Calcium acetate: Difference between revisions
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# Evaporate the solution gently leaving crystals of calcium acetate | # Evaporate the solution gently leaving crystals of calcium acetate | ||
'''N.B.''' This is a slight variation on the vinegar-and-baking-soda kitchen chemistry experiment, which produces sodium acetate. Because calcium carbonate is insoluble in water, it is easier to separate from the resulting acetate. | '''N.B.''' This is a slight variation on the vinegar-and-baking-soda kitchen chemistry experiment, which produces sodium acetate. Because calcium carbonate is insoluble in water, it is easier to separate from the resulting acetate. | ||
==Testing== | |||
==Purification== | |||
==Storage== | |||
==Disposal== | |||
==References== | ==References== | ||
<references/> | <references/> | ||
==See Also== | ==See Also== |
Revision as of 10:58, 20 June 2019
Chemical formula | Ca(CH3COO)2 |
---|---|
OTP appearance | white solid |
Molar Mass(g/mol) | 158.17 |
Density(g/cc) | 1.509 |
Solubility in water(g/L) | 347 |
NFPA 704 |
|
Thermal Decomposition |
Uses
Justification Questioned
Other
- Feedstock for propanone
- Component in "sterno"-type flammable gels (A semisolid saturated solution, gels by absorbing ethanol)
- As an intermediate form in the purification of acetic acid
- Nutritional calcium
Hazards
Calcium acetate is Generally Recognized As Safe by the US FDA
Production
Synthesis
- Prepare a strong solution of cool acetic acid
- Dissolve calcium carbonate in excess.
Check:This should produce bubbles of carbon dioxide.- CaCO3 + 2 CH3COOH → Ca(CH3COO)2 + H2O + CO2
- Filter the solution
- Run water in excess through the filter
- Discard the residue (chiefly calcium carbonate)
- Evaporate the solution gently leaving crystals of calcium acetate
N.B. This is a slight variation on the vinegar-and-baking-soda kitchen chemistry experiment, which produces sodium acetate. Because calcium carbonate is insoluble in water, it is easier to separate from the resulting acetate.