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Authors:  [[user:Hschwarz|Hans-Jürgen Schwarz ]], [[user:NMainusch|Nils Mainusch]], [[user:TMueller|Tim Müller]]
<br>English Translation by Sandra Leithäuser
<br>back to [[Sulfate]]
{{Infobox_Salt
{{Infobox_Salt
|Footnote            = <ref>http://webmineral.com/data/Gypsum.shtml seen on 30.07.2010</ref><ref>http://www.mindat.org/min-1784.html seen on 30.07.2010</ref>
|Footnote            = <ref>http://webmineral.com/data/Gypsum.shtml seen on 30.07.2010</ref><ref>http://www.mindat.org/min-1784.html seen on 30.07.2010</ref>
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|chemical_Name        = Calcium sulfate dihydrate
|chemical_Name        = Calcium sulfate dihydrate
|Trivial_Name        = Alabaster, Satin Spar, Selenite,  
|Trivial_Name        = Alabaster, Satin Spar, Selenite,  
|chemical_Formula    = Ca[SO<sub>4</sub>]•2H<sub>2</sub>O  
|chemical_Formula    = CaSO<sub>4</sub>•2H<sub>2</sub>O  
|Hydratforms          = Anhydrite (CaSO<sub>4</sub>)<br>Hemihydrate (CaSO<sub>4</sub>•0.5H<sub>2</sub>O)  
|Hydratforms          = CaSO<sub>4</sub> ([[Anhydrite]])<br> CaSO<sub>4</sub>•0.5H<sub>2</sub>O ([[Bassanite]])  
|Crystal_System      = monoclinic
|Crystal_System      = monoclinic
|Crystal_Structure    =  
|Crystal_Structure    =  
|Deliqueszenzhumidity = > 99% RH at 20°C
|Deliqueszenzhumidity = > 99% RH at 20°C
|Solubility          = 2.14 g/l
|Solubility          = 2.14 g/l
|Density              = 2.2-2.4 g/cm³  
|Density              = 2.31 g/cm³  
|MolVolume            = 74.69 cm<sup>3</sup>/mol  
|MolVolume            = 74.69 cm<sup>3</sup>/mol  
|Molweight            = 172.17g /mol  
|Molweight            = 172.17g /mol  
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|Crystal_Habit        =  flat, prismatic, needle- like crystal,  granular, massive aggregate
|Crystal_Habit        =  flat, prismatic, needle- like crystal,  granular, massive aggregate
|Twinning            = very common  
|Twinning            = very common  
|Refractive_Indices  = α = 1.519-1.521<br>β = 1.522-1.523<br>γ = 1.529-1.530
|Refractive_Indices  = α = 1.5207<br>β = 1.5230<br>γ = 1.5299
|Birefringence        = Δ = 0.010
|Birefringence        = Δ = 0.0092
|optical_Orientation  = biaxial positive
|optical_Orientation  = biaxial positive
|Pleochroism          = colorless
|Pleochroism          = colorless
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|chemBehavior        = hardly soluble in water
|chemBehavior        = hardly soluble in water
|Comments            =
|Comments            =
|Literature          =<bib id="Robie.etal:1978"/> <bib id="Dana:1951"/>
}}
}}
Authors:  [[user:Hschwarz|Hans-Jürgen Schwarz ]], [[user:NMainusch|Nils Mainusch]], [[user:TMueller|Tim Müller]]
 
<br>English Translation by Sandra Leithäuser
<br>back to [[Sulfate]]




Line 37: Line 41:
== Abstract  ==
== Abstract  ==


The article discusses the system CaSO<sub>4</sub>-H<sub>2</sub>O, in referecne to gypsum. Gypsum is one of the most important salts with regard to the damage of building materials and, particularly, wall-paintings. Objects exposed to exterior conditions where air pollution is present are the most prone to damage from gypsum. The appearance and mechanism of the damage, as well as the examination methods are described. Images, microphotographs and examples from practical experiences illustrate the subject.<br>
The article discusses the system CaSO<sub>4</sub>-H<sub>2</sub>O, in reference to gypsum. Gypsum is one of the most important salts in the deterioration of building materials and, particularly, wall-paintings. Objects exposed to exterior conditions where air pollution is present are the most prone to damage from gypsum. The appearance and mechanism of the damage, as well as the examination methods are described. Images, microphotographs and examples from practical experiences illustrate the subject.<br>
<br>
<br>


== Introduction  ==
== Introduction  ==


Gypsum is one of the most common salts causing the deterioration of inorganic porous building materials. It is present on most all exterior exposed surfaces and even in interior environments, under different shapes and induced deterioration patterns. <br>
Gypsum is one of the most common salts causing deterioration of inorganic porous building materials. It is present on most exterior exposed surfaces and even in interior environments, under different shapes and inducing various deterioration patterns. <br>
<br>
<br>
<br>
 
Gypsum, one of the most prevalent minerals, forms by precipitation from aqueous solution at temperatures under approximately 40°C. When the solution reaches higher temperatures (&gt; 60°C) anhydrite precipitates out. Calcium sulfate and calcium sulfate dihydrate are often present in rocks. Hemihydrate does not occur naturally.<br>
== Gypsum, one of the most prevalent minerals, forms by precipitation from aqueous solution at temperatures under approximately 40°C. At increased temperatures (&gt; 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.<br>


Gypsum occurs naturally in salt deposits and deserts, where "desert rose" crystals form in combination with quartz inclusions. In natural salt deposits, gypsum and anhydrite sometimes form a caprock, i.e., a massive layer of material covering the deposit.  
Gypsum occurs naturally in salt deposits and deserts, where "desert rose" crystals form in combination with quartz inclusions. In natural salt deposits, gypsum and anhydrite sometimes form a caprock, i.e., a massive layer of material covering the deposit.  
Synthetic gypsum is produced in coal-fired power plants, as a by-product of flue-gas desulfurization.  
Synthetic gypsum is produced in coal-fired power plants, as a by-product of flue-gas desulfurization.


== Origin and formation of gypsum on monuments ==
== Origin and formation of gypsum on monuments ==


On monuments made from porous inorganic building materials, particularly in urban environment where air pollutants are present, in particular sulfur oxides (SO<sub>x</sub>) that convert to sulfuric acid in the presence of moisture, the reaction of these gases with any calcium carbonate present in limestone, mortars, renders, results in the formation of gypsum. The reaction taking place can be simplified as follows:   
On monuments made from porous inorganic building materials, particularly in urban environment where anthropogenic air pollutants are present, such as sulfur oxides (SO<sub>x</sub>) that eventually convert to sulfuric acid in the presence of moisture, the reaction of these gases with any calcium carbonate present in limestone, sandstone, mortars, renders, results in the formation of gypsum. The reaction taking place can be simplified as follows:   


CaCO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + H<sub>2</sub>O + CO<sub>2</sub>
CaCO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → CaSO<sub>4</sub> + H<sub>2</sub>O + CO<sub>2</sub>
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It is to be remembered that gypsum can be a major component of some mortars, plasters and even some building stones (e.g., selenite, used for the base of the Garrisenda Tower in Bologna, Italy) thus being an integral part of the monuments fabric.  
It is to be remembered that gypsum can be a major component of some mortars, plasters and even some building stones (e.g., selenite, used for the base of the Garrisenda Tower in Bologna, Italy) thus being an integral part of the monuments fabric.  
<br>
<br>


==  Damage potential and weathering activity  ==
==  Damage potential and weathering activity  ==


=== Solubility properties  ===
=== Solubility properties  ===
[[file:CaSO4-Steiger-1.jpg|thumb|350px|right|'''Figure1:''' Solubility of CaSO4 in water (diagram: Michael Steiger)]]
[[file:CaSO4-Steiger-1.jpg|thumb|350px|right|'''Figure1:''' Solubility of CaSO4 in water (diagram: Michael Steiger)]]
<br>Gypsum belongs to the group of salts with a low solubility in aqueous solution and therefore is less mobile than the more soluble ones. However, the when other ions are present, its solubility can be significantly increased. For example, when halite is present, the  solubility of gypsum can be increased by a factor four depending on the concentration ratio of the two salts. <br>
Gypsum belongs to the group of salts with a low solubility in aqueous solution and therefore is less mobile than the more soluble ones. However, when other ions are present, its solubility can be significantly increased. For example, when halite, NaCl, is present, the  solubility of gypsum can be increased by a factor four depending on the concentration ratio of the two salts. <br>


[[file:Loeslichkeit Gips 02.JPG|thumb|right|350px|'''Figure 2:'''Solubility of gypsum compared with other salts  (after <bib id="Stark.etal:1996"/>)]]
[[file:Loeslichkeit Gips 02.JPG|thumb|right|350px|'''Figure 2:'''Solubility of gypsum compared with other salts  (after <bib id="Stark.etal:1996"/>)]]
<br clear=all>


=== Hydration behavior  ===
=== Hydration behavior  ===
 
The system CaSO<sub>4 </sub>–H<sub>2</sub>O: <br> Calcium sulfate can appear in three different hydrate phases:  
The system CaSO<sub>4 </sub>– H<sub>2</sub>O: <br> Calcium sulfate can appear in three different hydrate phases:  
*Anhydrite (CaSO<sub>4</sub>)- the above mentioned anhydrous form.  
*Anhydrite (CaSO<sub>4</sub>)- the above mentioned anhydrous form.  
*Hemihydrate (CaSO<sub>4</sub>0.5 H<sub>2</sub>O)- a metastable form.
*Bassanite (hemihydrate) (CaSO<sub>4</sub>•0.5H<sub>2</sub>O)- a metastable form.
*Gypsum (CaSO<sub>4</sub>2 H<sub>2</sub>O)- calcium sulfate dihydrate.   
*Gypsum (CaSO<sub>4</sub>•2H<sub>2</sub>O)- 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. <br>
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. <br>
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 SO<sub>3</sub> is effected.
<br clear=all>


Anhydrite exists in different varieties with different chemical properties, such as different solubilities in water, depending on the conditions of its formation. The same applies to bassanite, the hemihydrate. <br>
The transition temperature in aqueous solution for the gypsum-bassanite (dihydrate to hemihydrate) is in the 40°C-66°C range. 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°-60°C. However, in parallel with this reaction, metastable hemihydrate can also precipitate being subsequently transformed into the more stable dihydrate form. <br>
When heating the dihydrate (as a solid and dry) to approximately 50°C, the chemically combined water is lost leaving the hemihydrate. However, a complete transition to hemihydrate only takes place at temperatures of around 100°C. If the 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 SO<sub>3</sub> is effected.
<br clear="all">
=== Hygroscopicity ===
=== Hygroscopicity ===


[[File:Veraenderung Loeslichkeit durch Fremdionen Gips .JPG|thumb|right|350px|'''Figure 3''':  
[[File:Veraenderung Loeslichkeit durch Fremdionen Gips .JPG|thumb|right|350px|'''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 <bib id="DAns:1933"/>)]]. The pure gypsum salt has no defined [[deliquescence|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.  
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 <bib id="DAns:1933"/>)]]The pure gypsum salt has no defined [[deliquescence|deliquescence]] point. If, in the presence of halite, the relative humidity levels exceed 90% RH, gypsum crystals may dissolve, due to the deliqusecent behavior of halite. A decrease of humidity levels to approximately 75% RH will result in the recrystallization of gypsum.


=== Crystallization pressure  ===
=== Crystallization pressure  ===
Line 94: Line 91:
=== Hydration pressure  ===
=== Hydration pressure  ===


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 [[Schadensmechanismen|hydration pressure]] [Zahlenwerte nach <bib id="Sperling.etal:1980"/>]. 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/mm<sup>2</sup> can be effected- an extremely high value [ <bib id="Stark.etal:1996"/>].
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 [[Schadensmechanismen|hydration pressure]] [values according to <bib id="Sperling.etal:1980"/>]. 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/mm<sup>2</sup> can result -an extremely high value [according to <bib id="Stark.etal:1996"/>].


== Conversion reaction  ==
== Conversion reaction  ==
Line 190: Line 187:
== Under the Scanning Electron Microscope (SEM)==   
== Under the Scanning Electron Microscope (SEM)==   
<gallery caption="In a SEM" widths="200px" heights="150px" perrow="3">   
<gallery caption="In a SEM" widths="200px" heights="150px" perrow="3">   
Image:SA100_1.jpg | Gypsum crystals in a SEM
Image:SA100_1.jpg | SEM micrograph of gypsum crystals.
Image:SG2-2.jpeg  | Gypsum crystals in a SEM
Image:SG2-2.jpeg  | SEM of gypsum crystals.
Image:SG2-3.jpg | Gypsum crystals in a SEM
Image:SG2-3.jpg | SEM of gypsum crystals.
Image:SG3-SPC2.jpeg|EDX spektra of gypsum crystals in a SEM  
Image:SG3-SPC2.jpeg|EDX spectra of gypsum crystals.  
Image:SG3-3.jpeg  | Gypsum crystals in a SEM
Image:SG3-3.jpeg  | SEM of gypsum crystals.
Image:SG3-4.jpeg | Gypsum crystals in a SEM
Image:SG3-4.jpeg | SEM of gypsum crystals.
Image:SG1-5.jpeg | Gypsum crystals in a SEM
Image:SG1-5.jpeg | SEM of gypsum crystals.
Image:SG1-SPC.jpeg| EDX spektra of gypsum crystals in a SEM
Image:SG1-SPC.jpeg| EDX spectra of gypsum crystals.
</gallery>  
Image:Gypsum star.jpg|SEM of gypsum crystals grown from the hemihydrate.</gallery>  
<br clear=all>
<br clear=all>
== Literatur  == 
 
<biblist/>
 
 
 


==  Weblinks ==   
==  Weblinks ==   
<references />  
<references />  


== Literature  == 
<biblist/>
More Literature :
<bibprint filter="year:2011,  author:%Badosa%"/>
<bibprint filter="year:2007, volume:52, author:%Charola%"/>
<bibprint filter="year:1901, volume:5, author:%Cameron%"/>
<bibprint filter="year:1989, volume:34, author:%Ahad%"/>
<bibprint filter="year:1991,  author:%Livingston%"/>
<bibprint filter="year:1997,  author:%Neumann%, author:%Juling%"/>
<bibprint filter="year:1994,  author:%Schlütter%"/>
<bibprint filter="year:2009,  author:%Zehnder%"/>


   
   
[[Category:Gipsum]][[Category:Sulphate]][[Category:Salt]][[Category:InReview]][[Category:Sulfate]][[Category:Müller,Tim]][[Category:Mainusch,Nils]][[Category:Schwarz,Hans-Jürgen]]
[[Category:Gipsum]][[Category:Sulphate]][[Category:Salt]][[Category:editing]][[Category:Sulfate]][[Category:Müller,Tim]][[Category:Mainusch,Nils]][[Category:Schwarz,Hans-Jürgen]][[Category:List]]

Latest revision as of 10:55, 3 May 2023

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


Gypsum[1][2]
SA101 1.jpeg
Mineralogical name Gypsum
Chemical name Calcium sulfate dihydrate
Trivial name Alabaster, Satin Spar, Selenite,
Chemical formula CaSO4•2H2O
Other forms CaSO4 (Anhydrite)
CaSO4•0.5H2O (Bassanite)
Crystal system monoclinic
Crystal structure
Deliquescence humidity 20°C > 99% RH at 20°C
Solubility (g/l) at 20°C 2.14 g/l
Density (g/cm³) 2.31 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 = 1.5207
β = 1.5230
γ = 1.5299
Birefringence Δ = 0.0092
Optical Orientation biaxial positive
Pleochroism colorless
Dispersion 58°
Used Literature
[Robie.etal:1978]Title: Thermodynamic properties of minerals and related substances at 298.15 K and 1 bar pressure and higher temperatures
Author: Robie R.A., Hemingway B.S.; Fisher J.A.
Link to Google Scholar
[Dana:1951]Title: Dana's System of Mineralogy
Author: Dana J.D.
Link to Google Scholar




Calcium sulfate and gypsum[edit]

Abstract[edit]

The article discusses the system CaSO4-H2O, in reference to gypsum. Gypsum is one of the most important salts in the deterioration of building materials and, particularly, wall-paintings. Objects exposed to exterior conditions where air pollution is present are the most prone to damage from gypsum. The appearance and mechanism of the damage, as well as the examination methods are described. Images, microphotographs and examples from practical experiences illustrate the subject.

Introduction[edit]

Gypsum is one of the most common salts causing deterioration of inorganic porous building materials. It is present on most exterior exposed surfaces and even in interior environments, under different shapes and inducing various deterioration patterns.

Gypsum, one of the most prevalent minerals, forms by precipitation from aqueous solution at temperatures under approximately 40°C. When the solution reaches higher temperatures (> 60°C) anhydrite precipitates out. Calcium sulfate and calcium sulfate dihydrate are often present in rocks. Hemihydrate does not occur naturally.

Gypsum occurs naturally in salt deposits and deserts, where "desert rose" crystals form in combination with quartz inclusions. In natural salt deposits, gypsum and anhydrite sometimes form a caprock, i.e., a massive layer of material covering the deposit. Synthetic gypsum is produced in coal-fired power plants, as a by-product of flue-gas desulfurization.

Origin and formation of gypsum on monuments[edit]

On monuments made from porous inorganic building materials, particularly in urban environment where anthropogenic air pollutants are present, such as sulfur oxides (SOx) that eventually convert to sulfuric acid in the presence of moisture, the reaction of these gases with any calcium carbonate present in limestone, sandstone, mortars, renders, results in the formation of gypsum. The reaction taking place can be simplified as follows:

CaCO3 + H2SO4 → CaSO4 + H2O + CO2

It is to be remembered that gypsum can be a major component of some mortars, plasters and even some building stones (e.g., selenite, used for the base of the Garrisenda Tower in Bologna, Italy) thus being 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 is less mobile than the more soluble ones. However, when other ions are present, its solubility can be significantly increased. For example, when halite, NaCl, is present, the solubility of gypsum can be increased by a factor four depending on the concentration ratio of the two salts.

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 (CaSO4)- the above mentioned anhydrous form.
  • Bassanite (hemihydrate) (CaSO4•0.5H2O)- a metastable form.
  • Gypsum (CaSO4•2H2O)- calcium sulfate dihydrate.

Anhydrite exists in different varieties with different chemical properties, such as different solubilities in water, depending on the conditions of its formation. The same applies to bassanite, the hemihydrate.
The transition temperature in aqueous solution for the gypsum-bassanite (dihydrate to hemihydrate) is in the 40°C-66°C range. 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°-60°C. However, in parallel with this reaction, metastable hemihydrate can also precipitate being subsequently transformed into the more stable dihydrate form.
When heating the dihydrate (as a solid and dry) to approximately 50°C, the chemically combined water is lost leaving the hemihydrate. However, a complete transition to hemihydrate only takes place at temperatures of around 100°C. If the 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, the relative humidity levels exceed 90% RH, gypsum crystals may dissolve, due to the deliqusecent behavior of halite. A decrease of humidity levels to approximately 75% RH will result in 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 [values according to [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 result -an extremely high value [according to [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]


Under the polarising microscope[edit]


Under the Scanning Electron Microscope (SEM)[edit]




Weblinks[edit]

Literature[edit]

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