What volume of a 0.352 M hydrobromic acid solution is required to neutralize 24.1 mL of a 0.119 M barium hydroxide solution?

Question

 mL hydrobromic acid

Answer 1

First thing to do is to determine the balanced chemical equation:

2 HBR(aq) + Ba(OH)₂(aq) <=> BaBr₂(aq) + 2H20(aq)

Here we see that Hydrobromide reacts with Barium Hydroxide in a 1:2 mole ration. This means that it takes two moles of Barium Hydroxide to neutralise 1 mole of Hydrobromide .

Now we will use stoichometry to find out how many mL of Hydrobromic acid will be needed:

24.1 ml = 0.0241 L Ba(OH)₂

0.0241 L Ba(OH)₂ x ( 0.119 moles Ba(OH)₂/ L) x (2 mol HBR/ 1 mol Ba(OH)₂₎ x ( 1 L / 0.352 moles HBR) = 0.0163 L

16.3 mL of HBR will need to be added.

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