How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 125.0 mL of 0.19 M H2SO4?
mL x M = mL x M
4.75 mL
3289 mL
u r stupid this is wrong
To find out how many milliliters of a 5.0 M H2SO4 stock solution you need to prepare 125.0 mL of 0.19 M H2SO4, we can use the following formula:
M1 * V1 = M2 * V2
Where:
M1 is the initial concentration of the stock solution (5.0 M),
V1 is the volume of the stock solution needed (unknown),
M2 is the final concentration of the desired solution (0.19 M),
V2 is the final volume of the desired solution (125.0 mL).
Plugging these values into the formula, we get:
(5.0 M)(V1) = (0.19 M)(125.0 mL)
Now, solve for V1:
V1 = (0.19 M)(125.0 mL) / (5.0 M)
V1 = 4.75 mL
Therefore, you would need 4.75 milliliters of the 5.0 M H2SO4 stock solution to prepare 125.0 mL of 0.19 M H2SO4.