What is the concentration of 10.00 mL of HBr if it takes 16.73 mL of a 0.253 M LiOH solution to
neutralize it?
First, we can write a balanced chemical equation for the reaction between HBr and LiOH:
HBr + LiOH -> LiBr + H2O
Since the reaction is a acid-base neutralization reaction, we can use the following equation to calculate the concentration of HBr:
C(HBr) x V(HBr) = C(LiOH) x V(LiOH)
where C is the concentration in mol/L and V is the volume in L.
Plugging in the given values, we get:
C(HBr) x 10.00 mL = 0.253 M x 16.73 mL
C(HBr) = (0.253 M x 16.73 mL) / 10.00 mL
C(HBr) = 0.425 M
Therefore, the concentration of the HBr solution is 0.425 M.