To what volume should you dilute 25mL of a 12.0M H2SO4 solution to obtain a 0.170M H2S04 solution?
mL x M = mL x M
To calculate the volume of the 12.0 M H2SO4 solution that needs to be diluted to obtain a 0.170 M H2SO4 solution, you can use the formula:
C1V1 = C2V2
Where:
C1 = Initial concentration of the H2SO4 solution (12.0 M)
V1 = Initial volume of the H2SO4 solution (unknown)
C2 = Final concentration of the H2SO4 solution (0.170 M)
V2 = Final volume of the H2SO4 solution (25 mL)
Rearranging the formula to solve for V1, we get:
V1 = (C2V2) / C1
Plugging in the values, we have:
V1 = (0.170 M * 25 mL) / 12.0 M
V1 = (4.25 mL) / 12.0
V1 = 0.354 mL
Therefore, you need to dilute 25 mL of the 12.0 M H2SO4 solution to a volume of 0.354 mL to obtain a 0.170 M H2SO4 solution.
To determine the volume to which you should dilute the 25mL of 12.0M H2SO4 solution, you can use the dilution formula:
M1V1 = M2V2
Where:
M1 = initial concentration (12.0M)
V1 = initial volume (25mL)
M2 = final concentration (0.170M)
V2 = final volume
Rearranging the formula to find V2:
V2 = (M1V1) / M2
Substituting the given values:
V2 = (12.0M * 25mL) / 0.170M
V2 = 1764.70588 mL ≈ 1765 mL (rounded to three significant figures)
Therefore, you should dilute the 25mL of 12.0M H2SO4 solution to a final volume of approximately 1765 mL to obtain a 0.170M H2SO4 solution.