How many milliliters of 0.50M NaOH solution are required to titrate 20.0mL of a 0.20M H2SO4 solution to an end point?

2NaOH + H2SO4 ==> Na2SO4 + 2H2O

mols H2SO4 = M x L = ?
mols NaOH = twice that
M NaOH = mols NaOH/L NaOH. You know M and mols, solve for L and convert to mL.

To find the number of milliliters of 0.50M NaOH solution required to titrate 20.0mL of a 0.20M H2SO4 solution, we can use the equation:

M1V1 = M2V2

Where:
M1 = molarity of the first solution (0.20M H2SO4)
V1 = volume of the first solution (20.0mL)
M2 = molarity of the second solution (0.50M NaOH)
V2 = volume of the second solution (unknown)

Rearranging the equation to solve for V2, we get:

V2 = (M1 * V1) / M2

Let's substitute the given values:

V2 = (0.20M * 20.0mL) / 0.50M

V2 = (4.0 mL⋅M) / 0.50M

V2 = 8.0 mL

Therefore, 8.0 milliliters of the 0.50M NaOH solution are required to titrate 20.0mL of the 0.20M H2SO4 solution to an end point.