Concentrated sulfuric acid (18.3 M) has a density of 1.84 g/mL.
How many moles of H2SO4 are in each milliliter of solution?
If it's 18.3 M that means 18.3 mols/L which is 0.0183 mols/mL
To determine the number of moles of H2SO4 in each milliliter of solution, we need to use the density and molarity of the sulfuric acid.
First, let's calculate the mass of 1 milliliter (1 mL) of the solution:
mass = density × volume = 1.84 g/mL × 1 mL = 1.84 g
Next, we can convert the mass of the solution to moles of sulfuric acid using its molar mass. The molar mass of H2SO4 is:
H: 1.008 g/mol × 2 = 2.016 g/mol
S: 32.06 g/mol
O: 16.00 g/mol × 4 = 64.00 g/mol
Summing these up, the molar mass of H2SO4 is:
2.016 g/mol + 32.06 g/mol + 64.00 g/mol = 98.076 g/mol
Now, let's convert the mass of the solution to moles using the molar mass:
moles = mass / molar mass = 1.84 g / 98.076 g/mol ≈ 0.01878 mol
Therefore, each milliliter of the solution contains approximately 0.01878 moles of H2SO4.