What volume (in ml) of 0.8 M barium hydroxide would neutralize 50 ml of 2.709 M hydrobromic acid? Enter to 1 decimal place.

Question

What volume (in ml) of 0.8 M barium hydroxide would neutralize 50 ml of 2.709 M hydrobromic acid?  Enter to 1 decimal place.

Answer 1

Write the balanced equation:

Ba(OH)₂ + 2HBr ==> BaBr₂ + 2H₂O

Find moles of HBr present:

50 ml x 1 L/1000 ml x 2.709 mol/L = 0.13545 moles HBr

Find moles Ba(OH)₂ needed:

0.13545 mol HBr x 1 mol Ba(OH)₂ / 2 mol HBr = 0.067725 moles Ba(OH)₂ needed to react with HBr.

Find volume of Ba(OH)₂ solution needed to provide 0.067725 moles:

(0.8 moles / L) (x L) = 0.067725 moles

x = 0.08466 L = 84.7 mls