Well as this is a neutralisation reaction you're goingto make a salt and water. So basically as you're making water, you know that's 2 hydrogens and an oxygen taken care with then you have 2 hydrogens, 4 oxygens, phosphorus and sodium left. This compound then has the formula of NaH2PO4.
Well as this is a neutralisation reaction you're goingto make a salt and water. So basically as you're making water, you know that's 2 hydrogens and an oxygen taken care with then you have 2 hydrogens, 4 oxygens, phosphorus and sodium left. This compound then has the formula of NaH2PO4.
H3PO4 + NaOH --> NaH2PO4(aq) + H2O
thanks for the helps ,but how would i apply the same method for e.g.
how do i work out the product of H3PO4 + NaOH ? ? ? ?
technically you could end up with three different salts: Na3PO4 NaHPO4 Na2H2PO4
however in a level syllabus im pretty sure you would just want Na3PO4 because H3PO4 is a strong acid therefore fully dissociates which leaves you with PO4(3-) ion hence sodium-phosphate
technically you could end up with three different salts: Na3PO4 NaHPO4 Na2H2PO4
however in a level syllabus im pretty sure you would just want Na3PO4 because H3PO4 is a strong acid therefore fully dissociates which leaves you with PO4(3-) ion hence sodium-phosphate
Thanks , im still confused as to how these are worked out or do you just have to memeorise them ?
Yeah I tried working them out once and it takes too much effort to make sense of it (though i managed it in the end). Im just gonna learn them
btw i learnt the ionic equaions so i can apply them to several compounds
hey man could you explain the priciple of how to work these out as my book doesnt have all the ones i need as apparently any combination of acid and base could come up on my exam ?
hey man could you explain the priciple of how to work these out as my book doesnt have all the ones i need as apparently any combination of acid and base could come up on my exam ?
its kinda guesswork but basically in the example of H3PO4: PO4^3- is the main ion and its bonded to 3H+ so it's triprotic (Bronsted-Lowry - donates protons). Therefore those H+ will be replaced by 3 positive charges from the metal its reacting with. eg with NaOH: H3PO4 + 3Na+ ---> Na3PO4 + 3H+
its kinda guesswork but basically in the example of H3PO4:PO4^3- is the main ion and its bonded to 3H+ so it's triprotic (Bronsted-Lowry - donates protons). Therefore those H+ will be replaced by 3 positive charges from the metal its reacting with. eg with NaOH: H3PO4 + 3Na+ ---> Na3PO4 + 3H+
Thanks alot ! that def makes sense , does it work with all acids and bases though ?