# Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652c: 50

$H_3PO_4(aq) + H_2O(l) \lt -- \gt H_2{PO_4}^-(aq) + H_3O^+(aq)$ $H_2{PO_4}^-(aq) + H_2O(l) \lt -- \gt H{PO_4}^{2-}(aq) + H_3O^+(aq)$ $HP{O_4}^{2-}(aq) + H_2O(l) \lt -- \gt {PO_4}^{3-}(aq) + H_3O^+(aq)$

#### Work Step by Step

1. Write the ionization equation for the original acid. - Write an equation where $H_3PO_4$ donates a proton to a water molecule. 2. Now, for polyprotic acids, the conjugate base is capable of donating one proton too, so write an equation where it does that. - $H_2P{O_4}^-$ can act as an acid too, so write an equation where it donates a proton to a water molecule. - Repeat "Step 2" for the next reaction, until the conjugate base is incapable of donating one proton.

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