Final answer:
In a titration, the volume of a 2.000 M KOH solution required to neutralize 30.00 mL of 1.000 M HI is 30.00 mL.
Step-by-step explanation:
In a titration, the goal is to determine the volume of one solution that is needed to react completely with another solution. To find the volume of a 2.000 M KOH solution required to neutralize 30.00 mL of 1.000 M HI, we can use the balanced chemical equation for the reaction:
HCl (aq) + KOH (aq) → KCl (aq) + H2O (l)
From the equation, we can see that the stoichiometric ratio between HI and KOH is 1:1. This means that for every 1 mole of HI, 1 mole of KOH is needed. Therefore, the volume of KOH needed would be the same as the volume of HI used, which is 30.00 mL.