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Chapter 14: Problem 38

For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and the conjugate acid. a. \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\) b. \(\mathrm{H}_{2} \mathrm{O}+\mathrm{HONH}_{3}^{+} \rightleftharpoons \mathrm{HONH}_{2}+\mathrm{H}_{3} \mathrm{O}^{+}\) c. \(\mathrm{HOCl}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} \rightleftharpoons \mathrm{OCl}^{-}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\)

Short Answer

Expert verified
For each reaction: a. Acid: \(\mathrm{Al}(\mathrm{H}_{2}\mathrm{O})_{6}^{3+}\); Base: \(\mathrm{H}_{2}\mathrm{O}\); Conjugate Acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\); Conjugate Base: \(\mathrm{Al}(\mathrm{H}_{2}\mathrm{O})_{5}(\mathrm{OH})^{2+}\) b. Acid: \(\mathrm{HONH}_{3}^{+}\); Base: \(\mathrm{H}_{2}\mathrm{O}\); Conjugate Acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\); Conjugate Base: \(\mathrm{HONH}_{2}\) c. Acid: \(\mathrm{HOCl}\); Base: \(\mathrm{C}_{6}\mathrm{H}_{5}\mathrm{NH}_{2}\); Conjugate Acid: \(\mathrm{C}_{6}\mathrm{H}_{5}\mathrm{NH}_{3}^{+}\); Conjugate Base: \(\mathrm{OCl}^{-}\)

Step by step solution

01

In the given reaction, \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) donates a proton (H+) to \(\mathrm{H}_{2} \mathrm{O}\). Therefore, the acid is \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\). #Step 2: Identify the base#

In the given reaction, \(\mathrm{H}_{2}\mathrm{O}\) accepts a proton (H+) from \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\). Therefore, the base is \(\mathrm{H}_{2}\mathrm{O}\). #Step 3: Identify the conjugate acid#
02

In the given reaction, \(\mathrm{H}_{2}\mathrm{O}\) gains a proton (H+) and forms \(\mathrm{H}_{3}\mathrm{O}^{+}\). Therefore, the conjugate acid is \(\mathrm{H}_{3}\mathrm{O}^{+}\). #Step 4: Identify the conjugate base#

In the given reaction, \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) loses a proton (H+) and forms \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\). Therefore, the conjugate base is \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}\). b. \(\mathrm{H}_{2} \mathrm{O}+\mathrm{HONH}_{3}^{+} \rightleftharpoons \mathrm{HONH}_{2}+\mathrm{H}_{3} \mathrm{O}^{+}\) #Step 1: Identify the acid#
03

In the given reaction, \(\mathrm{HONH}_{3}^{+}\) donates a proton (H+) to \(\mathrm{H}_{2}\mathrm{O}\). Therefore, the acid is \(\mathrm{HONH}_{3}^{+}\). #Step 2: Identify the base#

In the given reaction, \(\mathrm{H}_{2}\mathrm{O}\) accepts a proton (H+) from \(\mathrm{HONH}_{3}^{+}\). Therefore, the base is \(\mathrm{H}_{2}\mathrm{O}\). #Step 3: Identify the conjugate acid#
04

In the given reaction, \(\mathrm{H}_{2}\mathrm{O}\) gains a proton (H+) and forms \(\mathrm{H}_{3}\mathrm{O}^{+}\). Therefore, the conjugate acid is \(\mathrm{H}_{3}\mathrm{O}^{+}\). #Step 4: Identify the conjugate base#

In the given reaction, \(\mathrm{HONH}_{3}^{+}\) loses a proton (H+) and forms \(\mathrm{HONH}_{2}\). Therefore, the conjugate base is \(\mathrm{HONH}_{2}\). c. \(\mathrm{HOCl}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} \rightleftharpoons \mathrm{OCl}^{-}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\) #Step 1: Identify the acid#
05

In the given reaction, \(\mathrm{HOCl}\) donates a proton (H+) to \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\). Therefore, the acid is \(\mathrm{HOCl}\). #Step 2: Identify the base#

In the given reaction, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) accepts a proton (H+) from \(\mathrm{HOCl}\). Therefore, the base is \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\). #Step 3: Identify the conjugate acid#
06

In the given reaction, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) gains a proton (H+) and forms \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\). Therefore, the conjugate acid is \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\). #Step 4: Identify the conjugate base#

In the given reaction, \(\mathrm{HOCl}\) loses a proton (H+) and forms \(\mathrm{OCl}^{-}\). Therefore, the conjugate base is \(\mathrm{OCl}^{-}\).

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Most popular questions from this chapter

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{B}(\mathrm{OH})_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-}(a q)+\mathrm{H}^{+}(a q)\) b. \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) c. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

What mass of \(\mathrm{NaOH}(s)\) must be added to \(1.0 \mathrm{~L}\) of \(0.050 \mathrm{M}\) \(\mathrm{NH}_{3}\) to ensure that the percent ionization of \(\mathrm{NH}_{3}\) is no greater than \(0.0010 \%\) ? Assume no volume change on addition of \(\mathrm{NaOH}\)

A solution is made by adding \(50.0 \mathrm{~mL}\) of \(0.200 M\) acetic acid \(\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)\) to \(50.0 \mathrm{~mL}\) of \(1.00 \times 10^{-3} \mathrm{M} \mathrm{HCl}\) a. Calculate the \(\mathrm{pH}\) of the solution. b. Calculate the acetate ion concentration.

A sample containing \(0.0500\) mole of \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) is dissolved in enough water to make \(1.00 \mathrm{~L}\) of solution. This solution contains hydrated \(\mathrm{SO}_{4}{ }^{2-}\) and \(\mathrm{Fe}^{3+}\) ions. The latter behaves as an acid: $$\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}^{2+}(a q)+\mathrm{H}^{+}(a q)$$ a. Calculate the expected osmotic pressure of this solution at \(25^{\circ} \mathrm{C}\) if the above dissociation is negligible. b. The actual osmotic pressure of the solution is \(6.73\) atm at \(25^{\circ} \mathrm{C}\). Calculate \(K_{\mathrm{a}}\) for the dissociation reaction of \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}{ }^{3+}\). (To do this calculation, you must assume that none of the ions go through the semipermeable membrane. Actually, this is not a great assumption for the tiny \(\mathrm{H}^{+}\) ion.)

What are the major species present in the following mixtures of bases? a. \(0.050 \mathrm{M} \mathrm{NaOH}\) and \(0.050 \mathrm{M} \mathrm{LiOH}\) b. \(0.0010 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) and \(0.020 \mathrm{M} \mathrm{RbOH}\) What is \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of each of these solutions?
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