Calculate the molarity of a 6% solution of ammoniun nitrate of density 1.025 g/mL
To calculate the molarity of a solution, we need to know the formula of the solute (ammonium nitrate) and its molar mass.
The molar mass of ammonium nitrate (NH4NO3) can be calculated by summing the atomic masses of its constituent elements:
NH4NO3 = [(1 * N) + (4 * H) + (3 * O)]
NH4NO3 = [14.01 + (4 * 1.01) + (3 * 16.00)]
NH4NO3 = 80.04 g/mol
Now, let's calculate the molarity using the formula:
Molarity (M) = (mass of solute in grams) / (molar mass of solute in g/mol) / (volume of solution in L)
First, let's determine the mass of the ammonium nitrate in the solution:
mass of ammonium nitrate = (percent concentration / 100) * volume of solution * density
mass of ammonium nitrate = (6 / 100) * volume of solution * density
mass of ammonium nitrate = 0.06 * volume of solution * density
Now, let's calculate the volume of the solution:
volume of solution = mass of solution / density
volume of solution = mass of solution / density
volume of solution = mass of solution / 1.025 g/mL
Finally, we can substitute the values into the molarity formula:
Molarity (M) = (0.06 * volume of solution * density) / (80.04 g/mol) / (volume of solution / 1.025 g/mL)
Simplifying the formula:
Molarity (M) = (0.06 * 1.025) / 80.04
Molarity (M) ≈ 0.0007689 M
So, the molarity of a 6% solution of ammonium nitrate with a density of 1.025 g/mL is approximately 0.0007689 M.