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).