What is the stoichiometric ratio of the reaction between 1.0M H3PO4 to NaOH?
Both will dissociate like so NaOH + H3PO4 –> Na+ + OH- + H+ + HPO4(2-) The full ionic equation is as follows Na+ + OH- + H+ + HPO4(2-) –> H2O + Na+ + HPO4(2-) The stoichiometric ratio is 1:1. Even though H3PO4 can lose three protons, it will lose the first one readily, but it is very hard to lose the second one and even harder to lose the last one. (Look up ka1, ka2 and ka3). However, your teacher may want an answer of 3H+ to 1OH- because H3PO4 can theoretically lose three protons (though not experimentally).
