A dilute sulfuric acid solution that is 3.39 m H2SO4 has a density of 1.18 g/mL. How many moles of H2SO4 are there in 375 mL of this solution?
3.39 is 3.39 Molality not molarity
Which is it? M = molar; m = molal.
its m = molal
To determine the number of moles of H2SO4 in the given solution, we need to use the formula:
moles = concentration (mol/L) * volume (L)
Starting with the given data:
- The solution is a dilute sulfuric acid solution with a concentration of 3.39 m (molality).
- The density of the solution is 1.18 g/mL.
- We want to find the number of moles in 375 mL of the solution.
First, we need to convert the volume of the solution from milliliters (mL) to liters (L), as the concentration is given in molality, which is the number of moles per kilogram of solvent.
Converting 375 mL to liters:
375 mL * (1 L / 1000 mL) = 0.375 L
Now that we have the volume in liters, we can calculate the number of moles of H2SO4:
moles = 3.39 m * 0.375 L
Note: Molality (m) is defined as moles of solute per kilogram of solvent. However, in this case, we are given the molality directly without the solvent mass. This implies that 3.39 mol of H2SO4 is dissolved in 1 kg of solvent.
Since we are dealing with a dilute solution, the difference in mass between 1 kg of the solvent and 375 mL of the solution is negligible, and we can assume that the mass of the solution is equal to the mass of the solvent.
Therefore, we can convert the mass of the solvent from 1 kg to grams, using the density of the solution:
mass = density * volume
mass = 1.18 g/mL * 375 mL
Now we can calculate the number of moles of H2SO4:
moles = 3.39 m * (mass / 1000 g)
Substituting the calculated mass, we find:
moles = 3.39 m * (1.18 g/mL * 375 mL / 1000 g)
Calculating this expression will give us the number of moles of H2SO4 in the given solution.