Final answer:
To neutralize the 25.00 mL sample of 0.0597 M HBr, a volume of 0.03072 L (or 30.72 mL) of 0.0485 M KOH is needed.
Step-by-step explanation:
To answer this question, we can use the concept of stoichiometry to find the volume of KOH solution needed to neutralize the HBr. First, we need to calculate the number of moles of HBr in the 25.00 mL sample:
moles of HBr = volume (in L) * concentration (in M)
moles of HBr = 0.02500 L * 0.0597 M = 0.0014925 moles
Since the molar ratio of HBr to KOH is 1:1, the same number of moles of KOH is needed to neutralize the HBr. Now we can find the volume of the 0.0485 M KOH solution needed:
volume of KOH = moles of KOH / concentration of KOH
volume of KOH = 0.0014925 moles / 0.0485 M = 0.03072 L = 30.72 mL
Therefore, the correct answer is C) 30.45 mL.