Final answer:
To titrate 10.00 mL of 0.100 M HCl to the equivalence point, 40.0 milliliters of 0.025 M KOH are required.
Step-by-step explanation:
In order to determine the number of millimeters of 0.025 M KOH required to titrate 10.00 mL of 0.100 M HCl to the equivalence point, we can use the concept of stoichiometry. The balanced chemical equation for the reaction between KOH and HCl is:
KOH + HCl → KCl + H2O
From the equation, we can see that 1 mole of KOH reacts with 1 mole of HCl. Therefore, we can calculate the number of moles of HCl in 10.00 mL of 0.100 M HCl:
Moles of HCl = Volume (L) × Concentration (M) = 0.0100 L × 0.100 M = 0.00100 moles
Since the stoichiometry is 1:1, we know that 0.00100 moles of KOH will be required to reach the equivalence point. To find the volume of KOH solution in milliliters, we can use its molarity and the number of moles:
Volume (mL) = Moles ÷ Concentration (M) = 0.00100 moles ÷ 0.025 M = 40.0 mL
Therefore, 40.0 milliliters of 0.025 M KOH are required to titrate 10.00 milliliters of 0.100 M HCl to the equivalence point.