1. Write out the balanced equation for the reaction of 1 mole of NaOH with 1 mole of H3PO4:

2. Write out the balanced equation for the reaction of 2 moles of NaOH with 1 mole of H3PO4:

3. Explain how the volume data from the indicator reactions corresponds to the dual steep slopes on the pH vs volume of base curve.

4. Explain how the pH range for the change of color of the two indicators corresponds with the shape of the pH curve.

5. Write out the net ionic reaction for 1 mole of OH– reacting with one mole of H3PO4. Below the first equation, line up and write out the net ionic reaction for 1 mole of OH– reacting with the non-water product of the first reaction:

6. Given similar concentrations, the stronger the acid, the lower the pH. Comment on the relative strengths of the acids H3PO4 and H2PO4 –.

Answer rating: 100% (QA)

NaOt Po4 Nat P04 H 2NAOH It3poa Na HPog 2H20 PH US ... View the full answer