-scale experiments illustrating thermal breakdown and ketone formation.

Calcium acetate is a chemical compound which is calcium salt of acetic acid. 
It has the formula Ca(C2H3O2)2. 
Its standard name is calcium acetate, while calcium ethanoate is the systematic name. 

An older name is acetate of lime. 
The anhydrous form is very hygroscopic; therefore the monohydrate (Ca(CH3COO)2?H2O) is the common form.
Calcium acetate is one of a number of calcium salts used to treat hyperphosphatemia (too much phosphate in the blood) in patients with kidney disease.

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.

The calcium salt of acetic acid. 
Calcium acetate 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.

Melting point: 160 °C (decomposition)
Density: 1.5 g/cm³
Refractive index: 1.5500
FEMA: 2228 | CALCIUM ACETATE
Flash point: 160 °C
Storage temperature: Hygroscopic; room temperature; under inert atmosphere
Solubility: H₂O – 1 M at 20 °C, clear, colorless
Form: Powder
Color: White
Specific gravity: 1.50
pH: 8 (1 mM solution); 8.43 (10 mM solution); 8.77 (100 mM solution); 9.13 (1000 mM solution)
Odor: Mild acetic
Odor type: Acetic
Water solubility: Soluble
Decomposition: 160 °C
Stability: Stable. Non-flammable. Incompatible with strong oxidizing agents.
InChIKey: VSGNNIFQASZAOI-UHFFFAOYSA-L
LogP: -0.29

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.

Calcium acetate can be prepared by soaking calcium carbonate (found in eggshells, or in common carbonate rocks such as limestone or marble) or hydrated lime in vinegar: CaCO3(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + H2O(l) + CO2(g)
Ca(OH)2(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + 2H2O(l)
Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then.

Patients with advanced renal insufficiency (creatinine clearance less than 30 ml/min) exhibit phosphate retention and some degree of hyperphosphatemia. 
The retention of phosphate plays a pivotal role in causing secondary hyperparathyroidism associated with osteodystrophy, and soft-tissue calcification. 
The mechanism by which phosphate retention leads to hyperparathyroidism is not clearly delineated. 

Therapeutic efforts directed toward the control of hyperphosphatemia include reduction in the dietary intake of phosphate, inhibition of absorption of phosphate in the intestine with phosphate binders, and removal of phosphate from the body by more efficient methods of dialysis. 
The rate of removal of phosphate by dietary manipulation or by dialysis is insufficient. 
Dialysis patients absorb 40% to 80% of dietary phosphorus. 

Therefore, the fraction of dietary phosphate absorbed from the diet needs to be reduced by using phosphate binders in most renal failure patients on maintenance dialysis. 
Calcium acetate when taken with meals combines with dietary phosphate to form insoluble calcium phosphate which is excreted in the feces. 
Maintenance of serum phosphorus below 6.0 mg/dl is generally considered as a clinically acceptable outcome of treatment with phosphate binders. 

Calcium acetate is highly soluble at neutral pH, making the calcium readily available for binding to phosphate in the proximal small intestine.
Calcium acetate and other calcium salts are phosphate binders. 
They work by binding with the phosphate in the food you eat, so that it is eliminated from the body without being absorbed.

Calcium acetate is utilized in wastewater treatment to adjust acidity and provide a carbon source for microbial growth.
It supports biological denitrification processes by acting as a readily biodegradable organic substrate.
This role is essential in maintaining the efficiency of biological filtration systems and reducing environmental nitrogen pollution.

Calcium acetate is also applied in textile, polymer, and cosmetic industries as a buffering agent and stabilizer.
It improves product consistency by maintaining chemical balance during manufacturing.
Its mild alkalinity and low reactivity make it safe for controlled industrial and consumer applications.

Despite its wide range of uses, calcium acetate must be handled with care in concentrated form.
Ingestion of large amounts can cause gastrointestinal discomfort, and excessive calcium intake may disturb electrolyte balance.
Therefore, pharmaceutical and food uses of calcium acetate are carefully regulated to ensure safe dosage levels.

Calcium acetate is a versatile inorganic salt valued for its buffering, stabilizing, and phosphate-binding properties.
It serves key roles in medicine, food technology, and environmental management due to its chemical stability and biological compatibility.
Its combination of safety, solubility, and reactivity makes it a compound of continued importance in both scientific and industrial applications.

Calcium acetate 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.
Calcium acetate 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.

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 acetate 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. 
Calcium acetate 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. 

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.

Calcium acetate is yet unknown among minerals. 
Calclacite—calcium acetate chloride pentahydrate—is listed as a known mineral, but its genesis is anthropogenic (human-generated, as opposed to naturally occurring).

Uses Of Calcium acetate:
Calcium acetate is used as a food additive and a mordant to fix dyes in the textile industry. 
Calcium acetate 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.
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.

In kidney disease, blood levels of phosphate may rise (called hyperphosphatemia) leading to bone problems. 
Calcium acetate binds phosphate in the diet to lower blood phosphate levels.
Calcium acetate is used as a food additive, as a stabilizer, buffer and sequestrant, mainly in candy products under the number E263.

Tofu is traditionally obtained by coagulating soy milk with calcium sulfate. 
Calcium acetate has been found to be a better alternative; being soluble, it requires less skill and a smaller amount.
Because it is inexpensive, calcium acetate was once a common starting material for the synthesis of acetone before the development of the cumene process: Ca(CH3COO)2 → CaCO3(s) + (CH3)2CO

A saturated solution of calcium acetate in alcohol forms a semisolid, flammable gel that is much like "canned heat" products such as Sterno.
Chemistry teachers often prepare "California Snowballs", a mixture of calcium acetate solution and ethanol.
The resulting gel is whitish in color, resembling a snowball and can be lit on fire; it will burn for around 20 minutes.

Calcium Acetate is the calcium salt of acetic acid which functions as a sequestrant and mold control agent. 
Calcium acetate contains approximately 25% calcium. 
Calcium acetate 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. 

Calcium acetates solubility decreases with increasing temperature, with a sol- ubility of approximately 29 g in 100 g of water at 100°c.
Calcium Acetate is the salt of acetic acid which is used as a preservative and sequestrant.

Calcium acetate is widely used in medicine as a phosphate binder to control high blood phosphate levels in patients with chronic kidney disease.
It works by binding dietary phosphate in the digestive tract, preventing its absorption into the bloodstream.
This action helps reduce the risk of complications such as bone disorders and vascular calcification associated with hyperphosphatemia.

In the pharmaceutical industry, calcium acetate is a key ingredient in various oral formulations and capsules.
It is often combined with other compounds to provide calcium supplementation and improve bone mineral density.
Its stability and solubility make it suitable for controlled-release tablet formulations and liquid suspensions.

In the food industry, calcium acetate functions as a preservative, stabilizer, and acidity regulator, known under the additive code E263.
It prevents spoilage and extends shelf life by inhibiting the growth of bacteria and mold in processed foods.
Additionally, it helps maintain pH balance in baked goods, beverages, and confectionery products, ensuring product consistency.

Calcium acetate is also used in the production of acetone through thermal decomposition.
When heated, it breaks down into calcium carbonate and acetone, which can be collected and purified.
This reaction serves both practical and educational purposes, demonstrating chemical decomposition and ketone formation.

In environmental and wastewater treatment systems, calcium acetate acts as a biodegradable carbon source.
It supports denitrifying bacteria in removing nitrate and nitrite compounds from water.
This property makes it valuable for biological treatment processes that aim to reduce nutrient pollution.

In the chemical industry, calcium acetate serves as a buffering agent and stabilizer in polymer and textile processing.
It maintains solution pH and prevents unwanted reactions during synthesis or dyeing operations.
Its compatibility with other salts and mild alkalinity make it ideal for maintaining stable production environments.

In agriculture, calcium acetate is sometimes used as a calcium supplement in animal feed and fertilizers.
It provides a readily available source of calcium that supports bone health and plant growth.
Its solubility allows it to blend easily with other nutrients in liquid or granular formulations.

In laboratory applications, calcium acetate functions as a reagent for producing acetates and studying thermochemical reactions.
It is used in research experiments to illustrate concepts such as salt formation, buffering, and decomposition chemistry.
Because of its low toxicity, it is suitable for educational demonstrations and small-scale organic synthesis.

In the cosmetics and personal care industries, calcium acetate may be included as a stabilizing or buffering component.
It helps balance formulation pH and improve product texture in lotions, creams, and skincare products.
Its mild and non-corrosive nature ensures compatibility with both organic and aqueous formulations.

Calcium acetate is valued for its multifunctional nature across medicine, food, environmental science, and industrial production.
Its phosphate-binding, stabilizing, and buffering abilities make it useful in diverse applications.
This combination of versatility, safety, and ease of handling secures its place as an essential compound in multiple industries.

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.

Calcium salts are used as a source of calcium cation for the treatment or prevention of calcium depletion in patients in whom dietary measures are inadequate. 
Conditions that may be associated with calcium deficiency include hypoparathyroidism, achlorhydria, chronic diarrhea, vitamin D deficiency, steatorrhea, sprue, pregnancy and lactation, menopause, pancreatitis, renal failure, alkalosis, and hyperphosphatemia. 

Administration of certain drugs (e.g., some diuretics, anticonvulsants) may sometimes result in hypocalcemia which may warrant calcium replacement therapy. 
Calcium acetate should be administered in long-term electrolyte replacement regimens and is also recommended for the routine prophylaxis of hypocalcemia during transfusions with citrated blood. 
Administration of calcium salts should not preclude the use of other measures intended to correct the underlying cause of calcium depletion.

Safety Profile Of Calcium acetate:
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.

Poison by intravenous and intraperitoneal routes, mutation data reported.
Calcium acetate is generally regarded as a low-toxicity and safe compound, but it can still present certain hazards under improper use or excessive exposure.
Direct contact with its solid or concentrated solutions may cause mild irritation to the skin or eyes.

Prolonged handling without protection can result in dryness, redness, or discomfort due to its mildly alkaline nature.
Inhalation of dust or fine particles of calcium acetate can irritate the respiratory system.
Symptoms may include coughing, throat dryness, or sneezing if inhaled in significant amounts.

Although not classified as a respiratory toxin, repeated exposure in poorly ventilated areas should be avoided.
Ingestion of small quantities is not usually harmful, but excessive intake can disrupt electrolyte balance in the body.

Overuse, especially in medical treatments, may lead to elevated calcium levels (hypercalcemia), which can cause nausea, fatigue, confusion, or irregular heartbeat.
Therefore, dosage in pharmaceutical and dietary applications must be carefully controlled by medical supervision.