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Chapter 20: Problem 37

\(\mathrm{Al}_{2} \mathrm{O}_{3}\) is amphoteric. What does this mean?

Short Answer

Expert verified
An amphoteric substance, such as \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (aluminum oxide), is one that can act as both an acid and a base depending on its environment. It can donate protons (H+) when acting as an acid and accept protons (H+) when acting as a base. For example, \(\mathrm{Al}_{2} \mathrm{O}_{3}\) acts as an acid when reacting with Sodium Hydroxide (NaOH) and as a base when reacting with Hydrochloric Acid (HCl).

Step by step solution

01

Definition of Amphoteric

An amphoteric substance has the ability to act as both an acid and a base depending on its environment. It can donate protons (H+) when acting as an acid, or accept protons (H+) when acting as a base. This dual nature exhibited by the compound differentiates it from regular acids or bases.
02

Amphoteric Nature of \(\mathrm{Al}_{2} \mathrm{O}_{3}\)(Aluminum oxide)

Aluminum oxide (\(\mathrm{Al}_{2} \mathrm{O}_{3}\)) is an amphoteric substance. This means that it can act as an acid or a base, depending on what it is reacting with. To better understand, let's see how aluminum oxide demonstrates both acidic and basic properties:
03

Acting as an Acid

When \(\mathrm{Al}_{2} \mathrm{O}_{3}\) reacts with a base, it acts as an acid by donating protons (H+). The reaction of \(\mathrm{Al}_{2} \mathrm{O}_{3}\) with Sodium Hydroxide (NaOH), a strong base, is an example: \[ \mathrm{Al}_{2} \mathrm{O}_{3}(s) + 2\mathrm{NaOH}(aq) + 3\mathrm{H}_{2}\mathrm{O}(l) \rightarrow 2\mathrm{Na}_{3}\mathrm{Al}(\mathrm{OH})^{-}_{4}(aq) \]
04

Acting as a Base

When \(\mathrm{Al}_{2} \mathrm{O}_{3}\) reacts with an acid, it acts as a base by accepting protons (H+). The reaction of \(\mathrm{Al}_{2} \mathrm{O}_{3}\) with Hydrochloric Acid (HCl), a strong acid, is an example: \[ \mathrm{Al}_{2} \mathrm{O}_{3}(s) + 6\mathrm{HCl}(aq) \rightarrow 2\mathrm{AlCl}_{3}(aq) + 3\mathrm{H}_{2}\mathrm{O}(l) \] In both examples, aluminum oxide demonstrates its amphoteric nature by reacting differently with acids and bases. As such, \(\mathrm{Al}_{2} \mathrm{O}_{3}\) is an amphoteric compound.

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Most popular questions from this chapter

There are three known xenon fluoride covalent compounds: $\mathrm{XeF}_{2}, \mathrm{XeF}_{4},\( and \)\mathrm{XeF}_{6} .$ In general, the xenon fluoride compounds must be stored in an inert atmosphere, free of oxygen and water. Why is this the case?

While selenic acid has the formula \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) and thus is directly related to sulfuric acid, telluric acid is best visualized as \(\mathrm{H}_{6} \mathrm{TeO}_{6}\) or \(\mathrm{Te}(\mathrm{OH})_{6}\) a. What is the oxidation state of tellurium in Te(OH) \(_{6} ?\) b. Despite its structural differences with sulfuric and selenic acid, telluric acid is a diprotic acid with \(\mathrm{p} K_{\mathrm{a}_{1}}=7.68\) and \(\mathrm{p} K_{\mathrm{a}_{2}}=11.29 .\) Telluric acid can be prepared by hydrolysis of tellurium hexafluoride according to the equation $$ \mathrm{TeF}_{6}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Te}(\mathrm{OH})_{6}(a q)+6 \mathrm{HF}(a q) $$ Tellurium hexafluoride can be prepared by the reaction of elemental tellurium with fluorine gas: $$ \mathrm{Te}(s)+3 \mathrm{F}_{2}(g) \longrightarrow \mathrm{TeF}_{6}(g) $$ If a cubic block of tellurium (density \(=6.240 \mathrm{g} / \mathrm{cm}^{3} )\) measuring 0.545 \(\mathrm{cm}\) on edge is allowed to react with 2.34 \(\mathrm{L}\) fluorine gas at 1.06 \(\mathrm{atm}\) and \(25^{\circ} \mathrm{C},\) what is the pH of a solution of \(\mathrm{Te}(\mathrm{OH})_{6}\) formed by dissolving the isolated TeF \(_{6}(g)\) in 115 \(\mathrm{mL}\) solution? Assume 100\(\%\) yield in all reactions.

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