what volume of a 2.5m stock soltio of acetic acid (HC2H3O2) is required to prepare 100.0 mililiters of a 0.50m acetic acid solution?
If you are too lazy to find (and use) the caps key in chemistry it can lead to serious problems. If m should be M (M = MOLAR; m = MOLAL) the answer provided by Wrinkly is correct. The same applies to things such as Co = cobalt, CO = carbon monoxide, co = company, etc. Beware.
To calculate the volume of the stock solution required, you need to use the equation:
C1V1 = C2V2
Where:
C1 = concentration of the stock solution
V1 = volume of the stock solution
C2 = concentration of the desired solution
V2 = volume of the desired solution
Let's plug in the known values:
C1 = 2.5 M (concentration of the stock solution)
V1 = ?
C2 = 0.50 M (concentration of the desired solution)
V2 = 100.0 mL (volume of the desired solution)
Now, rearrange the equation to solve for V1:
V1 = (C2 * V2) / C1
Substituting the values:
V1 = (0.50 M * 100.0 mL) / 2.5 M
Simplifying the equation:
V1 = 20 mL
Therefore, you would need 20 mL of the 2.5 M stock solution of acetic acid to prepare 100.0 mL of a 0.50 M acetic acid solution.
Use M1V1=M2V2
(2.5M)(X)=(0.1)(0.50M)
X=(0.1)(0.50)/2.5
X-0.02 L or 20 ML
2O ML.