Question

What is the molarity of a nitric acid solution that has a density of 1.19 g/mL and is 32 wt % HNO3 (FW = 63)

Answer 1

To find the molarity of a 32 wt% nitric acid solution with a density of 1.19 g/mL, calculate the mass of HNO3 per milliliter, convert the mass to moles, and then divide by the volume in liters, resulting in a molarity of 6.048 M.

Step-by-step explanation:

The molarity of a nitric acid solution can be determined by using the weight percentage of HNO3 and the density of the solution. First, calculate the mass of HNO3 per milliliter of solution by multiplying the density by the weight percentage of HNO3. Next, convert this mass to moles using the molar mass of HNO3 (FW = 63 g/mol). Finally, since molarity (M) is defined as moles of solute per liter of solution, you can find molarity by dividing the moles of HNO3 by the volume of the solution in liters.

For example, if we have a solution with a density of 1.19 g/mL and a 32 wt% concentration of HNO3, we would calculate the molarity as follows:

1. Find the mass of HNO3 in one milliliter of solution: 1.19 g/mL × 0.32 = 0.3808 g/mL.
2. Convert this mass to moles of HNO3: 0.3808 g/mL ÷ 63 g/mol = 0.006048 moles/mL.
3. Since molarity is moles per liter, convert the volume from mL to L and find the molarity: 0.006048 moles/mL × 1000 mL/L = 6.048 M.