What volume of NaOH(aq) would be needed to reach the equivalence point if the concentration of the added base were 0.290 M?

17.2mL are needed

Explanation:

The pH curve for titration of 50.0 mL of a 0.100 M solution of hydrochloric acid

A strong acid as HCl reacts with a strong base as NaOH producing water and a salt. The chemical equation is:

HCl + NaOH → H₂O + NaCl

Where 1 mole of HCl reacts per mole of NaOH

To solve this question we must find the moles of HCl added = Moles NaOH you must add to reach the equivalence point. With these moles and the molar concentration we can find the volume that would be needed as follows:

Moles HCl:

50.0mL = 0.0500L * (0.100moles / L) = 0.00500 moles HCl = Moles NaOH

Volume NaOH:

0.00500 moles NaOH * (1L / 0.290moles) = 0.0172L NaOH =

it is b that is the answer.