Question

i) Write the chemical reactions for the laboratory preparation of hydrogen chloride gas
with conditions if any:
(ii) Why can calcium oxide not be used as a drying agent in the laboratory preparation of hydrogen chloride gas?
(iii) Hydrogen chloride gas is not collected over water. Why?

Answer 1

Answer:

Explanation:

iii) Hydrogen chloride is not collected over water as it is highly soluble in water.

ii) Calcium oxide would be preferred over sulfuric acid when trying to dry basic compounds (ammonia or amines, for example), since those would react with the acid. It’s also probably a better choice for alcohols or many other organic molecules that would be attacked by H2SO4.

For many other cases, sulfuric acid would be preferred, either because whatever you’re trying to dry is an acid (which would react with CaO) or just because it’s conveniently liquid.

In terms of strength both these desiccants are similar. If used to dry air they leave a residual moisture of a few micrograms per liter - better than some other candidates like magnesium sulfate or calcium chloride, but not quite as aggressive as phosphorus pentoxide or elemental sodium.

In terms of actual lab practice these days, however, almost everyone prefers molecular sieves.

Sulphuric acid is a strong oxidizing agent as well, apart from being a dehydrating agent. Where as CaO is not as such. It dehyrates without giving any artifects

CaO+H2O----> Ca(OH)2

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