Sources of Human and Environmental Exposure
31
Table 6. Distribution of all platinum group metals in the environment
a
Region
Estimated concentration of PGMs
Earth
~30 mg/kg
Mantle (siliceous lithosphere)
~0.05 mg/kg
Earth’s crust (attainable by mining)
~0.01 mg/kg
Hydrosphere
<10
–6
mg/litre
Biomass (dry matter)
<10
–7
mg/kg
a
Adapted from Renner & Schmuckler (1991).
Table 7. Palladium output, by country
a
Country
Palladium output (tonnes)
1981
1987
1990
1993
1995
1996
1997
1998
Soviet
Union/
Russia
b
44.5
55.7
58.2
71.5
40
37.9
149.4
180.5
South Africa
28.3
33.9
38.2
43.4
44
103.6
56.3
56.3
Canada and
USA
5.0
5.9
11.5
11.5
13
7.5
17.0
20.5
Others
2.2
2.8
2.2
2.2
2.0
3.4
3.0
3.7
Total
(tonnes)
80.0
98.3
110.1
128.6
99.0
152.4
225.7
261.0
a
1981–1993 from Kroschwitz (1996); 1995 from Loebenstein (1996); 1996
from MMAJ (1999); 1997–1998 from Cowley (1998, 1999).
b
Russian values for 1981–1996: sales to the West.
3.2.1.1
Production processes
Several enrichment steps follow the mining of ores, either under-
ground or by opencast (strip) mining (Renner & Tröbs, 1986; Renner,
1992; Kroschwitz, 1996). In the case of PGMs from South Africa, the
crude ore is first crushed and pulverized. The metal sulfide particles are
then separated from the gangue by froth flotation.
The PGM sulfide pulp is melted in an electric furnace to produce
matte containing principally copper, nickel and iron sulfides, together
with the PGMs. Nickel and copper are separated by acid leaching to
yield the final PGM concentrate. The concentrate is then refined, using
either a selective dissolution and precipitation technique or a solvent
extraction process, whereby ammonium-chloro-complexes (e.g.,
EHC 226: Palladium
32
chloropalladosamine) are formed. Thermal decomposition (calcination)
of chloropalladosamine gives the impure palladium sponge.
3.2.1.2
Recycling
Processing of recycled material, including both new and old scrap,
resulted in the recovery of an estimated 60 tonnes of PGMs during
1995 in the USA (Loebenstein, 1996).
Scrapped automobile catalysts contributed 5.4 tonnes to the world
palladium demand of 72 tonnes in the automotive sector in 1998
(Cowley, 1999). According to Cowley (1999), 5.12 tonnes of palladium
were recovered from old automobile catalysts in North America and
Japan in 1998. The ultimate fate of many automobile catalysts may be
disposal in waste dumps. Recycling methods comprise pyrometallurgi-
cal refining techniques that are similar to those described previously
in section 3.2.1.1 (e.g., Degussa, 1997). The quantities recovered from
s crapped electrical components (electrical contacts) are larger, but
again no figures exist (Cowley, 1997). It is expected that some of the
utilized palladium ends up in wastes or incineration ashes. It can also
be expected that dental alloys are completely recycled if dental
prostheses have to be replaced.
Recycling rates for electronic equipment and automobile catalysts
depend on both economic and political decisions in the different
countries.
3.2.2
Processes for the production of important palladium
compounds
Many palladium compounds are in use as catalysts, as precursors
of metallic palladium, in preparative chemical production, in photog-
raphy, in electroplating and in medicine. The production processes of
some important compounds are described below:
<
Ammine complexes of pallad i u m: Addition of ammonia to
solutions of palladium(II) chloride first causes the formation of a
pink precipitate of the binuclear complex Pd(NH
3
)
4
PdCl
4
,
Vauquelin’s salt, which is converted to soluble tetraammine palla-
dium(II) chloride by further addition of ammonia. Acidification of
this solution yields the sparingly soluble light-yellow trans-
Sources of Human and Environmental Exposure
33
diamminedichloropalladium(II). Ammonium hexachloropalladate(IV) is
an oxidation product of ammonium tetrachloropalladate(II).
<
Palladium(II) ace tate: This compound is prepared from palladium
sponge (or nitrate) and glacial acetic acid.
<
Palladium(II) chloride: Palladium(II) chloride is prepared by the
careful evaporation of a solution of hydrogen tetrachloropalla-
date(II) in hydrochloric acid, preferably in a rotary evaporator.
<
Palladium(II) nitrate: This compound is prepared from palladium
and nitric acid (Renner, 1992).
<
Palladium(II) oxide: Palladium(II) oxide is obtained by reaction
of palladium black (powder) with oxygen or air at 750 °C.
Decomposition occurs at 850 °C. A catalytically active palladium
preparation analogous to platinum(IV) oxide (PtO
2
[H
2
O]
x
) can be
obtained by evaporating a solution of hydrogen tetrachloropalla-
date(II) and sodium nitrate and fusing the product (Cotton &
Wilkinson, 1982; Neumüller, 1985).
<
Tetrachloropalladic(II) acid: The metal is dissolved in hydro-
chloric acid/chlorine or hydrochloric acid/nitric acid. If dissolution
occurs below about 50 °C, hexachloropalladic(IV) acid is formed
first. Commercial solutions in hydrochloric acid contain 20%
palladium (Renner, 1992).
3.2.3
Uses of palladium metal
From Table 8, it can be seen that demand for palladium, in
particular for use in automobile catalysts, is increasing.
3.2.3.1
Electronics and electrical technology
Palladium metal or silver–palladium powder pastes are important
products in the production of many electronic components. T h e
metallization process is often carried out with silver–palladium thick
film paste. The pastes are used in active components such as diodes,
transistors, integrated circuits, hybrid circuits and semiconductor
memories. They are also needed for passive electronic components,
10>10>
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