STOICHIOMETRY REACTION

Question

What volume of a 0.308 M hydrobromic acid solution is required to neutralize 23.9 mL of a 0.197 M sodium hydroxide solution

Answer 1

Write the correctly balanced equation:

HBr(aq) + NaOH(aq) ==> NaBr(aq) + H₂O(l)'

You can use V1M1 = V2M2 to find the volume of HBr:

(x ml)(0.308 M) = (23.9 ml)(0.197 M)

x = 15.3 ml HBr

The long way is:

calculate moles of NaOH present: 23.9 ml x 1 L/1000 ml x 0.197 mol/L = 0.004708 mol NaOH

moles HBr needed = 0.004708 since the balanced eq. shows they react 1:1

volume HBr: (x L)(0.308 mol/L) = 0.004708 moles

x = 0.01528 L = 15.3 ml (3 sig. figs.)