A concentrated nitric acid (HNO3) solution has a density of 1.310 g/mL. If pure water has a density of 0.9982 g/mL, what is the molar concentration of this solution of HNO3?

Try starting by assuming you have 100 mL of the acid solution. 

To find the molar concentration of the nitric acid (HNO₃) solution, we can start by calculating the mass of the solution and then the mass of HNO₃ in that solution. Here's a step-by-step approach:

1. **Assume a Volume of Solution**: Let's assume we have 100 mL of the HNO₃ solution.

2. **Calculate the Mass of the Solution**:
   \[
   \text{Density} = 1.310 \, \text{g/mL}
   \]
   \[
   \text{Mass of solution} = \text{Density} \times \text{Volume} = 1.310 \, \text{g/mL} \times 100 \, \text{mL} = 131.0 \, \text{g}
   \]

3. **Determine the Mass of HNO₃ in the Solution**:
   Concentrated nitric acid is typically around 68% HNO₃ by mass. Therefore:
   \[
   \text{Mass of HNO₃} = 0.68 \times \text{Mass of solution} = 0.68 \times 131.0 \, \text{g} = 89.08 \, \text{g}
   \]

4. **Calculate the Moles of HNO₃**:
   The molar mass of HNO₃ is approximately 63.01 g/mol.
   \[
   \text{Moles of HNO₃} = \frac{\text{Mass of HNO₃}}{\text{Molar mass of HNO₃}} = \frac{89.08 \, \text{g}}{63.01 \, \text{g/mol}} \approx 1.415 \, \text{mol}
   \]

5. **Calculate the Molar Concentration**:
   Molar concentration (C) is defined as the number of moles of solute per liter of solution.
   \[
   C = \frac{\text{Moles of HNO₃}}{\text{Volume of solution in L}} = \frac{1.415 \, \text{mol}}{0.1 \, \text{L}} = 14.15 \, \text{mol/L}
   \]

Thus, the molar concentration of the HNO₃ solution is approximately **14.15 mol/L**.

Would you like to explore more details or have any questions? Here are some related topics you might find interesting:

1. What are the safety precautions when handling concentrated nitric acid?
2. How does the molarity of a solution affect its reactivity?
3. What are the implications of using concentrated acids in laboratory experiments?
4. How do you prepare a diluted solution from a concentrated one?
5. What is the role of nitric acid in chemical reactions and industrial applications?

**Tip**: Always handle concentrated acids in a well-ventilated area and use appropriate personal protective equipment (PPE).

A concentrated nitric acid (HNO3) solution has a density of 1.310 g/mL. If pure water has a density of 0.9982 g/mL, what is the molar concentration of this solution of HNO3?

Discover how to calculate the molar concentration of a concentrated nitric acid (HNO3) solution with a density of 1.310 g/mL. This step-by-step guide covers key concepts like density, mass, and molarity, leading to a final concentration of approximately 14.15 mol/L.

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