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Chapter 14: Problem 39

Write balanced equations that describe the following reactions. a. the dissociation of perchloric acid in water b. the dissociation of propanoic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}\right)\) in water c. the dissociation of ammonium ion in water

Short Answer

Expert verified
a. \( \mathrm{HClO}_{4}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{ClO}_{4}^{-}(aq) \) b. \( \mathrm{CH}_{3}\mathrm{CH}_{2}\mathrm{CO}_{2}\mathrm{H}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}(aq) \) c. \( \mathrm{NH}_{4}^{+}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{NH}_{3}(aq) \)

Step by step solution

01

Identify reactants and products

Perchloric acid (HClO4) dissociates in water to produce hydrogen ions (H+) and perchlorate ions (ClO4-). The water molecule will act as a solvent but does not participate directly in the reaction. Reactants: HClO4 Products: H+ ions and ClO4- ions Step 2: Write the balanced equation
02

Write the balanced equation

\( \mathrm{HClO}_{4}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{ClO}_{4}^{-}(aq) \) The above equation is already balanced. #b. Dissociation of propanoic acid (CH3CH2CO2H) in water#
03

Identify reactants and products

Propanoic acid (CH3CH2CO2H) dissociates in water to produce hydrogen ions (H+) and propanoate ions (CH3CH2CO2-). The water molecule will act as a solvent but does not participate directly in the reaction. Reactants: CH3CH2CO2H Products: H+ ions and CH3CH2CO2- ions
04

Write the balanced equation

\( \mathrm{CH}_{3}\mathrm{CH}_{2}\mathrm{CO}_{2}\mathrm{H}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}(aq) \) The above equation is already balanced. #c. Dissociation of ammonium ion in water#
05

Identify reactants and products

Ammonium ion (NH4+) dissociates in water to produce hydrogen ions (H+) and ammonia molecules (NH3). The water molecule will act as a solvent but does not participate directly in the reaction. Reactants: NH4+ ions Products: H+ ions and NH3 molecules
06

Write the balanced equation

\( \mathrm{NH}_{4}^{+}(aq) \rightarrow \mathrm{H}^{+}(aq) + \mathrm{NH}_{3}(aq) \) The above equation is already balanced.

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Most popular questions from this chapter

Using your results from Exercise \(133,\) place the species in each of the following groups in order of increasing base strength. a. \(\mathrm{OH}^{-}, \mathrm{SH}^{-}, \mathrm{SeH}^{-}\) b. \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\) c. \(\mathrm{NH}_{3}, \mathrm{HONH}_{2}\)

a. The principal equilibrium in a solution of \(\mathrm{NaHCO}_{3}\) is $$ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between \(\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right]\) and \(\left[\mathrm{CO}_{3}^{2-}\right] ?\) c. Using the equilibrium $$ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons 2 \mathrm{H}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ derive an expression for the pH of the solution in terms of \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) using the result from part b. d. What is the pH of a solution of \(\mathrm{NaHCO}_{3} ?\)

Monochloroacetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{2} \mathrm{ClO}_{2},\) is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of \(K_{\mathrm{a}}\) for monochloroacetic acid is \(1.35 \times 10^{-3}\) Calculate the pH of a \(0.10-M\) solution of monochloroacetic acid.

A \(0.20-M\) sodium chlorobenzoate \(\left(\mathrm{NaC}_{7} \mathrm{H}_{4} \mathrm{ClO}_{2}\right)\) solution has \(\mathrm{a} \mathrm{pH}\) of \(8.65 .\) Calculate the \(\mathrm{pH}\) of a \(0.20-M\) chlorobenzoic acid \(\left(\mathrm{HC}_{7} \mathrm{H}_{4} \mathrm{ClO}_{2}\right)\) solution.

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 \(14.3 .\) \(\begin{array}{ll}{\text { a. } \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}} & {\text { d. } \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{ClO}_{2}} \\ {\text { b. } \mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}} & {\text { e. } \mathrm{NH}_{4} \mathrm{F}} \\ {\text { c. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{O} \mathrm{l}} & {\text { f. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{CN}}\end{array}\)
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