How much of a 6.0M sucrose solution should you use to make 77.0mL of a 0.055M solution?
To determine how much of a 6.0M sucrose solution should be used, we need to calculate the volume of the 6.0M solution that contains enough sucrose to make a 0.055M solution.
The molarity (M) of a solution is defined as the number of moles of solute per liter of solution. In this case, the 6.0M solution has 6.0 moles of sucrose per liter.
To calculate the volume of the 6.0M solution needed, we can use the formula:
M₁V₁ = M₂V₂
Where:
M₁ = molarity of the initial solution (6.0M)
V₁ = volume of the initial solution to be used (unknown)
M₂ = molarity of the final solution (0.055M)
V₂ = volume of the final solution (77.0mL or 0.077L)
Rearranging the formula to solve for V₁:
V₁ = (M₂ * V₂) / M₁
Substituting the given values:
V₁ = (0.055M * 0.077L) / 6.0M
Simplifying the equation:
V₁ = 0.004235833333333333 L
Converting the volume to milliliters:
V₁ = 4.235833333333333 mL
Therefore, you should use approximately 4.24 mL of the 6.0M sucrose solution to make 77.0 mL of a 0.055M solution.
The dilution formula is
mL1 x M1 = mL2 x M2
mL1 x 6 = ....