entage.

Given:

Density of the solution = $1.5 \, \text{g/mL}$

Weight percentage of nitric acid = 68%

Calculate the mass of the solution in 1L:

Since the density is given as $1.5 \, \text{g/mL}$, the mass of 1 liter (1000 mL) of the solution would be:

$ \text{Mass of solution} = 1.5 \, \text{g/mL} \times 1000 \, \text{mL} = 1500 \, \text{g} $

Determine the mass of nitric acid in the solution:

The weight percentage indicates that 68% of the solution's mass is nitric acid. Therefore, the mass of nitric acid is:

$ \text{Mass of } \text{HNO}_3 = \frac{68}{100} \times 1500 \, \text{g} = 1020 \, \text{g} $

Calculate the molar mass of nitric acid ($\text{HNO}_3$):

Using the atomic masses provided:

$ \text{Molar mass of } \text{HNO}_3 = 1 \, (\text{H}) + 14 \, (\text{N}) + 16 \times 3 \, (\text{O}) = 63 \, \text{g/mol} $

Find the concentration in mol/L:

To find the number of moles of $\text{HNO}_3$ in 1L:

$ \text{Number of moles} = \frac{\text{Mass of } \text{HNO}_3}{\text{Molar mass } \text{HNO}_3} = \frac{1020 \, \text{g}}{63 \, \text{g/mol}} = 16.20 \, \text{mol/L} $

Therefore, the concentration of nitric acid is approximately $16.20 \, \text{mol/L}$.

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