Answer:
33.1mL of 0.315M Ba(OH) are required to reach the equivalence point.
Explanation:
The reaction of HBr with Ba(OH)₂ is:
2HBr + Ba(OH)₂ → BaBr₂ + 2H₂O
That means to find the theoretical volume Cal need to add we need to find moles of HBr in solution, convert these to moles of Ba(OH)₂ and with its molar concentration find the volume, thus:
Moles HBr:
57.5mL = 0.0575L * (0.363mol/L) = 0.0209 moles HBr
Moles Ba(OH)₂:
0.0209 moles HBr * (1mol Ba(OH)₂ / 2 mol HBr) = 0.0104 moles Ba(OH)₂
Volume:
0.0104 moles Ba(OH)₂ * (1L / 0.315mol) = 0.0331L =
33.1mL of 0.315M Ba(OH) are required to reach the equivalence point.
