A 4.0 g of mixture of `Na_(2)CO_(3)` and `NaHCO_(3)` loses 0.248 g when heated to `300^@C`, the temperature at which `NaHCO_(3)` decomposes to `Na_(2)CO_(3), CO_(2)` and `H_(2) O`. What is the percentage of `Na_(2) CO_(3)` in mixture?

Explanation

To solve the problem step by step, we will follow the reasoning provided in the video transcript and derive the percentage of \( \text{Na}_2\text{CO}_3 \) in the mixture of \( \text{Na}_2\text{CO}_3 \) and \( \text{NaHCO}_3 \).

### Step 1: Understand the decomposition reaction
When heated, sodium bicarbonate (\( \text{NaHCO}_3 \)) decomposes into sodium carbonate (\( \text{Na}_2\text{CO}_3 \)), carbon dioxide (\( \text{CO}_2 \)), and water (\( \text{H}_2\text{O} \)). The balanced equation for this reaction is:
\[ 2 \text{NaHCO}_3 \rightarrow \text{Na}_2\text{CO}_3 + \text{CO}_2 + \text{H}_2\text{O} \]

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