The volume of 18 molar concentrated H2SO4 that must be diluted with distilled water to prepare 10 liters
To prepare 10 L of WHAT?
To find the volume of 18-molar concentrated H2SO4 that must be diluted with distilled water to prepare 10 liters, you need to understand the concept of molarity and dilution.
Molarity (M) is a measure of the concentration of a solution, defined as the number of moles of solute per liter of solution. In this case, the given concentration is 18 M.
To prepare the desired 10 liters of a diluted solution, you will need to dilute the concentrated H2SO4 with distilled water. The final concentration will depend on the volume of the concentrated solution added.
To solve this problem, you can use the formula for dilution:
M1V1 = M2V2
Where:
M1 is the initial concentration of the concentrated solution
V1 is the initial volume of the concentrated solution
M2 is the final concentration of the diluted solution
V2 is the final volume of the diluted solution
In this case, M1 = 18 M, V1 is unknown, M2 is 10 M (assuming you want the final concentration to be 10 M), and V2 = 10 L.
Plugging in the values into the formula:
(18 M) * V1 = (10 M) * (10 L)
Simplifying the equation:
(18 M) * V1 = 100 M * L
V1 = 100 M * L / 18 M
V1 ≈ 5.556 liters
Therefore, you will need to dilute approximately 5.556 liters of the 18 M concentrated H2SO4 with distilled water to prepare 10 liters of a 10 M diluted solution.