Question

A 10.9 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid. If 26.1 mL of 0.245 M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass of hydrobromic acid in the mixture?

Answer 1

2HBr(aq) + Ba(OH)₂ -------> BaBr₂(aq) + 2H₂O(l)

This is the neutralization reaction that is taking place and it is balanced

Moles of barium hydroxide, Ba(OH)2 = molarity x volume (L)

Given, Molarity of barium hydroxide = 0.245 M

Volume of barium hydroxide = 26.1 mL = 0.0261 L

Moles of barium hydroxide =

From balanced reaction mole ratio b/w HBr : Ba(OH)2 = 2:1

Mass of HBr present in 10.9 g sample =

=1.035 g HBr

Mass of HBr present in 10.9 g sample = 1.035 g

Mass of Ba(OH)2 =

=1.095 g

Mass of Ba(OH)2 = 1.095 g

Percent by mass of HBr in the mixture =

=48.6%

Percent by mass of HBr = 48.6%

answered by: anonymous