Calculate the volume of 7.53×10-2 M barium hydroxide required to neutralize 16.6 mL of a 0.331 M hydrobromic acid solution.

Question

Calculate the volume of 7.53×10^-2 M barium hydroxide required to neutralize 16.6 mL of a 0.331 M hydrobromic acid solution.

Answer 1

First, write the balanced equation for the reaction taking place:

Ba(OH)₂ + 2HBr ==> BaBr₂ + 2H₂O

Next, determine moles of HBr present:

moles HBr = 16.6 ml x 1 L / 1000 ml x 0.331 mol / L = 0.005495 mols

Finally, using stoichiometric mol ratios in the balanced equation, calculate volume of Ba(OH)₂ needed:

Volume Ba(OH)₂ = 0.005495 mol HBr x 1 mol Ba(OH)₂/ 2 mol HBr x 1 L / 7.5x10^-2 mol = 0.0366 L

So you need 0.0366 L or 36.6 mls of Ba(OH)₂