Calcium acetate

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   Calcium acetate   
Names: calcium acetate
calcium diacetate
calcium ethanoate
lime acetate
acetate of lime
lime pyrolignite
brown acetate
grey acetate

Formula: Ca(CH3COO)2 (anhydrous)
Ca(CH3COO)2 · H2O (monohydrate)
SMILES: CC(=O)[O-].CC(=O)[O-].[Ca+2]
Molar mass: 158.166 g/mol (anhydrous)
176.181 g/mol (monohydrate)
Density: 2.34 g/cm3 (anhydrous)
1.54 g/cm3 (monohydrate)
Crystal system: triclinic (monohydrate)
a=6.75 Å, b=11.076 Å, c=11.782 Åα=116.49°, β=92.4°, γ=97.31°
Shapes:
https://media.crystalls.info/w/uploads/media/Irregular_pinacoidal_prism.json
https://media.crystalls.info/w/uploads/media/Needle.json

Color: colorless
Melting point: 160 °C433.15 K <br />320 °F <br />779.67 °R <br /> (monohydrate)
Refractive index: 1.55 (monohydrate)
Magnetic properties: diamagnetic
Stability: stable (monohydrate)
Hardness: very fragile
Toxicity: non-toxic
LD50=4280mg/kg

Description

Organic compound, salt of alkaline earth metal calcium and organic acetic acid. From water solutions crystallizes as monohydrate.

Precursors

Reaction between calcium carbonate or hydroxide and acetic acid

Chemical equation:

2CH3COOH + CaCO3 = Ca(CH3COO)2 + H2O + CO2
2CH3COOH + Ca(OH)2 = Ca(CH3COO)2 + 2H2O


For preparation of 100.00g of calcium acetate monohydrate а 56.81g of carbonate or 42.05g of hydroxide and 97.39g of 70% acetic acid is required.

Add acid to the flask, then add small parts of calcium compound with stirring until it will totally dissolve or, if you use carbonate, until carbon dioxide emission will stop. After reaction will stop, filter the solution and use it for crystal growing.

Reaction between calcium chloride or nitrate and excess of concentrated acetic acid

Chemical equation:

2CH3COOH + CaCl2 = Ca(CH3COO)2↓ + 2HCl
2CH3COOH + Ca(NO3)2 = Ca(CH3COO)2↓ + 2HNO3


For preparation of 100.00g of calcium acetate monohydrate а 124.35g of calcium chloride hexahydrate or 134.04g of calcium nitrate tetrahydrate and 68.17g of glacial acetic acid is required.

Add to the flask with hot iron compounds solution a acid solution with heating and stirring. Cooling this mixture will cause forming a large amount of crystalline precipitate. Filter precipitate and wash it wish small amount of glacial acetic acid, then filter the solution and use it for crystal growing.

Reaction between calcium nitrate and sodium acetate

Chemical equation:

Ca(NO3)2 + 2NaCH3COO = Ca(CH3COO)2↓ + 2NaNO3


For preparation of 100.00g of calcium acetate monohydrate а 134.04g of calcium nitrate tetrahydrate and 154.48g of sodium acetate trihydrate is required.

Add to the flask with hot calcium nitrate solution a sodium acetate solution with heating and stirring. Cooling this mixture will cause forming a large amount of crystalline precipitate. Filter precipitate and wash it wish small amount of cold water, then filter the solution and use it for crystal growing.

Storage conditions

Store in its original form or under several layers of varnish at average humidity and room temperature. Do not store in matchboxes or cotton wool and do not heat.

Solubility

Temperatureгр/100,00 гр waterгр/100,00 гр methanolгр/100,00 гр acetic acid
(anhydrous)(monohydrate)(anhydrous)(anhydrous)
0°C273.15 K <br />32 °F <br />491.67 °R <br />37.448.6
10°C283.15 K <br />50 °F <br />509.67 °R <br />36~45.1
15°C288.15 K <br />59 °F <br />518.67 °R <br />~35.4~43.30.75
20°C293.15 K <br />68 °F <br />527.67 °R <br />34.7~41.60.156
25°C298.15 K <br />77 °F <br />536.67 °R <br />~34.339.8
30°C303.15 K <br />86 °F <br />545.67 °R <br />33.8~39.4
40°C313.15 K <br />104 °F <br />563.67 °R <br />33.2~38.7
50°C323.15 K <br />122 °F <br />581.67 °R <br />~33.0~38.0
60°C333.15 K <br />140 °F <br />599.67 °R <br />32.7~37.3
70°C343.15 K <br />158 °F <br />617.67 °R <br />~33.1~36.61.01
80°C353.15 K <br />176 °F <br />635.67 °R <br />33.5~35.9
90°C363.15 K <br />194 °F <br />653.67 °R <br />31.1~35.2
100°C373.15 K <br />212 °F <br />671.67 °R <br />29.734.52.426
Soluble in hydrazine. Insoluble in ethanol, acetone and benzene.


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