What volume of 6.0m H2SO4 is needed to prepare 0.5L of a 0.3M H2SO4 solution?
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Use the dilution formula.
c1v1 = c1v2
c = concentration
v = volume.
To find the volume of a 6.0M H2SO4 solution needed to prepare a 0.5L of 0.3M H2SO4 solution, we can use the concept of molarity and the formula:
M1V1 = M2V2
where:
M1 = initial concentration of the solution (6.0M)
V1 = initial volume of the solution (unknown)
M2 = final concentration of the solution (0.3M)
V2 = final volume of the solution (0.5L)
Now let's solve for V1:
M1V1 = M2V2
(6.0M)(V1) = (0.3M)(0.5L)
Divide both sides of the equation by 6.0M:
V1 = (0.3M)(0.5L) / 6.0M
Now calculate the volume:
V1 = (0.15L) / 6.0
V1 = 0.025L
Therefore, the volume of the 6.0M H2SO4 solution needed to prepare 0.5L of a 0.3M H2SO4 solution is 0.025L (or 25mL).