An aqueous solution of nitric acid has a density of 1.084 g mL-1 and a measured concentration of 2.580 molar. What is the percent weight of nitric acid in the solution.

How much does a liter of solution weigh? It has a mass of 1.084 g/mL x 1000 mL = 1084 grams.

There are 2.580 moles HNO3 in the 1084 g of solution; therefore, 2.580 x molar mass HNO3 = about 162 g HNO3. (You need to do it exactly).
% HNO3 = (g HNO3/mass solution)*100 =
about (162/1084)*100 = ??
Check my work.

To find the percent weight of nitric acid in the solution, we need to calculate the weight of nitric acid in a given volume of the solution and then express it as a percentage of the total weight of the solution.

First, let's calculate the weight of nitric acid in 1 liter of the solution using the molarity and density information provided.

1. Determine the molar mass of nitric acid (HNO3):
- Hydrogen (H) atomic weight = 1.008 g/mol
- Nitrogen (N) atomic weight = 14.007 g/mol
- Oxygen (O) atomic weight = 16.00 g/mol
Molar mass of HNO3 = (1 × 1.008) + (1 × 14.007) + (3 × 16.00) = 63.015 g/mol

2. Calculate the weight of nitric acid in 1 liter of the solution:
- Concentration of the solution = 2.580 M
- Volume = 1 liter
- Moles of nitric acid = concentration × volume = 2.580 mol/L × 1 L = 2.580 mol
- Weight of nitric acid = moles × molar mass = 2.580 mol × 63.015 g/mol = 161.9427 g

Now, let's calculate the percentage weight of nitric acid in the solution.

3. Calculate the total weight of the solution:
- Density of the solution = 1.084 g/mL
- Volume of the solution = 1 liter
- Weight of the solution = density × volume = 1.084 g/mL × 1 L = 1.084 kg = 1084 g

4. Calculate the percent weight of nitric acid:
- Percent weight of nitric acid = (Weight of nitric acid / Weight of the solution) × 100
- Percent weight of nitric acid = (161.9427 g / 1084 g) × 100
- Percent weight of nitric acid = 14.95%

Therefore, the percent weight of nitric acid in the solution is approximately 14.95%.

To calculate the percent weight of nitric acid in the solution, we need to determine the mass of nitric acid present and divide it by the total mass of the solution.

First, let's calculate the mass of nitric acid in the solution:

Given:
Density of the solution = 1.084 g mL^(-1)
Concentration of the nitric acid = 2.580 M (molar)

The concentration of a solution is defined as the number of moles of solute per liter of solution. So, to find the number of moles of nitric acid, we can use the formula:

moles of nitric acid = concentration (M) × volume (L)

Since we don't have the volume of the solution, we cannot calculate the exact amount of moles present. However, we can proceed by assuming that we have 1 liter (1000 mL) of the solution.
Thus, we can calculate the number of moles:

moles of nitric acid = 2.580 mol/L × 1 L = 2.580 mol

The molar mass of nitric acid (HNO3) can be found by adding up the atomic masses of its constituent elements:

H: 1.01 g/mol × 1 = 1.01 g/mol
N: 14.01 g/mol × 1 = 14.01 g/mol
O: 16.00 g/mol × 3 = 48.00 g/mol

Total molar mass of HNO3 = 1.01 g/mol + 14.01 g/mol + 48.00 g/mol = 63.02 g/mol

Now, let's calculate the mass of nitric acid in the solution:

mass of nitric acid = moles × molar mass
mass of nitric acid = 2.580 mol × 63.02 g/mol = 162.52 g

Next, we need to find the mass of the entire solution. Since we know the density of the solution, we can calculate the mass using the formula:

mass of solution = density × volume

Again, assuming we have 1 liter (1000 mL) of the solution, we can substitute the given values:

mass of solution = 1.084 g/mL × 1000 mL = 1084 g

Finally, we can calculate the percent weight of nitric acid in the solution:

percent weight of nitric acid = (mass of nitric acid / mass of solution) × 100

Substituting the values we obtained:

percent weight of nitric acid = (162.52 g / 1084 g) × 100 ≈ 15.00%

Therefore, the percent weight of nitric acid in the solution is approximately 15.00%.