sir
p2o5+H2o = H2P2O6
why is it H3po4? instead of H2P2O6 please explain me
You appear to be trying to use the reactants and simply sum them to find the product. That is what is wrong.
For example, Na + Cl2 ==> is not NaCl2 but NaCl. When Na combines with Na, the result is NaCl because Na has a valence of +1 and Cl has a valence of -1 therefore the formula is NaCl. You take care of making the atoms equal by balancing the equation.
Na + Cl2 ==> NaCl and we balance it like this.
2Na + Cl2 ==> 2NaCl.
K2O + H2O ==> is not K2H2O2 but KOH. We balance it as this.
K2O + H2O ==> 2KOH
Sure, I'd be happy to explain why the formula is H3PO4 instead of H2P2O6.
To understand this, let's look at the balanced chemical equation: p2o5 + H2o → H2P2O6.
In this equation, the reactants are P2O5 (diphosphorus pentoxide) and H2O (water), and the product is H2P2O6 (diphosphoric acid). However, it's important to note that this is not the final product.
Diphosphorus pentoxide (P2O5) reacts with water (H2O) to form diphosphoric acid (H2P2O6) as an intermediate product.
The next step involves the dissociation of the intermediate product. When diphosphoric acid (H2P2O6) dissociates, it forms three H+ ions (protons) and one phosphate ion (PO4^3-).
The balanced equation for the dissociation is: H2P2O6 → 2H+ + HPO4^2-
Now, the hydrogen phosphate ion (HPO4^2-) can further protonate to form the final product, which is phosphoric acid (H3PO4). This is done by taking up another H+ ion, as shown in the following equation: HPO4^2- + H+ → H2PO4^-
Finally, when H2PO4^- accepts another H+ ion, it forms the fully protonated form of phosphoric acid, H3PO4.
So, in summary, the reason why the formula is H3PO4 instead of H2P2O6 is because diphosphoric acid (H2P2O6) dissociates into H+ ions and a phosphate ion (PO4^3-), which further undergoes protonation to form phosphoric acid (H3PO4).