What is the concentration of 10.00 mL of HBr if it takes 16.73 mL of a 0.253 M LiOH solution to

Question

neutralize it?

Answer 1

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.