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Chapter 14: Problem 19

Anions containing hydrogen (for example, \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) ) usually show amphoteric behavior. Write equations illustrating the amphoterism of these two anions.

Short Answer

Expert verified
The amphoteric behavior of the anions \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) can be illustrated through the following equations: 1. \( \mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{CO}_{3}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+} \) (Base) 2. \( \mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{2}\mathrm{CO}_{3}+\mathrm{OH}^{-} \) (Acid) 3. \( \mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}\mathrm{PO}_{4}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+} \) (Base) 4. \( \mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{3}\mathrm{PO}_{4}+\mathrm{OH}^{-} \) (Acid)

Step by step solution

01

Write the equation for \(\mathrm{HCO}_{3}^{-}\) acting as a base

In this case, \(\mathrm{HCO}_{3}^{-}\) will accept a proton from water. The reaction is as follows: \(\mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{CO}_{3}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+}\)
02

Write the equation for \(\mathrm{HCO}_{3}^{-}\) acting as an acid

In this case, \(\mathrm{HCO}_{3}^{-}\) will donate a proton to water. The reaction is as follows: \(\mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{2}\mathrm{CO}_{3}+\mathrm{OH}^{-}\)
03

Write the equation for \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) acting as a base

In this case, \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) will accept a proton from water. The reaction is as follows: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}\mathrm{PO}_{4}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+}\)
04

Write the equation for \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) acting as an acid

In this case, \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}\) will donate a proton to water. The reaction is as follows: \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{3}\mathrm{PO}_{4}+\mathrm{OH}^{-}\) By combining all the equations, we can see that both anions show amphoteric behavior: 1. \(\mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{CO}_{3}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+}\) (Base) 2. \(\mathrm{HCO}_{3}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{2}\mathrm{CO}_{3}+\mathrm{OH}^{-}\) (Acid) 3. \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}\mathrm{PO}_{4}^{2-}+\mathrm{H}_{3}\mathrm{O}^{+}\) (Base) 4. \(\mathrm{H}_{2}\mathrm{PO}_{4}^{-}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{3}\mathrm{PO}_{4}+\mathrm{OH}^{-}\) (Acid)

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of a \(0.200 \mathrm{M}\) solution of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\). Hint: \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\) is a salt composed of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}\) and \(\mathrm{F}^{-}\) ions. The prin- cipal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(a q)+\mathrm{F}^{-}(a q) \rightleftharpoons\) \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}(a q)+\mathrm{HF}(a q) \quad K=8.2 \times 10^{-3}\)

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Calculate the \(\mathrm{pH}\) of a \(0.050 \mathrm{M}\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) solution \(\left(K_{\mathrm{b}}=\right.\) \(\left.1.3 \times 10^{-3}\right)\)

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