What's the Net Ionic equation of H3PO4(aq)+NaOH(aq)->NaH2PO4(aq)+H2O(l) ?
I know H3PO4 is weak so it doesn't dissociate, so what I got was
H3PO4 (aq) + OH^- (aq) -> 2H^+ (aq) + PO4^3- (aq) + H2O(l)
But in my next question it asks to calculate the heat of the rxn for 1 mol of product, but in the Standard Enthalpies I can't find PO4, leading me to believe that I did something incorrectly. Unless H2PO4 is it's on unit, not to be broken up?
I know H3PO4 is weak so it doesn't dissociate, so what I got was
H3PO4 (aq) + OH^- (aq) -> 2H^+ (aq) + PO4^3- (aq) + H2O(l)
But in my next question it asks to calculate the heat of the rxn for 1 mol of product, but in the Standard Enthalpies I can't find PO4, leading me to believe that I did something incorrectly. Unless H2PO4 is it's on unit, not to be broken up?
1 Answer
Feb 25, 2018
Well phosphoric acid is diacidic in water...
Explanation:
And so with the one equiv of hydroxide, we would write...
...and with 2 equiv...
You are forming one and two moles respectively of water in each reaction, and the thermodynamic parameters will reflect this....
