Asked by Jonny
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?
Answers
Answered by
DrBob222
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<sup>=</sup> is formed and how much HCl remains.
Determine how much H2PO4<sup>-</sup> is formed from the remaining HCl.
Use the Henderson-Hasselbalch equation with HPO4<sup>=</sup> = base and H2PO4<sup>-</sup> the acid.
Check my thinking. Post your work if you get stuck.
Determine how much HPO4<sup>=</sup> is formed and how much HCl remains.
Determine how much H2PO4<sup>-</sup> is formed from the remaining HCl.
Use the Henderson-Hasselbalch equation with HPO4<sup>=</sup> = base and H2PO4<sup>-</sup> the acid.
Check my thinking. Post your work if you get stuck.
Answered by
Jonny
wouldn't you do it a different way since the Na3PO4 is a salt?
Answered by
Jonny
and what would you do with the 500 mL dilution after everything?
Answered by
DrBob222
What do you have in mind?
Answered by
DrBob222
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.
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