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Chapter 14: 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 ionization reactions of citric acid (H3C6H5O7) are as follows: 1. \[ \mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7} \rightleftharpoons \mathrm{H}^{+} + \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-} \] 2. \[ \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-} \rightleftharpoons \mathrm{H}^{+} + \mathrm{H}_{\mathrm{C}}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-} \] 3. \[ \mathrm{H}_{\mathrm{C}}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-} \rightleftharpoons \mathrm{H}^{+} + \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{3-} \]

Step by step solution

01

Write the first ionization reaction

The first ionization reaction is the process of citric acid losing one of its acidic protons (H+) and forming the first anion. The reaction is as follows: \[ \mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7} \rightleftharpoons \mathrm{H}^{+} + \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-} \]
02

Write the second ionization reaction

The second ionization reaction involves the first anion (formed in step 1) losing another acidic proton (H+) and forming the second anion. The reaction is as follows: \[ \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{-} \rightleftharpoons \mathrm{H}^{+} + \mathrm{H}_{\mathrm{C}}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-} \]
03

Write the third ionization reaction

The third ionization reaction involves the second anion (formed in step 2) losing its last acidic proton (H+) and forming the third anion. The reaction is as follows: \[ \mathrm{H}_{\mathrm{C}}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{2-} \rightleftharpoons \mathrm{H}^{+} + \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{3-} \] Now we have completed the stepwise reactions for the ionization of citric acid.

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Most popular questions from this chapter

Zinc hydroxide is an amphoteric substance. Write equations that describe \(\mathrm{Zn}(\mathrm{OH})_{2}\) acting as a Bronsted-Lowry base toward \(\mathrm{H}^{+}\) and as a Lewis acid toward \(\mathrm{OH}^{-} .\)

Which of the following represent conjugate acid-base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair. a. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}^{-}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) d. $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}$

Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced equations for the reactions causing the solution to be acidic or basic. The relevant \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values are found in Tables 14.2 and \(14.3 .\) $\begin{array}{ll}{\text { a. } \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}} & {\text { d. } \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{ClO}_{2}} \\ {\text { b. } \mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}} & {\text { e. } \mathrm{NH}_{4} \mathrm{F}} \\ {\text { c. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{O} \mathrm{l}} & {\text { f. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{CN}}\end{array}$

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

Trichloroacetic acid $\left(\mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}\right)$ is a corrosive acid that is used to precipitate proteins. The pH of a \(0.050-M\) solution of trichloroacetic acid is the same as the pH of a \(0.040-M \mathrm{HClO}_{4}\) solution. Calculate \(K_{\mathrm{a}}\) for trichloroacetic acid.
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