40.0 mL of a 0.65 M solution of HF is titrated with 0.100 M NaOH. After 0.400 L of the NaOH solution has been added, the resultant solution is:

Question

Quizplus · Accepted Answer

To determine the nature of the solution after titration, we first calculate the moles of HF and NaOH involved. Moles of HF = 0.040 L * 0.65 M = 0.026 moles. Moles of NaOH = 0.400 L * 0.100 M = 0.040 moles. Since more moles of NaOH have been added than there are moles of HF, all the HF will react, and there will be excess NaOH, making the solution basic. The reaction has passed the equivalence point because the amount of NaOH added exceeds the stoichiometric amount needed to neutralize the HF.

400 ML of a 0