The Solvay process or ammonia-soda
process is the major industrial process for the production of soda
ash (valued primarily for its
content of sodium carbonate). The
ammonia-soda process was developed into its modern form by Ernest
Solvay during the 1860s.
The ingredients for this process are readily available and
inexpensive: salt brine (from inland sources or from the sea) and
limestone (from mines). The worldwide production of soda ash in 2005
has been estimated at 42 billion kilograms, which is more than six
kilograms per year for each person on Earth. Solvay-based chemical
plants now produce roughly three-quarters of this supply, with the
remainder being mined from natural deposits.
Chemistry.
The Solvay Process as an example of a cyclic process in chemical
industry (green = reactants, black = intermediates, red =
products)
The Solvay process results in soda ash (predominantly sodium
carbonate (Na2CO3)) from brine (as a source of sodium chloride
(NaCl)) and from limestone (as a source of calcium carbonate
(CaCO3)).
The overall process is:
The actual implementation of this global, overall reaction is intricate.A simplified description can be given using the four different, interacting chemical reactions illustrated in the figure. In the first step in the process, carbon dioxide (CO2) passes through a concentrated aqueous solution of sodium chloride (table salt, NaCl) and ammonia (NH3).
In industrial practice, the reaction is carried out by passing
concentrated brine through two towers. In the first, ammonia bubbles
up through the brine (salt water) and is absorbed by it. In the
second, carbon dioxide bubbles up through the ammoniated brine, and
sodium bicarbonate (baking soda) precipitates out of the solution.
Note that, in a basic solution, NaHCO3 is less water-soluble than
sodium chloride. The ammonia (NH3) buffers the solution at a basic
pH; without the ammonia, a hydrochloric acid byproduct would render
the solution acidic, and arrest the precipitation.
The necessary ammonia "catalyst" for reaction (I) is reclaimed in a
later step, and relatively little ammonia is consumed. The carbon
dioxide required for reaction (I) is produced by heating
("calcination") of the limestone at 950 - 1100 °C. The calcium
carbonate (CaCO3) in the limestone is partially converted to
quicklime (calcium oxide (CaO)) and carbon dioxide:
The sodium bicarbonate (NaHCO3) that precipitates out in reaction (I) is filtered out from the hot ammonium chloride (NH4Cl) solution, and the solution is then reacted with the quicklime (calcium oxide (CaO)) left over from heating the limestone in step (II).
CaO makes a strong basic solution. The ammonia from reaction (III)
is recycled back to the initial brine solution of reaction (I).
The sodium bicarbonate (NaHCO3) precipitate from reaction (I) is then
converted to the final product, sodium carbonate (washing soda:
Na2CO3), by calcination (160 - 230 C), producing water and carbon
dioxide as byproducts:
The carbon dioxide from step (IV) is recovered for re-use in step
(I). When properly designed and operated, a Solvay plant can reclaim
almost all its ammonia, and consumes only small amounts of additional
ammonia to make up for losses. The only major inputs to the Solvay
process are salt, limestone and thermal energy, and its only major
byproduct is calcium chloride, which is sold as road salt.
In the modified Solvay process developed by Chinese chemist Hou
Debang in 1930s, the first few steps are the same as the Solvay
process. However, the CaCl2 is supplanted by ammonium chloride
(NH4Cl). Instead of treating the remaining solution with lime, carbon
dioxide and ammonia are pumped into the solution, then sodium
chloride is added until the solution saturates at 40°C. Next,
the solution is cooled to 10°C. Ammonium chloride precipitates
and is removed by filtration, and the solution is recycled to produce
more sodium carbonate. Hou's process eliminates the production of
calcium chloride. The byproduct ammonium chloride can be refined,
used as a fertilizer and may have greater commercial value than
CaCl2, thus reducing the extent of waste beds.
Additional details of the industrial implementation of this process
are available in the report prepared for the European Soda Ash
Producer's Association.
Note:
- The Solvay process is less polluting and less expensive than the Leblanc process; chemical process which allows to obtain the sodium carbonate from sea salt. It is because it rejects polluting hydrochloric acid (HCl in the first step) and calcium sulfide, CaS (last step).
- Salt and chalk are plentiful and inexpensive, and the ammonia is recycled during the reaction.