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Chapter 13: Problem 106

Write out the stepwise \(K_{\mathrm{a}}\) reactions for citric acid \(\left(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)\) a triprotic acid.

Short Answer

Expert verified
The stepwise $K_{a}$ reactions for citric acid (H3C6H5O7) are as follows: 1. \(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-}(aq)\) 2. \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{HC}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-}(aq) \) 3. \(\mathrm{HC}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{3-}(aq) \)

Step by step solution

01

First Dissociation Reaction

In the first dissociation reaction, citric acid donates its first acidic proton (H+). The equation for this step can be written as follows: \[\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-}(aq)\]
02

Second Dissociation Reaction

In the second dissociation reaction, the resulting ion from the first step, H2C6H5O7-, donates its second acidic proton (H+). The equation for this step can be written as follows: \[ \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{HC}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-}(aq) \]
03

Third Dissociation Reaction

In the third dissociation reaction, the resulting ion from the second step, HC6H5O7²-, donates its third and final acidic proton (H+). The equation for this step can be written as follows: \[ \mathrm{HC}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-}(aq) \rightleftharpoons \mathrm{H}^{+}(aq) + \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{3-}(aq) \]

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of each of the following solutions containing a strong acid in water. a. \(2.0 \times 10^{-2} M \mathrm{HNO}_{3}\) b. \(4.0 \mathrm{M} \mathrm{HNO}_{3}\) c. \(6.2 \times 10^{-12} \mathrm{M} \mathrm{HNO}_{3}\)

What are the major species present in a 0.150-M \(\mathrm{NH}_{3}\) solution? Calculate the \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of this solution.

Calculate the \(\mathrm{pH}\) of an aqueous solution containing \(1.0 \times\) \(10^{-2} M \mathrm{HCl}, 1.0 \times 10^{-2} \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4},\) and \(1.0 \times 10^{-2} \mathrm{M} \mathrm{HCN}\)

Place the species in each of the following groups in order of increasing acid strength. a. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{H}_{2} \mathrm{S}, \mathrm{H}_{2} \mathrm{Se}\) (bond energies: \(\mathrm{H}-\mathrm{O}, 467 \mathrm{kJ} / \mathrm{mol}\); \(\mathrm{H}-\mathrm{S}, 363 \mathrm{kJ} / \mathrm{mol} ; \mathrm{H}-\mathrm{Se}, 276 \mathrm{kJ} / \mathrm{mol})\) b. \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}, \mathrm{FCH}_{2} \mathrm{CO}_{2} \mathrm{H}, \mathrm{F}_{2} \mathrm{CHCO}_{2} \mathrm{H}, \mathrm{F}_{3} \mathrm{CCO}_{2} \mathrm{H}\) c. \(\mathrm{NH}_{4}^{+}, \mathrm{HONH}_{3}^{+}\) d. \(\mathrm{NH}_{4}^{+}, \mathrm{PH}_{4}^{+}\) (bond energies: \(\mathrm{N}-\mathrm{H}, 391 \mathrm{kJ} / \mathrm{mol} ; \mathrm{P}-\mathrm{H}\) \(322 \mathrm{kJ} / \mathrm{mol})\) Give reasons for the orders you chose.

What are the major species present in 0.250 \(M\) solutions of each of the following acids? Calculate the \(\mathrm{pH}\) of each of these solutions. a. \(\mathrm{HClO}_{4}\) b. HNO_3
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