how many milliliters of 5.5M H2so4 must you use to prepare 500ml of 0.2M sulfuric acid solution? Please hurry!!!!!!
the .2M H2SO4 contains .1 moles
so, you'd need only .1/5.5 = .018 L of the 5.5M acid
or, 18 mL
To find out how many milliliters of 5.5M H2SO4 you need to prepare a 500ml of 0.2M sulfuric acid solution, you can use the equation:
M1V1 = M2V2
where:
M1 = initial molarity (5.5M)
V1 = initial volume (unknown)
M2 = final molarity (0.2M)
V2 = final volume (500ml)
Rearranging the equation, we get:
V1 = (M2 * V2) / M1
Substituting the given values, we have:
V1 = (0.2M * 500ml) / 5.5M
V1 ≈ 18.18ml (rounded to two decimal places)
Therefore, you need approximately 18.18 milliliters of 5.5M H2SO4 to prepare 500ml of 0.2M sulfuric acid solution.