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Chapter 13: Problem 139

Aluminum hydroxide is an amphoteric substance. It can act as either a Brönsted-Lowry base or a Lewis acid. Write a reaction showing Al(OH) \(_{3}\) acting as a base toward \(\mathrm{H}^{+}\) and as an acid toward OH \(^{-}\)

Short Answer

Expert verified
As a Brönsted-Lowry base, aluminum hydroxide, Al(OH)\(_{3}\), accepts a proton (H\(^{+}\)) in the reaction: \[ Al(OH)_{3} + H^{+} \to Al(OH)_{4}^{-} \] As a Lewis acid, aluminum hydroxide, Al(OH)\(_{3}\), accepts an electron pair from the OH\(^{-}\) ions in the reaction: \[ Al(OH)_{3} + OH^{-} \to Al(OH)_{4}^{-} \]

Step by step solution

01

Brönsted-Lowry base

A Brönsted-Lowry base is a substance that can accept a proton (H\(^{+}\)). In this reaction, aluminum hydroxide, Al(OH)\(_{3}\) will act as a base by accepting a proton from the H\(^{+}\) ions. As a result, there will be an increase in hydroxide ions (OH\(^{-}\)) in the molecule. Reaction: Al(OH)\(_{3}\) + H\(^{+}\) → Al(OH)\(_{4}^{-}\)
02

Lewis acid

A Lewis acid is a substance that can accept an electron pair. In this reaction, aluminum hydroxide, Al(OH)\(_{3}\) will act as an acid by accepting an electron pair from the OH\(^{-}\) ions. As a result, there will be a change in the molecule's structure and charge distribution. Reaction: Al(OH)\(_{3}\) + OH\(^{-}\) → Al(OH)\(_{4}^{-}\)

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Most popular questions from this chapter

Hemoglobin (abbreviated Hb) is a protein that is responsible for the transport of oxygen in the blood of mammals. Each hemoglobin molecule contains four iron atoms that are the binding sites for \(\mathrm{O}_{2}\) molecules. The oxygen binding is \(\mathrm{pH}\) dependent. The relevant equilibrium reaction is $$\mathrm{HbH}_{4}^{4+}(a q)+4 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}(a q)+4 \mathrm{H}^{+}(a q)$$ Use Le Châtelier's principle to answer the following. a. What form of hemoglobin, \(\mathrm{HbH}_{4}^{4+}\) or \(\mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4},\) is favored in the lungs? What form is favored in the cells? b. When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in the blood is decreased. How does this affect the oxygenbinding equilibrium? How does breathing into a paper bag help to counteract this effect? (See Exercise 146.) c. When a person has suffered a cardiac arrest, injection of a sodium bicarbonate solution is given. Why is this necessary? (Hint: \(\mathrm{CO}_{2}\) blood levels increase during cardiac arrest.

You have \(100.0 \mathrm{g}\) saccharin, a sugar substitute, and you want to prepare a \(\mathrm{pH}=5.75\) solution. What volume of solution can be prepared? For saccharin, \(\mathrm{HC}_{7} \mathrm{H}_{4} \mathrm{NSO}_{3}, \mathrm{p} K_{\mathrm{a}}=11.70\) \(\left(p K_{a}=-\log K_{a}\right)\)

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. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation $$2 \mathrm{NaOCN}(s)+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s) \longrightarrow 2 \mathrm{HNCO}(l)+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s)$$ Upon isolating pure HNCO(I), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the \(\mathrm{pH}\) of a \(100 .\) -mL solution of HNCO prepared from the reaction of \(10.0 \mathrm{g}\) each of \(\mathrm{NaOCN}\) and \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) assuming all of the HNCO produced is dissolved in solution? \((K_{\mathrm{a}}\) of HNCO \(\left.=1.2 \times 10^{-4} .\right)\)

A typical sample of vinegar has a pH of \(3.0 .\) Assuming that vinegar is only an aqueous solution of acetic acid \(\left(K_{a}=1.8 \times\right.\) \(10^{-5}\) ), calculate the concentration of acetic acid in vinegar.
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