<unk>  shares the typical properties of other carbonates. Notably it * reacts with acids, releasing carbon dioxide (technically speaking, carbonic acid, but that disintegrates quickly to CO2 and H2O): ::CaCO3() + 2 H+() → Ca2+() + CO2() + H2O() * releases carbon dioxide upon heating, called a thermal decomposition reaction, or calcination (to above 840 °C in the case of<unk> , to form calcium oxide, commonly called quicklime, with reaction enthalpy 178 kJ/mol: ::CaCO3() → CaO() + CO2()<unk>  reacts with water that is saturated with carbon dioxide to form the soluble calcium bicarbonate.<unk> () + CO2() + H2O() → Ca(HCO3)2() This reaction is important in the erosion of carbonate rock, forming caverns, and leads to hard water in many regions. An unusual form of<unk>  is the hexahydrate ikaite,<unk> ·6H2O. Ikaite is stable only below 8 °C.
Calcium carbonate
Strontium ranelate
Potassium fluoride
Sodium fluoride
Lanthanum carbonate
Aluminum chloride hexahydrate
Calcium fructoborate
Magnesium citrate