In the removal of temporary hardness of a sam | vedclass

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(A) The chemical reaction for the removal of temporary hardness using lime water is: $Ca(HCO_3)_2 + Ca(OH)_2 \rightarrow 2CaCO_3 \downarrow + 2H_2O$ F

Vedclass · Accepted Answer

$1$

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(A) The chemical reaction for the removal of temporary hardness using lime water is: $Ca(HCO_3)_2 + Ca(OH)_2 \rightarrow 2CaCO_3 \downarrow + 2H_2O$ From the balanced chemical equation,$1 \ mole$ of $Ca(OH)_2$ reacts with $1 \ mole$ of $Ca(HCO_3)_2$ to precipitate calcium carbonate. Therefore,the number of moles of $Ca(OH)_2$ required is $1$.

In the removal of temporary hardness of a sample containing $Ca^{2+}$,what is the number of moles of $Ca(OH)_2$ used per mole of $Ca(HCO_3)_2$ removed?

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