How much of a 6.0 M sucrose solution should be used to make 81.0 mL of a 0.055 M solution?
To find out how much of a 6.0 M sucrose solution should be used to make a 81.0 mL of a 0.055 M solution, we need to use the concept of dilution.
Dilution is the process of reducing the concentration of a solute in a solution, by adding more solvent to the solution. The formula to determine the volume of the concentrated solution needed to make a diluted solution is:
C1V1 = C2V2
Where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.
Let's plug in the values for our problem:
C1 = 6.0 M (initial concentration)
V1 = unknown (initial volume)
C2 = 0.055 M (final concentration)
V2 = 81.0 mL (final volume)
Now, we can rearrange the formula to solve for V1:
V1 = (C2 * V2) / C1
Plugging in the values:
V1 = (0.055 M * 81.0 mL) / 6.0 M
Now, let's calculate:
V1 = 0.7475 mL
So, approximately 0.7475 mL of the 6.0 M sucrose solution should be used to make 81.0 mL of a 0.055 M solution.