How much ml of H2So4 added to make 0.02M H2So4 solution to make volume 250ml?

You have to have the initial concentration of the sulfuric acid.

Here is an example: Pretend it is concentrated H2SO4 (12M).

you are diluting it 12/.02 or 60 times. So you need one part acid, 59 parts water.

1 part acid is 250/60, or 4.1ml acid
and the remainder is water. Always add acid to water.

gogo

To determine the amount of H2SO4 needed to create a 0.02M H2SO4 solution with a volume of 250ml, we can use the formula:

M1V1 = M2V2

Where:
M1 = initial concentration
V1 = initial volume
M2 = final concentration
V2 = final volume

In this case, the initial concentration (M1) is unknown, the initial volume (V1) is also unknown, the final concentration (M2) is 0.02M, and the final volume (V2) is 250ml.

Let's substitute the values into the formula:

M1 * V1 = 0.02 * 250

Since M1 and V1 are both unknown, we can't calculate their exact values. However, if we assume that the initial volume (V1) is greater than 250ml, we can still find the concentration (M1) needed to obtain the desired final concentration.

For example, let's assume the initial volume (V1) is 500ml. The equation becomes:

M1 * 500 = 0.02 * 250

M1 = (0.02 * 250) / 500

M1 = 0.01M

Therefore, to make a 0.02M H2SO4 solution with a volume of 250ml, you would need to add 250ml of a 0.01M H2SO4 solution.
Alternatively, if you have concentrated H2SO4 with a known concentration, you can calculate the volume needed to dilute it to the desired final concentration using the same formula.