A 10.0 g sample of a mixture of calcium chloride and sodium chloride is treated with $\mathrm{Na_2CO_3}$ to precipitate the calcium as calcium carbo...

Question

A 10.0 g sample of a mixture of calcium chloride and sodium chloride is treated with $\mathrm{Na_2CO_3}$ to precipitate the calcium as calcium carbonate. This $\mathrm{CaCO_3}$ is heated to convert all the calcium to CaO and the final mass of CaO is 1.62 gms. The % by mass of $\mathrm{CaCl_2}$ in the original mixture is :

**Options:**
- **A.** [object Object]
- **B.** [object Object]
- **C.** [object Object]
- **D.** [object Object]

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**Difficulty:** HARD | **Chapter:** Mole concept | **Topic:** Basic stoichiometry, POAC, percent yield & limiting reagent

Accepted Answer

## ✅ Correct Answer: **B**

### 📖 Detailed Explanation:
This question uses stoichiometry and limiting reagent. Write the balanced chemical equation, compute moles of each reactant, identify the limiting reagent, and use stoichiometric ratios (and % yield, if needed) to obtain the answer; this gives option B.

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A 10.0 g sample of a mixture of calcium chloride and sodium chloride is treated with \(\mathrm{Na_2CO_3}\) to precipitate the calcium as calcium carbo...

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