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Calcium hydroxide is modestly soluble in water, as seen for many dihydroxides. Its solubility increases from 0.66 g/L at 100 °C to 1.89 g/L at 0 °C. [8] Its solubility product K sp of 5.02 × 10 −6 at 25 °C, [1] its dissociation in water is large enough that its solutions are basic according to the following dissolution reaction:
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Calcium chlorate – Ca(ClO 3) 2; Calcium chloride – CaCl 2; Calcium chromate – CaCrO 4; Calcium cyanamide – CaCN 2; Calcium fluoride – CaF 2; Calcium hydride – CaH 2; Calcium hydroxide – Ca(OH) 2; Calcium monosilicide – CaSi; Calcium oxalate – CaC 2 O 4; Calcium hydroxychloride – CaOCl 2; Calcium perchlorate – Ca(ClO 4) 2 ...
Calcium bisulfite can be prepared by treating lime (chemical formula Ca(OH) 2) with an excess of sulfur dioxide and water. [2] Upon synthesis of calcium bisulfite solution, it will have a green to yellow opaque appearance as an aqueous solution. [3]
The structure is related to that of zirconium orthosilicate (zircon): Ca 2+ is 8-coordinate, SO 2− 4 is tetrahedral, O is 3-coordinate. CaSO 4 ·2H 2 O (gypsum and selenite (mineral)): dihydrate. [7] CaSO 4 · 1 / 2 H 2 O : hemihydrate, also known as plaster of Paris. Specific hemihydrates are sometimes distinguished: α-hemihydrate ...
SO 2 + CaCO 3 → CaSO 3 + CO 2. Scrubbing with hydrated lime follows the following idealized reaction: [4] [5] SO 2 + Ca(OH) 2 → CaSO 3 + H 2 O. The resulting calcium sulfite oxidizes in air to give gypsum: 2 CaSO 3 + O 2 → 2 CaSO 4. The gypsum, if sufficiently pure, is marketable as a building material.
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Na 2 S + CaCO 3 → CaS + Na 2 CO 3. Millions of tons of this calcium sulfide byproduct was discarded, causing extensive pollution and controversy. [2] Milk of lime, Ca(OH) 2, reacts with elemental sulfur to give a "lime-sulfur", which has been used as an insecticide. The active ingredient is probably a calcium polysulfide, not CaS. [3]