Kieserite

Kieserite
HJS MgSO4 092503-3.jpg
Mineralogical name	Kieserite
Chemical name	Magnesiumsulfate Monohydrate
Trivial name
Chemical formula	Mg[SO4] • H2O
Other forms	Sanderite (MgSO4•2H2O) Starkeyite (MgSO4•4H2O) Pentahydrite (MgSO4•5H2O) Hexahydrite (MgSO4•6H2O) Epsomite (MgSO4•7H2O) Meridianite (MgSO4•11 H2O) Magnesium 12-Hydrate
Crystal system	monoclinic
Crystal structure	monoclinic prismatic
Deliquescence humidity 20°C
Solubility (g/l) at 20°C	684 g/l (100°C)
Density (g/cm³)	2.57 g/cm3
Molar volume	53.85 cm3/mol
Molar weight	138.9 g/mol
Transparency	translucent
Cleavage	perfect
Crystal habit
Twinning
Phase transition
Chemical behavior
Comments	can be produced from an aqueous solution over 67°C
Crystal Optics
Refractive Indices	nx = 1.523-1.520 ny = 1.535-1.533 nz = 1.586-1.584
Birefringence	Δ = 0.063-0.064
Optical Orientation	biaxial positive
Pleochroism
Dispersion	55°
Used Literature
{{{Literature}}}

Authors: Hans-Jürgen Schwarz, Tim Müller
English version by Christa Gerdwilker
back to Sulfate

Abstract

Overview of the magnesium sulfate ‘kieserite’.

Occurrence of kieserite

Kieserite rarely forms individual crystals. The magnesium sulfate hydrate occurs in natural salt deposits together with sylvine and halite. These can be found in the alps as well as Northern Germany, Italy ( Mt. Vesuvius), Arizona (Bisbee), Nevada and Washington (Mt. Kruger). More commonly epsomite occurs as efflorescence on magnesian stone. These stones generally also contain significant amounts of carbonate (calcite or dolomite). Kieserite is precipitated during the evaporation of liquids and as secondary mineral during the oxidation of iron sulfides. It also forms on natural stone surfaces where it can cause substantial damages.

Information on the origins and formation of kieserite on monuments

Magnesium sulfate forms on surfaces which offer a source of magnesium ions. These can be found in different materials:

• Lime with dolomitic content:

Dolomite is a double salt which can contain both calcium and magnesium. Carbonate forms the negatively charged ion. Dolomitic lime is used to manufacture mortar. Burning dolomitic limestone and slaking the resultant lime results in the formation of pure salts (CaCO₃ and MgCO₃). The solubility of magnesite (1,76 g/l) is noticeably higher than that of the pure calcite (0,014 g/l) or of dolomite (0,078 g/l). Dampness in the masonry can cause magnesium bonds to dissolve and salts to re-form on drying. This can lead to the formation of sulfates, especially if the use of gypsum-rich products on the same object offer a ready source of sulfate ions.

CaMg[CO₃]₂ -> CaCO₃ + MgCO₃

MgCO₃ + n H₂O -> Mg²⁺ aq + CO₃^2- aq

Mg²⁺ + SO4^2- -> MgSO₄

• Magnesia binder:

Magnesia binder also contains magnesium compounds which can form hygroscopic salts. These are a source of magnesium which, in combination with sulfate ions, can lead to the formation of magnesium sulfate.

• Cement:

Cement also contains magnesium. To prevent damage, DIN 1164 stipulates that cement must not contain more than 5M% as magnesium can also be dissolved from cement and form sulfates. A further source of magnesium ions in solution can be road gritting salts as these often contain small amounts of magnesium chloride. Ions dissolved in the ground can also be problematic if transported to the surfaces by capillary action.

Solubility behavior

Image 1:Solubility in water MgSO4, Graphic: M. Steiger

The water solubility of kieserite is 684 g/l at a temperature of 100 °C [Steiger and Asmussen,2008]. It subsequently belongs, like all discussed forms of magnesium sulphate with a solubility of clearly above 100 g/l (at 20 °C) to the group of very water soluble salts. This entails a high risk of salt mobility and frequent re-deposition of salts within the material matrix. Due to the influence of temperature on solubility, a rapid drop in temperature can result in the precipitation of salts [Mainusch:2001]Title: Erstellung einer Materialsammlung zur qualitativen Bestimmung bauschädlicher Salze für Fachleute der Restaurierung
Author: Mainusch, Nils

Hygroscopicity

The low hygroscopicity of the pure kieserite salt (illustrated by its 42% equilibrium RH) cannot be examined on its own.

Image 2: Deliquescence humidity of MgSO₄, Graphic: M. Steiger

The sorption point of mixed systems, i.e. in the presence of other ions, is lower. The possibility of hygroscopic moisture absorption and associated problems is still present, in spite of the high deliquescence point [Mainusch:2001]Title: Erstellung einer Materialsammlung zur qualitativen Bestimmung bauschädlicher Salze für Fachleute der Restaurierung
Author: Mainusch, Nils

Hydration behavior

The six hydrate forms of magnesium sulfate listed above are shown to be stable compounds. With the exception of magnesium sulfate-12-hydrates, all the above crystal water phases of magnesium sulfate have been found on monuments. These predominantly occur as epsomite, hexahydrite, pentahydrite und kieserite.

Kieserite is the magnesium sulfate monohydrate. It can be formed through the dehydration of magnesium sulfate hydrates. A water-loss resultant reduction in volume occurs during this change. Increased relative humidity also results in an increased hydrate-water content within the magnesium sulfate. Kieserite is stable at room temperature (25°C) up to a RH of approx. 42 % , above this the change to hexahydrite or epsomite occurs. Hexahydrite is stable below 51 % RH, above this epsomite is formed. The phase changes can happen directly or via solution and re-crystallization. This results in the metastable existence of the lower hydration phase up to its deliquescence humidity. Above this RH the phase dissolves and a supercritical solution is formed, from which the hydrated phase crystallizes [Steiger.etal:2008]Title: Crystallization of sodium sulfate phases in porous materials: The phase diagram Na2SO4–H2O and the generation of stress
Author: Steiger, Michael; Asmussen, Sönke
.

Transition reactions

see magnesium sulfate

Analytical validation

Micro chemistry

see magnesium sulfate

Microscopy

Polarizing microscope investigations:

During microscopic investigations, it is important to remember that hexahydrite is the stable phase in ambient room conditions, i.e. a temperature of approx. 20 °C and RH of approx. 40%. Subsequently, the environmental conditions need to be changed to allow the crystallization of kieserite to be observed.

Since it is an optically anisotropic mineral, it displays a birefringence when viewed through crossed polars. Its interference colors are low and within the first order. The refractive indices are around α=1,520 β=1,533 γ=1,584 with a birefringence of 0,01. In comparison with other sulfates and salts, the refractive indices are relatively high. The birefringence is in the lower region of the sulfates and very low in comparison to nitrates.

Literature

[Broul.etal:1981]	Elsevier (eds.) Broul M., Nyvlt J.; Soehnel O. (1981): Solubility in organic two component systems, Elsevier
[Dana:1951]	Dana E.S. (eds.) Dana J.D. (1951): Dana's System of Mineralogy, 7, Wiley & Sons
[Friedrich.etal:1961]	Friedrich K., Kuhn R., Strunz H. (1961): Identität von Wathlingenit mit Kieserit. In: Kali Steinsalz, 3 (7), 221-227
[Mainusch:2001]	Mainusch, Nils (2001): Erstellung einer Materialsammlung zur qualitativen Bestimmung bauschädlicher Salze für Fachleute der Restaurierung, Diplomarbeit, HAWK Hochschule für angewandte Wissenschaft und Kunst Hildesheim/Holzminden/Göttingen, file:Diplomarbeit Nils Mainusch.pdf
[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
[Steiger.etal:2011a]	Steiger, Michael; Linnow, Kirsten; Ehrhardt, Dorothee; Rohde, Mandy (2011): Decomposition reactions of magnesium sulfate hydrates and phase equilibria in the MgSO4-H2O and Na+-Mg2+-Cl--SO42--H2O systems with implications for Mars. In: Geochimica et Cosmochimica Act, 75 (12), 3600-3626, 10.1016/j.gca.2011.03.038,

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

crystallization of a dissolved salt

relative humidity

the relative humidity, above which a material, e.g. a salt, absorbes humidity from the air and dissolves.

a mineral with more than one principal refractive index.

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

Hochschule für angewandte Wissenschaft und Kunst Hildesheim/Holzminden/Göttingen, University of Applied Sciences and Arts Hildesheim/Holzminden/Göttingen