What mass in grams of dextrose (C6H12O6) will be required to produce 6.00 L of a 0.15M aqueous solution?
Question 5 answers
How many moles do you need in the final solution? That is M x L = ?
Then moles dextrose = grams/molar mass. Solve for grams.
To find the mass of dextrose required to produce the given concentration and volume of the solution, you need to use the formula:
Molarity (M) = moles of solute / volume of solution (L)
First, rearrange the formula to solve for moles of solute:
moles of solute = Molarity (M) x volume of solution (L)
Now, substitute the given values into the formula:
moles of solute = 0.15 mol/L x 6.00 L
Calculate the moles of solute:
moles of solute = 0.9 mol
Next, you need to convert moles of dextrose to grams using its molar mass.
The molar mass of dextrose (C6H12O6) can be calculated as follows:
(6 x atomic mass of carbon) + (12 x atomic mass of hydrogen) + (6 x atomic mass of oxygen)
(6 x 12.01 g/mol) + (12 x 1.01 g/mol) + (6 x 16.00 g/mol)
= 180.18 g/mol
Finally, calculate the mass of dextrose required:
mass of dextrose = moles of solute x molar mass
mass of dextrose = 0.9 mol x 180.18 g/mol
mass of dextrose = 162.162 g
Therefore, you would need 162.162 grams of dextrose to produce 6.00 L of a 0.15M aqueous solution.