Determine the mols Na3PO4 in 0.322 g Na3PO4 and mols HCl in 14.35 mL of 0.200 F HCl.
Determine how much HPO4= is formed and how much HCl remains.
Determine how much H2PO4- is formed from the remaining HCl.
Use the Henderson-Hasselbalch equation with HPO4= = base and H2PO4- the acid.
Check my thinking. Post your work if you get stuck.
What is the pH of a solution formed by mixing 14.35 mL of 0.200 F HCl with 0.322 g of Na3PO4, followed by dilution to 500.00 mL?
5 answers
wouldn't you do it a different way since the Na3PO4 is a salt?
and what would you do with the 500 mL dilution after everything?
What do you have in mind?
dilution just changes the concentration.
concn = mols/L. And both salt and acid are diluted to the same volume.
concn = mols/L. And both salt and acid are diluted to the same volume.