You have 500 mL of a 5.0 M solution of nitric acid HNO3 (63.01 g / mol) dissolved in water. How many grams of nitrogen does the solution contain?
What is the percent N in HNO3? That's
(14/63)*100 = about 22% or so.
mols HNO3 = M x L = 5.0*0.500L = 2.5 mols.
grams HNO3 = 2.5 mols x molar mass = about 160g.
Then about 160 x 0.22 = ?. Don't forget I estimated these numbers.
Well, that's easy! To find the number of grams of nitrogen in the solution, we need to first calculate the number of moles of nitric acid HNO3.
Since the concentration is 5.0 M and you have 500 mL of the solution, we can use the formula:
moles = concentration × volume
moles = 5.0 mol/L × 0.5 L
moles = 2.5 mol
Now, in one molecule of HNO3, we have one atom of nitrogen (N), so the number of moles of nitrogen is also 2.5.
Finally, to calculate the number of grams of nitrogen, we can multiply the number of moles by the molar mass of nitrogen.
grams = moles × molar mass
grams = 2.5 mol × 14.01 g/mol
grams = 35.025 g
So, the solution contains approximately 35.025 grams of nitrogen. My goodness, that's a lot of nitrogen! Sounds like this solution is just bursting with it!
To determine the number of grams of nitrogen in the solution, you first need to calculate the moles of nitric acid present.
Step 1: Find the moles of nitric acid (HNO3):
To calculate the moles, you can use the formula:
Moles = Molarity × Volume (L)
Given:
Molarity (M) = 5.0 M
Volume (L) = 500 mL = 0.5 L
Moles of nitric acid = 5.0 M × 0.5 L = 2.5 moles
Step 2: Calculate the moles of nitrogen (N):
In one molecule of nitric acid (HNO3), there is 1 atom of nitrogen (N). Therefore, the moles of nitrogen (N) will be the same as the moles of nitric acid (HNO3).
Moles of nitrogen (N) = 2.5 moles
Step 3: Calculate the grams of nitrogen (N):
To calculate the grams, you can use the formula:
Grams = Moles × Molar Mass
The molar mass of nitrogen (N) is 14.01 g/mol.
Grams of nitrogen (N) = 2.5 moles × 14.01 g/mol = 35.03 grams
Therefore, the 500 mL solution of 5.0 M nitric acid contains 35.03 grams of nitrogen (N).
To calculate the number of grams of nitrogen in the solution, we need to determine the number of moles of nitric acid first.
Given:
- Volume of the solution = 500 mL = 0.5 L
- Concentration of nitric acid = 5.0 M (moles per liter)
Using the formula for number of moles (n) = concentration (M) × volume (L), we can calculate the number of moles of nitric acid:
n = 5.0 M × 0.5 L
n = 2.5 moles
Next, we need to determine the molecular weight of nitric acid to calculate the number of grams of nitrogen. The molecular weight is the sum of the atomic weights of all the atoms in the molecule.
Nitric acid (HNO3) consists of one nitrogen (N) atom, one hydrogen (H) atom, and three oxygen (O) atoms.
Atomic weights:
- Nitrogen (N) = 14.01 g/mol
- Hydrogen (H) = 1.01 g/mol
- Oxygen (O) = 16.00 g/mol
Molecular weight of nitric acid = (1 × atomic weight of N) + (1 × atomic weight of H) + (3 × atomic weight of O) = (1 × 14.01) + (1 × 1.01) + (3 × 16.00) = 63.01 g/mol
Since 1 mole of nitric acid (HNO3) contains 1 mole of nitrogen (N), we can conclude that the solution contains 2.5 moles of nitrogen.
Finally, to determine the grams of nitrogen, we use the formula:
grams of nitrogen = moles of nitrogen × molecular weight of nitrogen
grams of nitrogen = 2.5 moles × 14.01 g/mol
grams of nitrogen = 35.025 grams (rounded to three decimal places)
Therefore, the 500 mL solution of 5.0 M nitric acid contains approximately 35.025 grams of nitrogen.