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(B) The reaction of quick lime $(CaO)$ with water is exothermic and produces slaked lime $(Ca(OH)_{2})$,which is '$A$'.$CaO + H_{2}O \rightarrow Ca(OH

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Slaked lime

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(B) The reaction of quick lime $(CaO)$ with water is exothermic and produces slaked lime $(Ca(OH)_{2})$,which is '$A$'.$CaO + H_{2}O \rightarrow Ca(OH)_{2}$When $CO_{2}$ is passed through an aqueous solution of '$A$' $(Ca(OH)_{2})$,it forms a white precipitate of calcium carbonate $(CaCO_{3})$,which is '$B$'.$Ca(OH)_{2} + CO_{2} \rightarrow CaCO_{3} + H_{2}O$Further reaction of $CaCO_{3}$ with $CO_{2}$ and water leads to the formation of soluble calcium bicarbonate $(Ca(HCO_{3})_{2})$.$CaCO_{3} + H_{2}O + CO_{2} \rightarrow Ca(HCO_{3})_{2}$Therefore,'$A$' is slaked lime.

Lime reacts exothermally with water to give '$A$' which has low solubility in water. Aqueous solution of '$A$' is often used for the test of $CO_{2}$,a test in which insoluble $B$ is formed. If $B$ is further reacted with $CO_{2}$ then a soluble compound is formed. '$A$' is

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