Question

Solvay process is used for the manufacture of :
(A) NaOH
(B) $N{a_2}C{O_3}.10{H_2}O$
(C) ${K_2}C{O_3}$
(D) $N{a_2}{O_2}$

Answer 1

The Solvay process, often known as the ammonia-soda process, is the most used commercial method for producing sodium carbonate. During the 1860s, Belgian scientist Ernest Solvay improved the ammonia-soda process into its present form. The components for this are salt brine (from inland sources or the sea) and limestone, which are both widely available and affordable (from quarries). In 2005, the global output of soda ash was predicted to reach 42 million tonnes, or more than six kilogrammes (13 lb) per person per year.

Complete Step By Step Answer:
Soda ash is produced via the Solvay process, which uses brine as a source of sodium chloride and limestone as a source of calcium carbonate. The entire procedure is $2{\text{ }}NaCl{\text{ }} + {\text{ }}CaC{O_3}\; \to {\text{ }}N{a_2}C{O_3}\; + {\text{ }}CaC{l_2}$
The reaction is carried out in industrial practise by feeding concentrated brine through two towers. Ammonia bubbles up through the brine in the first and is absorbed by it. Carbon dioxide rises up through the ammoniated brine in the second, precipitating sodium bicarbonate out of the solution. Ammonia bubbles up through the brine in the first and is absorbed by it. Carbon dioxide rises up through the ammoniated brine in the second, precipitating sodium bicarbonate (baking soda) from the solution. It's worth noting that $NaHC{O_3}$ is less water-soluble than sodium chloride in a basic solution. The ammonia buffers the solution, keeping it at a basic (high) pH; without it, a hydrochloric acid byproduct would make the solution acidic, halting precipitation. The "mother liquor" in this case is NH4 in combination with ammoniacal brine.
$NaCl + C{O_2} + N{H_3} + {H_2}O \to NaHC{O_3} + N{H_4}Cl$
In a later stage, the required ammonia "catalyst" for reaction is recovered, and just a small amount of ammonia is used.
Quicklime (calcium oxide (CaO)) and carbon dioxide are produced from the calcium carbonate in the limestone:
$CaC{O_3} \to C{O_2} + CaO$
The sodium bicarbonate that forms during the reaction is filtered out of the hot ammonium chloride solution, which is then reacted with the quicklime (calcium oxide) that was left over from the previous stage of heating the limestone.
$2N{H_4}Cl + CaO \to 2N{H_3} + CaC{l_2} + {H_2}O$
CaO is an excellent basic solution. The ammonia from the reaction is recycled back into the reaction's brine solution.
Calcination converts the sodium bicarbonate precipitate from the reaction to the end product, sodium carbonate (washing soda), yielding water and carbon dioxide as byproducts.
$2NaHC{O_3} \to N{a_2}C{O_3} + {H_2}O + C{O_2}$
Hence option B is correct.

Note:
Step (IV) produces carbon dioxide, which is collected and reused in step (I). A Solvay plant can recover virtually all of its ammonia when correctly built and managed, and only requires tiny quantities of extra ammonia to compensate for losses. Salt, limestone, and heat energy are the only main inputs to the Solvay process, while calcium chloride, which is occasionally sold as road salt, is the only major output.