Gypsum

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Gypsum[1][2]
SA101 1.jpeg
Mineralogical name Gypsum
Chemical name Calcium sulfate dihydrate
Trivial name plaster of paris, Alabaster, Satin Spar, Selenite
Chemical formula Ca[SO4]•2H2O
Other forms Anhydrite (CaSO4)
Hemihydrate (CaSO4•0.5H2O)
Crystal system monoclinic
Crystal structure
Deliquescence humidity 20°C
Solubility (g/l) at 20°C 2.14 g/l
Density (g/cm³) 2.2-2.4 g/cm³
Molar volume 74.69 cm3/mol
Molar weight 172.17g /mol
Transparency transparent to opaque
Cleavage perfect, clearly visible formation of fibre
Crystal habit flat, prismatic, needle- like crystal, granular, massive aggregate
Twinning very common
Phase transition
Chemical behavior hardly soluble in water
Comments
Crystal Optics
Refractive Indices α = 1.519-1.521
β = 1.522-1.523
γ = 1.529-1.530
Birefringence Δ = 0.010
Optical Orientation biaxial positive
Pleochroism colorless
Dispersion 58°
Used Literature
{{{Literature}}}


Authors: Hans-Jürgen Schwarz , Nils Mainusch, Tim Müller
English Translation by Sandra Leithäuser
back to Sulfate


Calciumsulfate and Gipsum[edit]

Abstract[edit]

This article deals with the system CaSO4/H2O, in particular with gypsum. Gypsum is one of the most important salts responsible for the damage on buildings and wallpaintings. Especially objects exposed to exterior conditions are prone to damage from gypsum. The properties, the effect of the damage, the appearance, but also examination methods are included in the following article. Images, micro photos and examples from practical experiences illustrate the subject.

Introduction[edit]

Gypsum is one of the most common salts causing the deterioration of constructions. It is present in very different types and characteristics, nearly on all external constructions, but can also to be found in the internal environment.


Occurrence of Gypsum[edit]

One of the most prevalent minerals, gypsum forms by precipitation from aqueous solution at temperatures under approximately 40°C. At increased temperatures (> 60°C) of a solution the formation of anhydrite takes place directly. Calcium sulfate and calcium sulfate dihydrate are often present in rocks. Hemihydrate does not occur naturally.
Gypsum occurs naturally in salt deposits and salt deserts, where sometimes desert rose crystals form in combination with quartz inclusions. In salt deposits gypsum and anhydrite sometimes form a caprock, i.e. a massive layer of material covering a natural salt deposit. Synthetic gypsum is produced in coal-fired power plants, as a by-product of flue- gas desulferization.

Origin and formation of gypsum on monuments[edit]

The relevance of the damage caused by gypsum, on monuments made from mineral building materials, is substantially linked to the conversion reaction from lime to gypsum. When exposed to air containing SOx and in combination with moisture, important material components of buildings can be converted into gypsum. The reaction takes place as follows:

CaCO3 + H2SO4 → CaSO4 + H2O + CO2

Moreover, gypsum as a major component of mortars, plasters and some building stones (e.g. anhydrite) can be an original building material, an integral part of the monuments fabric.


Damage potential and weathering activity[edit]

Solubility properties[edit]

Figure1: Solubility of CaSO4 in water (diagram: Michael Steiger)


Gypsum belongs to the group of salts with a low solubility in aqueous solution and therefore it can be described as less mobile than others. However, the influence of ions from other sources is comparatively high. For example, the presence of halite can increase the solubility of gypsum in dependence of the concentration ratio, up to the factor of four.

Figure 2:Solubility of gypsum compared with other salts (after [Stark.etal:1996]Title: Bauschädliche Salze
Author: Stark, Jochen; Stürmer, Sylvia
Link to Google Scholar)


Hydration behavior[edit]

The system CaSO4 – H2O:
calcium sulfate can appear in three different hydrate phases:

  • anhydrite- the above mentioned anhydrous form
  • hemihydrate- the least stable form
  • Gypsum- calcium sulfate dihydrate

Anhydrite exists in different modifications, resulting in different chemical properties, in dependence of the modification (e.g. varying solubility in water). The same applies for hemihydrate.
A value for the transition temperature (in aqueous solution) is the range of between 40°C-66°C. Under normal climatic conditions, on monuments, the precipitation of calcium sulfate from aqueous solution will therefore be predominantly gypsum. Anhydrite forms when the temperature in solution is higher than 40°C-60°C. Parallel to this the formation of large amounts of the metastable hemihydrate takes place during precipitation, it is later transformed into more stable hydrate phases.
When heating the dihydrate (as a solid and dry) to approximately 50°C, the chemically combined water is expelled and hemihydrate forms. However, a complete transition to hemihydrate only takes place at temperatures of around 100°C. If dihydrate is heated to 500-600°C, the anhydrous calcium sulfate is formed. At temperatures above 1000°C the thermal decomposition into calcium oxide and SO3 is effected.


Hygroscopicity[edit]

Figure 3: The modification of the solubility of gypsum in water, in the presence of halite, is shown in Figure 3. If the concentration of halite is approximately 140 g/l in aqueous solution, around 8 g gypsum is dissolved (Angaben nach [DAns:1933]Title: Die Lösungsgleichgewichte der Systeme der Salze ozeanischer Salzablagerungen
Author: d'Ans, J.
Link to Google Scholar)

. The pure gypsum salt has no defined Deliquescence point. If, in the presence of halite, relative Humidity levels exceed 90 % RH, gypsum crystals may dissolve, due to the sorption behavior of halite. A decrease of humidity levels to approximately 75% RH causes the recrystallization of gypsum.

Crystallization pressure[edit]

At crystallization in aqueous solution, with the saturation at a ration of 2:1, gypsum produces a linear growth pressure of 28,2-33,4 N/mm2 within a temperature range of 0-50°C. In comparison with other damaging salts, these values lie in the middle range of a calculated scale of values reaching from 7,2 to 65,4 N/mm2 [according to [Winkler:1975]Title: Stone: Properties, Durability in Man´s Environment
Author: Winkler, Erhard M.
Link to Google Scholar].

Hydration pressure[edit]

Gypsum as a constituent of an object, can only release the water of crystallization (chemically combined water) at temperatures of approx. 50°C, i.e. it will normally not dehydrate. In contrast the enclosure of the water of crystallization is possible, if anhydrite or hemihydrate are present in a monument. Both processes are associated with a change in volume (of 31.9 % at the conversion from hemihydrate- gypsum) and the emergence of hydration pressure [Zahlenwerte nach [Sperling.etal:1980]Title: Salt Weathering on Arid Environment, I. Theoretical ConsiderationsII. Laboratory Studies
Author: Sperling, C.H.B.and Cooke, R.U.
Link to Google Scholar]. In the instance of a conversion from hemihydrate- gypsum (keyword Gipstreiben) at temperatures ranging from 0-20°C and an RH or 80%, a hydration pressure of 114 –160 N/mm2 can be effected- an extremely high value [ [Stark.etal:1996]Title: Bauschädliche Salze
Author: Stark, Jochen; Stürmer, Sylvia
Link to Google Scholar].

Conversion reaction[edit]

The hazardous character of gypsum to historic substance, is connected to the conversion reaction calcite- gypsum. The gypsum molecules formed by calcite hold a volume, that exceeds the volume of the original calcite molecule by about 100%. In this context a relevant damage factor is the modification of the water solubility. Calcite has a water solubility of approx. 0,014g/l (20°C) and is therefore more difficult to dissolve than gypsum. When a conversion to gypsum takes place the result is a more water sensitive system. N.B. The research by Snethlage and Wendler [Snethlage.etal:1998]Title: Steinzerfall und Steinkonservierung - neueste Ergebnisse der Münchner Forschungen
Author: Snethlage, Rolf; Wendler, Eberhard
Link to Google Scholar analyses the influence of gypsum on the linear hygroscopic expansion of certain sandstone materials. The damages and the change in swelling behavior of the material was explained through the influence of gypsum.

Analytical identification[edit]

Microscopy[edit]

Laboratory examination: Gypsum is slightly water soluble, therefore gypsum-containing sample material only dissolves slightly, when mixed with distilled Water. In solution, gypsum- containing sample material recrystallizes by carefully concentrating the solvent. At first, single needles form, then increasingly needle- like gypsum aggregate in proximity of the seam of the solvent emerges. Alternatively, sample material can be dissolved in hydrochloric acid, which also leads to the formation of crystal needles. Compared to other salts that can recrystallize in needle-like shapes, e.g. sodium carbonate, gypsum needles are clearly shorter.

Refraction indices:    nx = 1.521; ny =1.523; nz =1.530
birefringence:      Δ = 0.009
crystal class:            monoclinic

Polarized light microscopy examination:
Apart from the typical acicular habit of gypsum crystals, (especially in recrystallized material) different morphological characteristics appear. These can be useful for identifying gypsum. Gypsum particles (in raw material samples) display shapes of rounded fragments and plate- like rhombohedra, clearly showing the inner cleavage planes. Furthermore, the occurrence of twinning shapes is typical for gypsum crystals, whether they are lath- shaped, tabular or lamellar. The assignment of refractive indices is carried out in accordance with the immersion method using media with indices nD=1,518 und nD=1,53. Due to the often small- scale particles the examination using the Schoeder van der Kolk method is more significant and reliable than the Becke- Line test. Gypsum crystals belong to the class of monoclinic crystals. Thus, they show, depending on the orientation of the single particle under the microscope, a parallel or respectively a symmetrical extinction, but mainly exhibit a characteristicly oblique axis position in the extinction position. On well developed crystal rhombi the oblique extinction can clearly be measured. Of all calcium sulfate crystals, gypsum has the lowest birefringence. Under crossed polarizers, gypsum has very low interference colors, lying within the gray to yellowish white range of the first order, (of course depending on the thickness of the particles).


Possibility for mistakes:
The Analysis methods mentioned above clearly identify gypsum, provided the following evaluation criteria are explicitly clarified.

  • low water solubility
  • characteristic needle- like morphology of the recrystallized particles
  • all observable indices have a nD –value from 1,518 and 1,530
  • gypsum crystal show low interference colors
  • gypsum crystals have an oblique extinction


Table 1: Salt phases with a gypsum- like chemical and optical properties
salt phase differentiating features
Syngenite K2Ca(SO4) • 2H2O all observable indices; 1,518
Tachyhydrite CaMg2Cl6 • 12H2O mostly observable index < 1,518 / only parallel and symmetrical extinction
Hydromagnesite Mg5[OH(CO3)2]2 • 4H2O mostly one index > 1,53




Photos of gypsum crystals and deterioration pattern caused by gypsum[edit]

On an object[edit]

  • Salt damage on a brick, St. Jakobi Church, Perleberg

    Salt damage on a brick, St. Jakobi Church, Perleberg


Under the polarising microscope[edit]

  • In thin section of bricks
  • Brick with gypsum caused damage, St. Jakobi Church, Perleberg, Germany

    Brick with gypsum caused damage, St. Jakobi Church, Perleberg, Germany

  • Brick with gypsum caused damage, St. Jakobi Church, Perleberg, Germany

    Brick with gypsum caused damage, St. Jakobi Church, Perleberg, Germany

  • Gypsum crystals between plaster layers

    Gypsum crystals between plaster layers

  • Gypsum crystallized out of a solution in water on a glass slide
  • Calcium sulfate crystallized out of a solution in water on a glass slide

    Calcium sulfate crystallized out of a solution in water on a glass slide

  • Calcium sulfate with sodium chloride of a real sample, Gypsum crystallized out of a solution in water on a glass slide

    Calcium sulfate with sodium chloride of a real sample, Gypsum crystallized out of a solution in water on a glass slide

  • Calcium sulfate with sodium chloride of a real sample, Gypsum crystallized out of a solution in water on a glass slide

    Calcium sulfate with sodium chloride of a real sample, Gypsum crystallized out of a solution in water on a glass slide

  • Calcium sulfate, Gypsum crystallized out of a solution in water on a glass slide

    Calcium sulfate, Gypsum crystallized out of a solution in water on a glass slide


Under the Scanning Electron Microscope (SEM)[edit]

  • In a SEM
  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • EDX spektra of gypsum crystals in a SEM

    EDX spektra of gypsum crystals in a SEM

  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • Gypsum crystals in a SEM

    Gypsum crystals in a SEM

  • EDX spektra of gypsum crystals in a SEM

    EDX spektra of gypsum crystals in a SEM


Literatur[edit]

[DAns:1933] d'Ans, J. (1933): Die Lösungsgleichgewichte der Systeme der Salze ozeanischer Salzablagerungen, Verlagsgesellschaft für Ackerbau, M.B.H. BerlinLink to Google Scholar
[Dana:1951]Dana E.S. (eds.) Dana J.D. (1951): Dana's System of Mineralogy, 7, Wiley & SonsLink to Google Scholar
[Robie.etal:1978]Robie R.A., Hemingway B.S.; Fisher J.A. (1978): Thermodynamic properties of minerals and related substances at 298.15 K and 1 bar pressure and higher temperatures. In: U.S. Geol. Surv. Bull, 1452 ()Link to Google Scholar
[Snethlage.etal:1998]Snethlage, Rolf; Wendler, Eberhard (1998): Steinzerfall und Steinkonservierung - neueste Ergebnisse der Münchner Forschungen. In: Münchner Geologische Hefte, A 23, Festschrift zum 65. Geburtstag von Prof. Dr. Dietrich D. Klemm, (), 177-201Link to Google Scholar
[Sperling.etal:1980]Sperling, C.H.B.and Cooke, R.U. (1980): Salt Weathering on Arid Environment, I. Theoretical ConsiderationsII. Laboratory Studies. In: Papers in Geography, 8 ()Link to Google Scholar
[Stark.etal:1996] Stark, Jochen; Stürmer, Sylvia (1996): Bauschädliche Salze, Bauhaus-Univ. WeimarLink to Google Scholar
[Winkler:1975] Winkler, Erhard M. (1975): Stone: Properties, Durability in Man´s Environment, Springer Verlag, WienLink to Google Scholar

Weblinks[edit]

  1. ↑ http://webmineral.com/data/Gypsum.shtml seen on 30.07.2010
  2. ↑ http://www.mindat.org/min-1784.html seen on 30.07.2010

A phase is a physically distinctive form of matter and is characterized by having relatively uniform chemical and physical properties.

Calciumsulfatehemihydrate exists in two modifications: α - and β-hemihydrate. β-hemihydrate is formed in dry media, when gypsum is heated over 40°C, while α –hemihydrates is formed in aqueous media when heated over 97.2°C.

relative humidity

A molecule is an electrically neutral group of at least two atoms.

the mathematical difference between the largest and smallest refractive index for an anisotropic mineral

Scanning Electron Microscope

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