How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 132.0 mL of 0.21 M H2SO4?
How many mols do you need? That is M H2SO4 x L H2SO4 = ?
Then mL x M = moles Substitute the dilute numbers and solve for the unknown.
You can use the dilution formula, also, if that is easier for you.
c1v1 = c2v2
c = concn
v = volume
To solve this problem, we can use the formula of dilution:
C1V1 = C2V2
Where:
C1 = concentration of the stock solution (in mol/L)
V1 = volume of the stock solution to be used (in mL)
C2 = concentration of the final diluted solution (in mol/L)
V2 = final volume of the diluted solution (in mL)
In this problem, the stock solution has a concentration of 5.0 M and we want to prepare a final solution with a concentration of 0.21 M. The final volume of the diluted solution is given as 132.0 mL. We need to calculate the volume of the stock solution required.
Let's substitute the values into the formula and solve for V1:
(5.0 M)(V1) = (0.21 M)(132.0 mL)
Divide both sides by 5.0 M to isolate V1:
V1 = (0.21 M)(132.0 mL) / 5.0 M
V1 = 5.544 mL
Therefore, you would need to measure 5.544 mL of the 5.0 M H2SO4 stock solution to prepare 132.0 mL of a 0.21 M H2SO4 solution.