Question:
When slaked lime is passed through excess \( \mathrm{CO_2} \), it forms
When slaked lime is passed through excess \( \mathrm{CO_2} \), it forms
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Excess \( \mathrm{CO_2} \) converts insoluble carbonates into soluble bicarbonates.
Updated On: Feb 11, 2026
- \( \mathrm{CaCO_3} \)
- \( \mathrm{CaCl_2} \)
- \( \mathrm{Ca(HCO_3)_2} \)
- \( \mathrm{Ca_2HCO_3} \)
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The Correct Option is C
Solution and Explanation
Step 1: Reaction of slaked lime with carbon dioxide.
Slaked lime is calcium hydroxide, \( \mathrm{Ca(OH)_2} \). With limited \( \mathrm{CO_2} \), it forms calcium carbonate.
Step 2: Effect of excess \( \mathrm{CO_2} \).
When excess carbon dioxide is passed, calcium carbonate further reacts to form soluble calcium bicarbonate.
Step 3: Chemical equation.
\[ \mathrm{Ca(OH)_2 + 2CO_2 \rightarrow Ca(HCO_3)_2} \]
Step 4: Conclusion.
Thus, calcium bicarbonate is formed when slaked lime is treated with excess \( \mathrm{CO_2} \).
Slaked lime is calcium hydroxide, \( \mathrm{Ca(OH)_2} \). With limited \( \mathrm{CO_2} \), it forms calcium carbonate.
Step 2: Effect of excess \( \mathrm{CO_2} \).
When excess carbon dioxide is passed, calcium carbonate further reacts to form soluble calcium bicarbonate.
Step 3: Chemical equation.
\[ \mathrm{Ca(OH)_2 + 2CO_2 \rightarrow Ca(HCO_3)_2} \]
Step 4: Conclusion.
Thus, calcium bicarbonate is formed when slaked lime is treated with excess \( \mathrm{CO_2} \).
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