Calcium carbonate (e.g. from limestone) is relatively insoluble in water, and the solubilitydecreases with rising temperature. This is why CaCO3 precipitates out as ‘scale’ in hot water more readily than cold water. At a temperature of 20oC, calcium carbonate pKs= 8.8; at 35oC, pKs= 9.25. If you had water that was at equilibrium with excess calcium carbonate at 20oC and then raised the temperature to 35oC, what is the mass of CaCO3 that will precipitate out per litre of water? Hint: the difference in solubility will drive the reaction back to solid.  CaCO3(s)↔Ca2++CO2−

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