Question
Suggest a reason why the acid strength decreases with each step in the ionization of phosphoric acid: $\mathrm{H}_{3} \mathrm{PO}_{4} \rightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^{-} \rightarrow$$\mathrm{HPO}_{4}^{2-}$
Step 1
When a proton (hydrogen ion) is removed from this acid, it becomes $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$. This process is relatively easy because a single positive charge (the proton) is being removed from a neutral species. Show more…
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We learned in Chapter 16 that for polyprotic acids, ionization constants for successive ionization steps decrease rapidly. That is, $K_{\mathrm{a}_{1}} \gg K_{\mathrm{a}_{2}} \gg K_{\mathrm{a}_{3}} .$ The ionization constants for the first two steps in the ionization of $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(\text { reactions } 24.10 \text { and } 24.11)$ are more nearly equal in magnitude. Why does this multistep ionization seem not to follow the pattern for polyprotic acids?
Explain why acid strength increases in the order $\mathrm{HClO} <\mathrm{HClO}_{2} <\mathrm{HClO}_{3}< \mathrm{HClO}_{4}$
Explain why the Ka value of a polyprotic acid gets smaller each time it loses a hydrogen ion?
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