A 10.0 mL solution of HCl of unknown molarity is titrated with a .2M NaOH solution. If 40.0mL of NaOH is needed to reach the equivalence point, what was the initial concentration of the hydrochloric acid?
This titration is a strong acid- strong base titration. Therefore, the pH level at the equivalence point should be 7. All of the HCl will have been neutralized at this point. Since one mole of NaOH is required to neutralize one mole of HCl, it first necessary to find the number of moles of NaOH used in the titration.
The solution began with eight millimoles of hydrochloric acid. Since the volume of the original solution was 10.0 mL, the original solution was .8M HCl.
