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Diss Factsheets

Environmental fate & pathways

Endpoint summary

Administrative data

Description of key information

Additional information

Boron is almost exclusively found in the environment in the form of boron-oxygen compounds, which are often referred to as borates. The high strength of the B-O bond relative to those between boron and other elements makes boron oxide compounds stable compared to nearly all non-oxide boron materials. Indeed, the B-O bond is among the strongest found in the chemistry of naturally occurring inorganic substances. A trivial exception occurs with some rare boron fluoride minerals, as the B-F bond is even stronger.

As a result of the high relative stability of boron oxides compared to other boron compounds they are the thermodynamicallyfavoureddecomposition products. This is an inescapable outcome of the laws of thermodynamics. Although virtually all boron compounds ultimately decompose under environmental conditions to the thermodynamically most stable state represented by boric acid, many boron compounds exhibit high kinetic stability and decompose extremely slowly under environmental conditions - in some cases so slowly that they can be regarded chemically inert for practical purposes.

In aqueous solution, the equilibrium distribution of B(OH)3and B(OH)4- is known to be strongly pH dependent, such that at values higher than 8.6 borate ion dominates while at lower pH boric acid is the dominant species (Hershey JP et al., 1986).

In seawater (pH=8.2) borate ion comprises +/- 28.5% of boron species (assuming the dissociation constant of boric acid pKB=8.597 (at 25 °C)), representing ca. 6% of seawater alkalinity (Dickson AG, 1990).

Boron is an essential plant micronutrient with an average total concentration of 10 mg/kg in the earth’s crust (Adriano, 2001). Dissolution of boron-bearing minerals (e. g. tourmaline, muscovite), irrigation waters, fertilizers, atmospheric deposition of emitted boron (e. g. coal fly ash) as well as the soil’s buffering capacity, affect the boron concentration in soil. The natural level of boron in soils largely depends upon the soil parent material. In general, soils derived from igneous rocks and those of tropical and semitropical regions of the world are considerably lower in boron content compared with soils derived from sedimentary rocks and those of arid and semiarid regions. The content of total boron in the latter group may range up to 200 mg/kg, particularly in alkaline, calcareous soils, while that for the former group is usually lower than 10 mg/kg (Swaine, 1955, cited in Adriano, 2001).

The oceans are the largest global reservoir for boron with a global average concentration of about 4.6 mg B/L (Argust, 1998, Park and Schlesinger, 2002). However, boron may range in concentration from 0.52 mg B/L in the Baltic Sea to 9.6 mg B/L in the Mediterranean Sea (Argust, 1998).

Natural events such as generation of sea salt aerosols over the ocean, biomass burning, rock weathering and volcanic activity are estimated to release 2 x 10^9 kg B/year (Park and Schlesinger, 2002) Formation of sea salt aerosols and their transfer to land represents the largest flux of boron from the sea to the terrestrial environment, estimated as 1.44 x 10^9 kg B/yr by Park and Schlesinger (2002). They estimate riverine transfer to the oceans to be about 0.58 Tg B/yr.

Most anthropogenic releases of boron to the environment are from global coal combustion, estimated as 2 x 10^8 kg B/yr (Park and Schlesinger, 2002). Boron produced from mining is estimated to be about 3.1 x 10^8 kg B/yr (Argust, 1998) with about half the processed boron being used in products that are unlikely to release boron to the environment (glass, fiberglass and ceramics) (Park and Schlesinger, 2002).

Most anthropogenic boron (excluding coal-related materials) in Europe originates from mines in Turkey and California. Ratios of the boron isotopes 11B and 10B provide a tool to distinguish locally-derived boron from anthropogenic boron, although this has not been widely done (Vengosh et al., 1994; Chatelet and Gaillardet, 2005). 11B separates preferentially into dissolved boron (i. e. boric acid), whereas 10B is preferentially incorporated into the solid phase (Vengosh et al., 1994). The boron-11 isotope enrichment value (identified asδ 11B) ranges from about 39‰ in seawater, to about 0 ‰ in average continental crust, to -0.9 to +10.2‰ in sodium borate minerals from Turkey and California (Vengosh et al., 1994). The ratio has been used to identify anthropogenic boron fractions in surface waters (Chatelet and Gaillardet, 2005) and groundwaters (Vengosh et al., 1994; Kloppmann et al, 2005).


Justification for grouping of different borate compounds

In aqueous solutions at environmentally relevant concentrations and pH ranges, low concentrations of simple borates such as boric acid B(OH)3, potassium pentaborate (K2B10O16.8H2O), potassium tetraborate (K2B4O7.4H2O), disodium tetraborate decahydrate (Na2B4O7.10H2O; borax), disodium tetraborate pentahydrate (Na2B4O7.5H2O; borax pentahydrate), boric oxide (B2O3) and disodium octaborate tetrahydrate (Na2B8O13.4H2O) will predominantly exist as undissociated boric acid. Above pH 9 the metaborate anion B(OH)4- becomes the main species in solution (WHO, 1998). The toxicokinetics and toxicological effects of boric acid, potassium tetraborate, potassium pentaborate, disodium tetraborate decahydrate, boric oxide and disodium octaborate tetrahydrate are likely to be similar on a boron equivalents basis. Therefore, the data obtained from studies with the borates can be read across in the health and environmental assessments for each individual substance.

For comparative purposes, exposures to borates are often expressed in terms of boron (B) equivalents based on the fraction of boron in the source substance on a molecular weight basis. As noted previously, only boric acid and the borate anion are present at environmentally and physiologically relevant concentrations. Read- across between the different boron compounds can be done on the basis of boron (B) equivalents. (See section on dissociation constants). Conversion factors are given in the table below.

Conversion factors to boron equivalents



 Conversion factor for equivalent dose of B (multiply by)

 Boric acid



 Boric oxide



 Disodium tetraborate anhydrous



 Disodium tetraborate pentahydrate



 Disodium tetraborate decahydrate



 Disodium octaborate tetrahydrate



 Sodium metaborate (anhydrous)



 Sodium metaborate (dihydrate)



 Sodium metaborate (tetrahydrate)



 Sodium pentaborate (anhydrous)



 Sodium pentaborate (pentahydrate)



 Dipotassium tetraborate (anhydrous)



 Dipotassium tetraborate (tetrahydrate)



 Potassium pentaborate (anhydrous)



 Potassium pentaborate (tetrahydrate)