Answer: 0.075 L or 75.0 mL
Step-by-step explanation:
In a titration, the equivalence point is when the moles of acid are equal to the moles of base. From the balanced chemical equation for the reaction between HCl and Ba(OH)2, we know that 2 moles of HCl are required to react with 1 mole of Ba(OH)2.
So, the number of moles of Ba(OH)2 used in the titration is:
(0.100 mol/L) x (0.01500 L) = 0.0015 mol
Since 2 moles of HCl react with 1 mole of Ba(OH)2, the number of moles of HCl required to reach the equivalence point is:
0.0015 mol Ba(OH)2 x (2 mol HCl/1 mol Ba(OH)2) = 0.0030 mol HCl
To calculate the volume of 0.100 M HCl required to provide 0.0030 moles of HCl, we can use the following formula:
moles of solute = concentration x volume (in liters)
0.0030 mol = (0.100 mol/L) x volume
volume = 0.0030 mol / 0.100 mol/L = 0.0300 L = 30.0 mL
Therefore, 30.0 mL of 0.100 M HCl is required to reach the equivalence point.