Answer:
253.5mL of Ba(OH)₂ are required to neutralize the HCl solution
The pH at equivalence point is = 7
Explanation:
The reaction of Ba(OH)₂ with HCl is:
Ba(OH)₂ + 2HCl → BaCl₂ + 2H₂O
First, we need to find moles of HCl. With these moles and the chemical equation we can find the moles of Ba(OH)₂ and the volume required:
<em>Moles HCl:</em>
75.0mL = 0.075L * (0.845mol / 1L) = 0.063375moles HCl
<em>Moles Ba(OH)₂:</em>
0.06338moles HCl * (1mol Ba(OH)₂ / 2mol HCl) = 0.03169 moles Ba(OH)₂
<em>Volume of the 0.125M Ba(OH)₂:</em>
0.03169 moles Ba(OH)₂ * (1L / 0.125mol) = 0.2535L are required =
253.5mL of Ba(OH)₂ are required to neutralize the HCl solution
As the titration was of a strong acid, HCl, with a strong base, Ba(OH)₂, the pH at equivalence point is = 7
