What is the concentration of an HBr solution if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?

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Quizplus · Accepted Answer

The concentration of the HBr solution can be found using the concept of molarity and the stoichiometry of the neutralization reaction. The reaction between HBr and KOH is a 1:1 stoichiometry, meaning 1 mole of HBr reacts with 1 mole of KOH. Given that 15.0 mL of 0.25 M KOH is used, the moles of KOH are:$$ \text{Moles of KOH} = 0.25 \, \text{M} \times 0.015 \, \text{L} = 0.00375 \, \text{moles} $$Since the reaction is 1:1, the moles of HBr will also be 0.00375. To find the concentration of HBr:$$ \text{Concentration of HBr} = \frac{\text{Moles of HBr}}{\text{Volume of HBr solution in L}} = \frac{0.00375}{0.012} = 0.3125 \, \text{M} $$Rounded to two significant figures, the concentration of the HBr solution is 0.31 M.

What Is the Concentration of an HBr Solution If 12