19855-56-2

Usage

Uses

Used in Food Industry:
Calcium fumarate is used as a food additive for the purpose of calcium fortification in various food products, enhancing their nutritional value and contributing to the maintenance of bone health.
Used in Pharmaceutical Industry:
In pharmaceuticals, calcium fumarate serves as a calcium supplement, incorporated into formulations to address calcium deficiencies and support overall health.
Used in Animal Feed Production:
Calcium fumarate is utilized as a calcium supplement in animal feed, ensuring that livestock receive adequate calcium for optimal health and growth.
Used in Industrial Applications:
In the industrial sector, calcium fumarate is employed in the production of certain plastics and polymers, where it contributes to the enhancement of material properties and performance.

InChI:InChI=1/C4H4O4.Ca/c5-3(6)1-2-4(7)8;/h1-2H,(H,5,6)(H,7,8);/q;+2/b2-1+;

Upstream product

• 108-31-6 maleic anhydride 
• 110-16-7 maleic acid 
• 87-69-4 tartaric acid 
• 110-17-8 (2E)-but-2-enedioic acid 
• 115609-54-6 C₈H₆O₅^(2-)*Ca⁽²⁺⁾ 

Downstream Products

• 110-17-8 (2E)-but-2-enedioic acid 

Relevant academic research and scientific papers

Application of calcium carbonate nanoparticles and microwave irradiation in submerged fermentation production and recovery of fumaric acid: A novel approach

The aim of the present study was to explore the possible application of calcium carbonate nanoparticles (CCNPs) and microwave irradiation (MWI) in fumaric acid (FA) production and recovery, respectively. The fungal strain Rhizopus oryzae 1526 was employed as the biocatalyst for FA production. A glucose-basic salt medium was used as the fermentation medium. Scanning electron microscopy (SEM) analysis of CCNPs displayed the spherical shapes, while zetasizer measurements showed the CCNPs to be around 190 ± 20 nm in size. FTIR analysis of CCNPs confirmed the chemical composition. BET analysis confirmed higher specific surface areas of CCNPs (11.95 ± 0.03 m2 g-1) compared to calcium carbonate microparticles (CCMPs) (3.51 ± 0.02 m2 g-1). FA neutralization timing for CCNPs was much lower than CCMPs (190 and 350 seconds, respectively). CCNPs enhanced the volumetric productivity of FA from 0.47 g L-1 h-1 to 0.74 g L-1 h-1. At 20, 40 and 60 g L-1 concentrations and at 25 °C, viscosities of the CCNPs were found to be lower than respective CCMPs. Moreover, the CCNPs did not exhibit any toxicity towards the fungus. FA production obtained with CC micro and CCNPs were 67.34 ± 2 g L-1 and 66.92 ± 2.7 g L-1, respectively. Under MWI heating, 10 ± 1 min was found to be sufficient for recovery of FA and this was much lower than conventional heating timing of 28 ± 1 min.

Process for the production of crystalline aspartic acid

The invention provides a process for the preparation of aspartic acid via a fermentation process for the preparation of ammonia fumarate, wherein the pH of the fermentation broth is controlled by the addition of a calcium base to produce a calcium fumarate precipitate, characterized in that ammonium fumarate is produced by separating the precipitated calcium fumarate from the fermentation broth, and reacting the same with a reagent selected from ammonia, ammonium carbonate, ammonia in combination with CO2 and mixtures therefore, to form ammonium fumarate and a co-product selected from calcium carbonate and calcium hydroxide, wherein the energy of indirect neutralization of fumaric acid by ammonia serves as the driving force for the conversion of calcium fumarate to the desired ammonium fumarate product and for the regeneration of a calcium base reagent, and wherein diammonium fumarate is enzymatically converted to ammonium aspartate and acidulated to from aspartic acid.

Chemical process

There is disclosed herein improved processes for the preparation of ether carboxylates by reacting in an alkaline reaction medium the salts of maleic acid and a carboxylic or polycarboxylic acid having a reactive hydroxyl group on a non-carbonyl carbon atom in the presence of a calcium ion catalyst wherein unreacted acid salts are recovered from the reaction medium by lowering the pH of the reaction medium to a range of from about 4 to about 6. The precipitated salts are recycled to the synthesis reaction to prepare additional amounts of product.