Mirabilite: Difference between revisions
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Mirabilite which is the deacahydrate of sodium sulfate and its properties are presented. | Mirabilite which is the deacahydrate of sodium sulfate and its properties are presented. | ||
== Occurrence == | == Occurrence == | ||
Both [[thenardite]] and mirabilite appear as natural minerals. Sodium sulfate occurs naturally in mineral waters, as deposits of former salt lakes and in the form of different double salts. Knowledge of sodium sulfate containing crystalline water can be traced back to the 16th century. It was first described by Glauber in 1658, who referred to it as "sal mirable". Based on his name, the trivial name "Glauber's salt" for Mirabilite can also be found in the literature. | |||
== | == Origin and formation of thenardite / mirabilite in monuments == | ||
The introduction of materials containing soluble sodium compounds can lead to the formation of sodium sulfate as an efflorescence salt in the mineral system of a monument, if the air is contaminated with sulfurous gases or other sources of sulfate are present. Cements with a high sodium ion content may contain up to 0.5% soluble alkalis according to DIN specifications. In purely mathematical terms, 100 kg of Portland cement with a content of only 0.1% soluble Na2O can form 520 g of mirabilite in air containing sulfuric acid [data according to Arnold/Zehnder 1991]. An abundance of cleaning materials and especially formerly used restoration products (such as water glass) can introduce sodium ions into architectural monuments. Other sources are groundwater and surface water, which may contain Na+ ions. Road salt consists largely of readily soluble [[Halite|sodium chloride]]. Near the coast, seawater containing NaCl must be considered as a source of sodium. | |||
== Solubility properties == | == Solubility properties == | ||
[[file:S Na2SO4.jpg|thumb| | [[file:S Na2SO4.jpg|thumb|600px|left|'''Figure1''': Solubilities in the system Na<sub>2</sub>SO<sub>4</sub>-H<sub>2</sub>O in dependence of the temperature [according to <bib id="Steiger.etal:2008"/>].]] | ||
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| Line 57: | Line 57: | ||
== Hygroscopicity == | == Hygroscopicity == | ||
[[file:D Na2SO4e.jpg|thumb| | [[file:D Na2SO4e.jpg|thumb|600px|left|'''Figure 2''': Deliquescence behaviour in the system Na<sub>2</sub>SO<sub>4</sub>-H<sub>2</sub>O and equilibrium humbidities for the transformation thenardite/mirabilite, according to <bib id="Steiger.etal:2008"/>]] | ||
Figure 2 illustrates the influence of temperature on the deliquescence humidities of mirabilite and on the other phases of sodium sulfate. It is notable that for mirabilite and [[thenardite]] the graphs of the deliquescence humidities run in opposite directions. Unlike the deliquescence humidity of | Figure 2 illustrates the influence of temperature on the deliquescence humidities of mirabilite and on the other phases of sodium sulfate. It is notable that for mirabilite and [[thenardite]] the graphs of the deliquescence humidities run in opposite directions. Unlike the deliquescence humidity of thenardite those of mirabilite decreases with increasing temperature.<br> | ||
The deliquescence humidity of mirabilite lies always above 87 % in its stable temperature range (table 1). See also [[sodium sulfate]] | The deliquescence humidity of mirabilite lies always above 87 % in its stable temperature range (table 1). See also [[sodium sulfate]] | ||
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Latest revision as of 07:39, 3 May 2023
Authors: Hans-Jürgen Schwarz, Nils Mainusch
English version by Christa Gerdwilker
back to Sulfate
| Mirabilite[1][2] | |
| |
| Mineralogical name | Mirabilite |
| Chemical name | Sodium sulfate decahydrate |
| Trivial name | Glauber salt, Reussin, Soda Sulfate |
| Chemical formula | Na2SO4•10H2O |
| Other forms | Na2SO4•7H2O (sodium sulfate heptahydrate) |
| Crystal system | monoclinic |
| Crystal structure | |
| Deliquescence humidity 20°C | 95.6 % |
| Solubility (g/l) at 20°C | 1.353 mol/kg |
| Density (g/cm³) | 1.466 g/cm³ |
| Molar volume | 219.8 cm3/mol |
| Molar weight | 322.19 g/mol |
| Transparency | transparent to opaque |
| Cleavage | perfect |
| Crystal habit | |
| Twinning | |
| Phase transition | |
| Chemical behavior | |
| Comments | soluble in water and glycerin, insoluble in pure alcohol easily loses some water, converts to thenardite at 32°C abnormal blue or brown interference colors |
| Crystal Optics | |
| Refractive Indices | nx = 1.394 ny = 1.396 nz = 1.398 |
| Birefringence | Δ = 0.004 |
| Optical Orientation | negative |
| Pleochroism | |
| Dispersion | 76° |
| 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.  [Dana:1951]Title: Dana's System of MineralogyAuthor: Dana J.D.
| |
Abstract[edit]
Mirabilite which is the deacahydrate of sodium sulfate and its properties are presented.
Occurrence[edit]
Both thenardite and mirabilite appear as natural minerals. Sodium sulfate occurs naturally in mineral waters, as deposits of former salt lakes and in the form of different double salts. Knowledge of sodium sulfate containing crystalline water can be traced back to the 16th century. It was first described by Glauber in 1658, who referred to it as "sal mirable". Based on his name, the trivial name "Glauber's salt" for Mirabilite can also be found in the literature.
Origin and formation of thenardite / mirabilite in monuments[edit]
The introduction of materials containing soluble sodium compounds can lead to the formation of sodium sulfate as an efflorescence salt in the mineral system of a monument, if the air is contaminated with sulfurous gases or other sources of sulfate are present. Cements with a high sodium ion content may contain up to 0.5% soluble alkalis according to DIN specifications. In purely mathematical terms, 100 kg of Portland cement with a content of only 0.1% soluble Na2O can form 520 g of mirabilite in air containing sulfuric acid [data according to Arnold/Zehnder 1991]. An abundance of cleaning materials and especially formerly used restoration products (such as water glass) can introduce sodium ions into architectural monuments. Other sources are groundwater and surface water, which may contain Na+ ions. Road salt consists largely of readily soluble sodium chloride. Near the coast, seawater containing NaCl must be considered as a source of sodium.
Solubility properties[edit]
Author: Steiger, Michael; Asmussen, Sönke
].
The solubility of mirabilite is 1.35 mol/kg at 20 °C. The solubility shows a high temperature dependence, it decreases with decreasing temperatures and it increases at higher temperatures. Above 32.4 °C mirabilite is unstable, so thenardite is the stable phase at higher temperatures.
see Sodium sulfate
Hygroscopicity[edit]
Author: Steiger, Michael; Asmussen, Sönke
Figure 2 illustrates the influence of temperature on the deliquescence humidities of mirabilite and on the other phases of sodium sulfate. It is notable that for mirabilite and thenardite the graphs of the deliquescence humidities run in opposite directions. Unlike the deliquescence humidity of thenardite those of mirabilite decreases with increasing temperature.
The deliquescence humidity of mirabilite lies always above 87 % in its stable temperature range (table 1). See also sodium sulfate
| 0°C | 10°C | 20°C | 30°C |
| 98.8%r.h. | 97.8%r.h. | 95.6%r.h. | 90.1%r.h. |
The presence of other ions, as in the case of salt mixtures, can significantly alter the equilibrium humidity parameters, i.e., the temperature and humidity conditions which initiate phase changes. Table 2 lists the experimentally determined equilibrium humidity of different salt mixtures. This shows that the equilibrium humidity of pure mirabilite is higher than that of the other salts.
| MgSO4 | Ca(NO3)2 | KNO3 | |
| Na2SO4 • 10H2O | 87(21°C) | 74 (21°C) | 81(21°C) |
Crystallization pressure[edit]
The crystallization of mirabilite from aqueous solution results in a crystallization pressure of 7.2-8.3 N/mm2.
Hydration behavior[edit]
The Na2SO4 – H2O system:
The only stable forms of sodium sulfate are the decahydrate (mirabilite) and the anhydrite (thenardite). The generation of mirabilite by recrystallization of the salt from an aqueous supersaturated solution occurs at 32.4°C. In particular, the transition from thenardite to mirabilite and the incorporation of 10 water molecules in the crystal lattice causes a volume expansion of 320%. This transition happens at a relatively low temperature (32-35°C), the damage caused by this salt is highly dependent on the temperature and thus on the environment. This temperature range is given as a guide, because this transition could happen for example at 25°C at 80% relative humidity, or even at 0°C at 60.7% relative humidity [information from Gmelin]. Due to this strong dependence on the environmental parameters, an estimate of the damage caused on buildings by crystallization and hydration of sodium sulfate are very difficult to obtain.
Analytical evidence[edit]
Microscopy
[edit]
Laboratory analysis:
Observations of the solubility behavior through the microscope allows to verify the high water solubility of sodium sulfate and its insolubility in ethanol. Thenardite and mirabilite do not have morphological characteristics to aid their identification during simple recrystallization experiments. Instead, a broad range of different forms can be observed.
Refractive indices: nx = 1,395; ny =1.396-1.410; nz =1.398-1.419
Birefringence: Δ = 0.04-0,023
Crystal classe: monocline
Under the polarizing microscope:
The crystallization water content of the sample or its re-crystallized form depends on the ambient RH and temperature levels. In dry air (lower than 80% RH at room temperature) mirabilite loses its water of crystallization content and changes to thenardite. This process can be observed during recrystallization under the microscope. Mirabilite has characteristic abnormal interference colors which weaken during water loss and the formation of thenardite.
Differentiation from different salts:
Generally, the differentiation of certain sulfates (listed below and including thenardite) without the microchemical determination of the cations is problematic as their refractive indices are close to each other and all salts display a slight double refraction. The use of an immersion material with a nD-value of 1.48 is helpful and allows the differentiation of salts within this group. Additionally, the properties listed below can also be taken into consideration. Thenardite can be determined indirectly by the appearance of mirabilite during recrystallization to the hydrated form.
| Salt phase | Characteristics |
| Boussingaultite (NH4)2Mg(SO)4 • 6H20 | no abnormal interference colors/oblique extinction |
| Picromerite K2Mg(SO4)2 • 6H20 | no abnormal interference colors/oblique extinction |
| Bloedite Na2Mg(SO4)2 • 6H20 | all indices >1.48 / no abnormal interference colors/oblique extinction / negative optical orientation |
| Glaserite K3Na(SO4)2 | all indices >1.48 / no abnormal interference colors/oblique extinction |
| Arcanite K2SO4 | all indices >1.48 / no abnormal interference colors |
| Dashkovaite Mg(HCO2)2 • 2H2O | relatively high birefringence/ no abnormal interference colors/oblique extinction |
Mixtures:
Mixed systems Na+– Ca2+– SO4 2-: Due to its lower solubility, gypsum precipitates first during re-crystallization. The characteristic needle shaped gypsum crystals are the first to form while sodium sulfate precipitates later, the crystal growth is noticeably faster but the morphology is non-specific.
Mixed system Na+– SO4 2-– Cl-: The precipitation of both types of particles begins practically at the same time. Halite has a characteristic morphology whereas sodium sulfate occurs in extremely varying forms.
Under the polarizing microscope[edit]
- Sodium sulfate crystallization between two glass slides
Photo taken through crossed polars and red I
Photo taken through crossed polars
Weblinks
[edit]
- ↑ http://webmineral.com/data/Mirabilite.shtml accessed 29/07/2010
- ↑ http://www.mindat.org/min-2725.html accessed 29/07/2010
Literatur[edit]
| [Dana:1951] | Dana E.S. (eds.) Dana J.D. (1951): Dana's System of Mineralogy, 7, Wiley & Sons | |
| [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 () | |
| [Steiger.etal:2008] | Steiger, Michael; Asmussen, Sönke (2008): Crystallization of sodium sulfate phases in porous materials: The phase diagram Na2SO4–H2O and the generation of stress. In: Geochimica et Cosmochimica Acta, 72 (17), 4291-4306, Url | |
| [Vogt.etal:1993] | Vogt, R.; Goretzki, Lothar (1993): Der Einfluss hygroskopischer Salze auf die Gleichgewichtsfeuchte und Trocknung anorganischer Baustoffe, unveröffentlichter Bericht. | |