What volume of ethanol must be diluted with
water to prepare 315 mL of 0.620 M solution?
The density of ethanol is given as 0.789 g/mL.
Answer in units of mL
You want 315 mL of 0.620M = 0.315*0.620 = mols ethanol needed. mol = g/molar mass to give you grams, then use the density to calculate volume (mL) ethanol. Then to make this solution, you must add H2O to make a total volume of 315 mL.
To find the volume of ethanol that needs to be diluted with water, we first need to determine the amount of ethanol required in moles.
Given:
- desired volume of the solution (V) = 315 mL
- desired concentration of ethanol (C) = 0.620 M
The formula to calculate the moles of ethanol is:
moles = concentration x volume
moles of ethanol = 0.620 mol/L x 0.315 L
Now, we need to find the mass of ethanol required:
mass = volume x density
mass of ethanol = 315 mL x 0.789 g/mL
Using the molar mass of ethanol (46.07 g/mol), we can calculate the moles of ethanol:
moles = mass / molar mass
moles of ethanol = (315 mL x 0.789 g/mL) / 46.07 g/mol
Now, we can find the volume of ethanol that needs to be diluted:
volume = moles / concentration
volume of ethanol = (315 mL x 0.789 g/mL / 46.07 g/mol) / 0.620 mol/L
Calculating this expression would give us the volume of ethanol that needs to be diluted with water to prepare the desired solution.