Answer:
0.156 M
Explanation:
The neutralization reaction between hydrobromic acid (HBr) and sodium hydroxide (NaOH) is the following:
HBr(ac) + NaOH(aq) → NaBr(aq) + H₂O(l)
As we can see, 1 mol of HBr reacts with 1 mol NaOH. During a titration, at the equivalence point, the number of moles of NaOH added reacts completely with the number of moles of HBr:
moles of NaOH = moles of HBr
The moles of each reactant is calculated as the product of the molarity (M) and the volume (V):
M(NaOH) x V(NaOH) = M(HBr) x V(HBr)
We have the following data:
base: V(NaOH) = 13.5 mL
acid: M(HBr) = 0.104 M; V(HBr) = 20.2 mL
Thus, we calculate M(NaOH) from the equivalent point equation:
M(NaOH) = (M(HBr) x V(HBr))/(V(NaOH) = (0.104 M x 20.2 mL)/(13.5 mL) = 0.1556 M ≅ 0.156 M
