Help me please! Is Ba3(po4)2 soluble in water?
Is Ba3(PO4)2 soluble in water? In the following equation, what is the state of Ba3(PO4)2?
Ba(OH)2 (aq) + H3PO4 (aq) ———-> H2O (l) + Ba3(PO4)2
Should Ba3(PO4)2 be classified as (s) or (aq)? Additionally, is this an acid-base reaction? I understand that phosphate salts are generally insoluble. Is it possible for an acid-base reaction to produce a solid salt?
5 Answers
Barium phosphate will precipitate out of this solution as a solid, as it is extremely insoluble in water.
This is an acid/base reaction. Yes, the solid barium phosphate produced here is a solid salt.
If you want to be tecnical the salt would be soluble if the final solution was acidic (Phosphoric acid in excess) however the reaction would most likely result in a precipitate (solid) for most purposes.
The reaction between Ba(OH)2(aq) and H2SO4(aq) will produce BaSO4(s) and H2O(l)
Hmmm PO4 salts are insoluble, based on what info?
sodium phosphates are soluble in water.
barium phosphate is slightly soluble in water
You need to balance your equation. Also, everything is soluble, it just depends on how much. I think Ba3PO4 is only very slightly soluble, however, if only a teensy amount is being produced, it may be all dissolved and if you have any pH modifiers or buffers then it depends.
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