Final answer:
The molarity of a 14.5% H2SO4 solution with a density of 1.131 g/mL can be calculated by converting the percentage by mass to grams of H2SO4 per milliliter, finding the moles of H2SO4, and dividing by the volume of the solution in liters. The calculation yields a molarity of 1.478 M.
Step-by-step explanation:
To find the molarity of a 14.5% aqueous solution of sulfuric acid (H2SO4) with a density of 1.131 g/mL, follow these steps:
- Convert the percentage by mass to grams of H2SO4 per milliliter of solution. Since the density is 1.131 g/mL, a 100 mL solution would have a mass of 113.1 grams, and 14.5% of that would be H2SO4.
- Calculate the mass of H2SO4 in grams for a given volume of solution, such as 1 liter (1000 mL).
- Convert this mass to moles of H2SO4 using its molar mass.
- Divide the number of moles by the volume of solution in liters to get the molarity.
Molarity is calculated using the formula M = moles of solute / volume of solution in liters.
For example, if you have 14.5 grams of H2SO4 in 100 grams of solution, and the density is 1.131 g/mL, the molarity would be:
M = (0.145 g/mL × 1000 mL) / (98.079 g/mol) / 1 L
First, calculate the mass of H2SO4 per liter: 0.145 g/mL × 1000 mL = 145 g of H2SO4.
Next, convert the mass of H2SO4 to moles: 145 g / 98.079 g/mol = 1.478 moles of H2SO4.
Finally, divide the moles by the volume in liters (which is 1 in this case) to find the molarity.
M = 1.478 moles / 1 L = 1.478 M