Natrite

<bibimport/> Authors: Hans-Jürgen Schwarz, Nils Mainusch
English version by Christa Gerdwilker
back to Carbonate

Natrite
Mineralogical name	Natrite
Chemical name	Sodium carbonate
Trivial name
Chemical formula	Na2CO3
Other forms	Sodium carbonate hydrate (Na2CO3•H2O) Sodium carbonate heptahydrate (Na2CO3•7H2O) Sodium carbonate decahydrate (Na2CO3•10H2O)
Crystal system	monoclinic
Crystal structure
Deliquescence humidity 20°C
Solubility (g/l) at 20°C	210 g/l
Density (g/cm³)	2.532 g/cm3
Molar volume
Molar weight	105.99 g/mol
Transparency
Cleavage	good
Crystal habit
Twinning
Phase transition
Chemical behavior	alkaline in aqueous solution, pH ≈ 12
Comments	blooms quickly in dry air and passes into the monohydrate pH about 12
Crystal Optics
Refractive Indices	nx = 1.415 ny = 1.535 nz = 1.546
Birefringence	Δ = 0.131
Optical Orientation	biaxial negative
Pleochroism
Dispersion
Used Literature
{{{Literature}}}

Occurrence

Sodium carbonates occur naturally in solid salt deposits, in salt lakes e.g. Lake Magadi in East Africa or Owens Lake in California. Varying amounts of natural sodium carbonate can also be found in alkaline springs. Different extraction techniques have been developed to produce pure sodium carbonate through dissolution, purification and evaporation processes.

Information on the origins and formation of nitrate on monuments

Sodium carbonate can be formed within the mineral matrix of monuments in direct contact with soluble sodium compounds which can lead to salt efflorescence.

Cements containing up to 0.5% soluble alkalis (in accordance with DIN standards) have a high content of sodium ions. It can be calculated that 1g of Na₂O can lead to the formation of 4.6g of sodium carbonate decahydrate. If, for example, a Portland cement only contains 0.1% Na₂O then 0.45kg of sodium carbonate can be formed per100kg of cement [Arnold.etal:1991]Title: Monitoring Wall Paintings Affected by soluble Salts
Author: Arnold, Andreas; Zehnder, Konrad
. A large number of cleaning materials and, in particular, previously used conservation products (like waterglass) can introduce sodium ions into monuments. Further sources are ground and surface water which may contain Na⁺-ions. Gritting salt largely consists of very soluble sodium chloride. In coastal areas seawater contains NaCl and must thus be considered as a source of sodium.

Decay mechanisms of natrite

Solubility behavior

The three types of sodium carbonates found on monuments are very water soluble which is generally associated with high salt mobility. Temperature has a pronounced influence on the solubility behavior of thermonatrite and natrite in water. As a consequence, dropping temperatures may result in the oversaturation of such water solutions with the subsequent precipitation of natrite, even though the water content remains the same.

Diagram 1 – Illustration of temperature controlled solubility changes in thermonatrite and natrite in comparison with other salt phases (solubility data, Schwarz and Stark/Stürmer 1993).

Hygroscopicity

It is difficult to evaluate the hygroscopicity of sodium carbonates found in situ as the sorption and saturation points are influenced by local conditions (other ions, hydrate forms and temperature levels) and subsequently vary considerably.

The table below illustrates the deliquescence humidity of natrite in relation to the ambient temperature (see also table Equilibrium humidity in relation to temperature):

Table1: Deliquescence humidity of natrite [ [Arnold.etal:1991]Title: Monitoring Wall Paintings Affected by soluble Salts
Author: Arnold, Andreas; Zehnder, Konrad
]

15°C	20°C	25°C	30°C
96,5% RH	97,9% RH	88,2% RH	83,2% RH

Crystallization pressure

The crystallization of thermonatrite from an aqueous solution results in a crystallization pressure of 28.0-33.3 N/mm², whereas the crystallization pressure for natrite is 7.8-9.2N/mm² (for comparison, the crystallization pressure data of other masonry decaying salts: 7.2-65.4 N/mm²) [Winkler:1975]Title: Stone: Properties, Durability in Man´s Environment
Author: Winkler, Erhard M.
.

Hydration behavior

The compound Na₂CO₃ and H₂O:

Three stable hydrate forms of the Na₂CO₃ and H₂O compound can be found on monuments: 10-hydrate (sodium carbonate decahydrate), 7-hydrate (sodium carbonate heptahydrate) and 1-hydrate (sodium carbonate monohydrate). The different sodium carbonate hydrates are formed by initiating their precipitation from a supersaturated aqueous solution at different temperatures. Sodium carbonate decahydrate is formed during precipitation at a temperature below 32°C whereas sodium carbonate heptahydrate is formed at a temperature between 32°C and 35.4°C and a solution temperature of above 35.4°C results in the precipitation of sodium carbonate monohydrate, i.e. thermonatrite. These temperatures are called phase transition temperatures. Water-free sodium carbonate can be obtained by drying the hydrate forms at approx. 98°C. It will, however, revert to thermonatrite and/or other hydrates at room temperature and normal humidity levels. Since the heptahydrate is formed within a narrow temperature zone of 32°C to 35.4°C, it is (like the non-hydrated form of sodium carbonate) relatively unstable in common climatic conditions and usually occurs as a transitional product during phase changes from the more stable thermonatrite to natrite or vice versa.

Hydration pressure

Natrite and thermonatrite are considered as damaging to masonry due to their frequent changes in crystal structure and varying water of crystallization content. This occurs as a result of the low hydration/phase transition temperatures of around 35°C illustrated above. The change from thermonatrite to natrite and resultant addition of 9 water molecules into the crystal lattice involves a volume increase of around 260%. The transition from thermonatrite to sodium carbonate heptahydrate (at a temperature of 0-20°C and an RH of approx. 80%) results in a build up of hydration pressure in the region of 28.4 –63.7 N/mm² [Stark.etal:1996]Title: Bauschädliche Salze
Author: Stark, Jochen; Stürmer, Sylvia
.

Analytical validation

Initial identification of thermonatrite and natrite can be carried out in situ with the aid of simple solubility tests and pH-measurements: According to Bläuer-Böhm, natrite is the only currently known efflorescent salt to have an alkaline pH-value well above 8 but which also displays the ability to deliquesce in its own water of crystallization when heated slightly. Similarly, thermonatrite found in situ also has an alkaline pH-value and is soluble in water. However, thermonatrite is not soluble in water-free ethanol.

Microscopy

Laboratory analysis:

The solubility in water and insolubility in ethanol can be confirmed through microscopic examination. Thermonatrite and natrite
have the clear tendency to form needle and/or dendritic crystal shapes during re-crystallization. If gypsum is present in the sample material, a rapid precipitation of calcium carbonate will occur which is visible as a whitish deposit.

Refractive index:  n_x = 1.420;  n_y = 1.509; n_z = 1.25;
Birefringence:    Δ  = max. 0.105
Crystal systeme:          orthorhombic

Under the polarizing microscope:

The water of crystallization content of sampled crystals changes in relation to the ambient relative humidity and temperature levels the sample is exposed to. Subsequently, after only a short while in dry air (with approx. 60% RH) thermonatrite would predominantly be found.
The determination of the refractive index is carried out according to the immersion method. Individual particles soaked in standard immersion oil with a refractive index of n_D = 1.518 display a strong change in relief during rotation under transmitted polarized light [Blaeuer-Boehm:1994]Title: Salzuntersuchungen an Baudenkmälern
Author: Bläuer-Böhm, Christine
, a.a.O., p. 86. Due to the high birefringence, thermonatrite crystals display bright interference colors. This clearly differentiates it from natrite which has a noticeably smaller maximal birefringence.
Thermonatrite belongs to the orthorhombic crystal system. Associated with this is the parallel and/or symmetric extinction when viewed under crossed polars. Larger crystal needles generally appear completely extinguished and the extinction occurs suddenly.

Differentiation of thermonatrite from similar salts:

Thermonatrite is clearly identifiable when the following criteria are known:

• high pH-value
• good solubility in water
  
• characteristic crystal habit
• all refractive indices under n_D=1.53
• high birefringence
• parallel/symmetric extinction
  

Table 3: Salt phases with partially identical properties

Salt phase	Differing characteristic in comparison with Thermonatrite
Nesquehonite MgCO3 •  3H2O;	poor water solubility / oblique extinction
Lansfordite MgCO3 • 5H2O	poor water solubility / oblique extinction / low birefringence
Trona Na3H(CO3)2 • 2H2O	usually a noticeable refractive index > 1.53 / oblique extinction
Potash K2CO3	usually a noticeable refractive index > 1.53 / oblique extinction / strongly hygroscopic

Raman-Spectroscopy

Natrite images

Under the polarizing microscope

• Na2CO3 from an aqueous solution on a microscope slide
• 

  under plane-polarized light

• 

  under crossed polars

• 

  under crossed polars and Red I

• Na2CO3 from an aqueous solution on a microscope slide
• 

  under crossed polars

• 

  under plane-polarized light

Through the Scanning Electron Microscope

• Image through SEM
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Literature

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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

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

relative humidity

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

Scanning Electron Microscope