Chapter 4: Problem 100
Sodium carbonate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right)\) is available in very pure form and can be used to standardize acid solutions. What is the molarity of an \(\mathrm{HCl}\) solution if \(28.3 \mathrm{~mL}\) of the solution is required to react with \(0.256 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3} ?\)
Short Answer
Step by step solution
Write the balanced chemical equation
Calculate moles of Na2CO3
Determine moles of HCl needed
Calculate molarity of the HCl solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Molarity Calculation
- Volume in liters = \( \frac{28.3 \text{ mL}}{1000} = 0.0283 \text{ L} \)
- \( M = \frac{0.004828 \text{ moles}}{0.0283 \text{ L}} \approx 0.1707 \text{ M} \)
Balanced Chemical Equation
- 1 mole \( \mathrm{Na}_2\mathrm{CO}_3 \) requires 2 moles \( \mathrm{HCl} \)
- This stems from the stoichiometry of reaction, maintaining equal balance on both sides in terms of atoms of each element.
Moles Calculation
- Given mass = 0.256 g
- Molar mass of \( \mathrm{Na}_2\mathrm{CO}_3 \) = 105.99 g/mol
- \( \text{moles of } \mathrm{Na}_2\mathrm{CO}_3 = \frac{0.256 \text{ g}}{105.99 \text{ g/mol}} \approx 0.002414 \text{ moles} \)
Sodium Carbonate Standardization
- \( \mathrm{Na}_2\mathrm{CO}_3 \) has a reliable and stable molar mass, making it ideal for precise calculations.
- The reaction with HCl is straightforward and produces easily detectable products.
- By knowing the exact amount of \( \mathrm{Na}_2\mathrm{CO}_3 \), you can calculate the precise molarity of the HCl solution, ensuring accurate titration results.