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Calcium lactate
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Calcium lactate
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.
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.
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.
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. 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+
.
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.
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.
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. Here are approximate pH values for calcium lactate solutions at various concentrations:
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Calcium lactate
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.
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.
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.
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. 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+
.
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.
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.
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. Here are approximate pH values for calcium lactate solutions at various concentrations:
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