A chemist doesn\'t add a sufficient quantity of barium chloride to reaction with

Question

A chemist doesn't add a sufficient quantity of barium chloride to reaction with and precipitate the sulfate ions. As a result, would the experimental mass percentage of sulfate be overestimated, underestimated or remain unaffected? explain your reasoning. A chemist forgets to add hydrochloric acid to the metal sulfate hydrate solution before the precipitation. Consequently, a portion of carbonate ions in solution from dissolved carbon dioxide also reacts and precipitates with barium ions. As a result, would the experimental mass percentage of sulfate be overestimated, underestimated or remain unaffected? explain your reasoning.

Explanation / Answer

Q2.

IF ions in solution of SO4-2 aren't stoichiometrically mathed with those of Ba+2 ions

then

The total mass will not precipitate (i.e. solid will not be formed)

Since we filter only solids, this will have a lower mass than that of the total SO4-2 in solution

Q3.

HCl to a MSO4*H2O

CO3-2 ions in solution form CO2

This will incrase (incorrectly) the total mass, but this is not favoured, the real value will be much higher than that of the original mix

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