What mass (g) of the solute C3H8O3 should be mixed with 8270 mL of the solvent H2O to produce a solution that is 1.02 m glycerol.
Molar Mass (g/mol)
C3H8O3 92.09
H2O 18.015
Density (kg/L):
C3H8O3 1.261
H2O 0.9982
Name/Formula:
glycerol
C3H8O3
water
H2O
mols solute/kg solvent = molality
You know molality, you know kg solvent, calculate mols solute.
Then mols = grams/molar mass.
You know mols from above, you know molar mass solute, calculate grams solute.
To solve this problem, we can use the concept of molarity. Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, we are given the molarity (1.02 M) and the volume of the solvent (8270 mL = 8.27 L).
The molarity formula is:
Molarity (M) = Moles of Solute / Volume of Solution (in L)
We can rearrange this formula to solve for the moles of solute:
Moles of Solute = Molarity x Volume of Solution
Now, let's calculate the moles of solute using the given molarity and volume of solution:
Moles of Solute = 1.02 M x 8.27 L
Moles of Solute = 8.4654 moles
Next, we need to convert the moles of solute to grams using the molar mass of glycerol (C3H8O3).
Molar mass (C3H8O3) = 92.09 g/mol
Grams of Solute = Moles of Solute x Molar mass of Solute
Grams of Solute = 8.4654 moles x 92.09 g/mol
Grams of Solute = 779.28 g
Therefore, 779.28 grams of the solute C3H8O3 should be mixed with 8270 mL of the solvent H2O to produce a solution that is 1.02 m glycerol.