Limescale is a hard chalky deposit, consisting mainly of calcium carbonate (CaCO3), that often builds up inside kettles, hot water boilers, and pipework, especially that for hot water. It is also often found as a similar deposit on the inner surfaces of old pipes and other surfaces where "hard water" has evaporated.
The color varies from off-white through a range of greys and pink or reddish browns, depending on the other minerals present. Iron compounds give the reddish-browns.
In addition to being unsightly and hard to clean, limescale can seriously damage or impair the operation of various plumbing and heating components. Descaling agents are commonly used to remove limescale. Prevention of fouling by scale build-up relies on the technologies of water softening.
The type found deposited on the heating elements of water heaters consists mainly of calcium carbonate (CaCO3). Hard water contains calcium (and often magnesium) bicarbonate or similar ions. Magnesium salts originate from dolomitic limestone present in the rocks through which rainwater percolates before collection. Calcium salts, such as calcium carbonate and calcium bicarbonate (Ca(HCO3)2), are more soluble in hot water than cold water; thus, heating water does not cause calcium carbonate to precipitate per se. However, there is an equilibrium between dissolved calcium bicarbonate and dissolved calcium carbonate as represented by the chemical equation
Ca2+ + 2HCO3− ⇋ Ca2+ + CO32− + CO2 + H2O
where the equilibrium is driven by the carbonate/bicarbonate, not the calcium. Note that the CO2 is dissolved in the water. Carbon dioxide dissolved in water (dis) also tends to equilibrate with carbon dioxide in the gaseous state (g):
CO2(dis) ⇋ CO2(g)
The equilibrium of CO2 also moves to the right toward gaseous CO2 when the water temperature rises. When water that contains dissolved calcium carbonate is warmed, CO2 leaves the water as gas, causing the equilibrium of bicarbonate and carbonate to shift to the right, increasing the concentration of dissolved carbonate. As the concentration of carbonate increases, calcium carbonate precipitates as the salt: Ca2+ + CO32− ⇋ CaCO3.
As new cold water with dissolved calcium carbonate/bicarbonate is added and heated, the process continues: CO2 gas is again removed, carbonate concentration increases, and more calcium carbonate precipitates.
As a stone
The Roman Eifel aqueduct was completed around 80 AD and broken and largely destroyed by Germanic tribes in 260. By the Middle Ages the limestone-like limescale accretions from the inside of the aqueduct were particularly desirable as a building material, called "Eifel marble" in an area with little natural stone. In the course of operation of the aqueduct, many sections had a layer as thick as 200 millimetres (7.9 in). The material had a consistency similar to brown marble and was easily removable from the aqueduct. Upon polishing, it showed veins, and it could also be used like a stone board when cut flat. This artificial stone found use throughout the Rhineland and was very popular for columns, window frames, and even altars. Use of "Eifel marble" can be seen as far east as Paderborn and Hildesheim, where it was used in the cathedrals. Roskilde Cathedral in Denmark is the northernmost location of its use, where several gravestones are made of it.
Trade to the west took it to England as a high-status export material in the 11th and 12th centuries, where it was made into columns for a number of Norman English Cathedrals. The impressive polished brown stone was known for many years as 'Onyx Marble'. Its origin and nature was a mystery to people studying the stonework at Canterbury Cathedral, until its source was identified in 2011. It is used there as columns supporting the cloister roof, alternating with columns of Purbeck Marble. These large cathedral cloisters needed several hundred such columns around an open quadrangle, which must have been supplied by a well-organized extraction and transport operation. The Eifel deposits, now called Calcareous sinter or calc-sinter (since it is neither onyx nor marble), have also been identified at Rochester and in the now lost Romanesque cloister at Norwich as well as the Infirmary Cloisters, Chapter House windows, and Treasury doorway at Canterbury.
Soap scum forms when calcium cations from hard water combine with soap, which would dissolve in soft water. This precipitates out in a thin film on the interior surfaces of baths, sinks, and drainage pipes.
- Hermann Weingärtner, "Water" in Ullmann's Encyclopedia of Industrial Chemistry, December 2006, Wiley–VCH, Weinheim. doi:10.1002/14356007.a28_001
- Tegethoff, F. Wolfgang; Rohleder, Johannes; Kroker, Evelyn. Calcium Carbonate: From the Cretaceous Period Into the 21st Century. Birkhäuser, 2001. ISBN 3-7643-6425-4
- C. Wilson (2015). "Canterbury Cathedral's Mystery "Marble": A Double Imposture Unmasked'". In P. Fergusson (ed.). Canterbury Cathedral Priory in the Age of Becket. New Haven and London. pp. 156–60.
- John McNeill (2015). "The Romanesque Cloister in England". Journal of the British Archaeological Association. 168: 34–76. doi:10.1179/0068128815Z.00000000038.
- R.B. Harris (2019). "RECONSTRUCTING THE ROMANESQUE CLOISTER OF NORWICH CATHEDRAL". The Antiquaries Journal. Cambridge University Press. 99: 133–159. doi:10.1017/S0003581519000118.
- Geoff Downer (2019). "calc-sinter or Onyx Marble". canterbury-archaeology.org.uk. Canterbury Historical & Archaeological Society (CHAS).