To what volume must 25.0mL of 18.0M H2SO4 be diluted to produce 1.50 M H2SO4?
same dilution formula.
To calculate the volume to which the 18.0 M H2SO4 should be diluted to produce a 1.50 M H2SO4 solution, we need to use the dilution formula:
C1V1 = C2V2
Where:
C1 = initial concentration of the solution
V1 = initial volume of the solution
C2 = final concentration of the solution
V2 = final volume of the solution
In this case, we have:
C1 = 18.0 M
V1 = 25.0 mL
C2 = 1.50 M
V2 = ?
Rearranging the formula to find V2:
V2 = (C1 * V1) / C2
Substituting the known values:
V2 = (18.0 M * 25.0 mL) / 1.50 M
Now let's calculate it step by step:
Step 1: Convert milliliters to liters
V2 = (18.0 M * 0.025 L) / 1.50 M
Step 2: Simplify the expression
V2 = (0.45 L) / 1.50 M
Step 3: Calculate the volume
V2 = 0.30 L
Therefore, 25.0 mL of 18.0 M H2SO4 should be diluted to a volume of 0.30 liters (or 300 mL) to produce a 1.50 M H2SO4 solution.
To find the volume of 18.0M H2SO4 that must be diluted to produce 1.50M H2SO4, we can use the dilution formula:
M1 * V1 = M2 * V2
Where:
M1 = initial concentration of the solution (18.0M)
V1 = initial volume of the solution (25.0mL)
M2 = final concentration of the solution (1.50M)
V2 = final volume of the solution (unknown)
Substituting the given values into the formula, we have:
(18.0M) * (25.0mL) = (1.50M) * V2
Now we can solve for V2:
V2 = (18.0M * 25.0mL) / 1.50M
V2 = 300mL
Therefore, 25.0mL of 18.0M H2SO4 must be diluted to a volume of 300mL in order to produce a 1.50M H2SO4 solution.