Final answer:
To prepare 1.00 L of a 0.0250 M NaOH solution, 12.5 mL of a 2.00 M standard NaOH solution is required, found using the dilution formula, C1V1 = C2V2.
Step-by-step explanation:
The question asks what volume of a 2.00 molar sodium hydroxide (NaOH) solution is needed to prepare a 1.00 L of a 0.0250 molar NaOH solution. To answer this, we use the concept of dilution, which is based on the principle that the number of moles of solute before dilution equals the number of moles after dilution (moles before = moles after). The original concentration (C1) of the NaOH solution is 2.00 M, and we want to achieve a final concentration (C2) of 0.0250 M.
Using the dilution formula, which is C1V1 = C2V2, where V1 is the volume of the initial concentrated solution we need to find, we can rearrange it to solve for V1:
V1 = (C2V2) / C1
Substituting the known values, we get:
V1 = (0.0250 M * 1.00 L) / 2.00 M
V1 = 0.0125 L or 12.5 mL
Therefore, to prepare 1.00 L of a 0.0250 M NaOH solution, 12.5 mL of a 2.00 M standard NaOH solution is needed.