Difference between revisions of "Amphoterism" - New World Encyclopedia

Latest revision as of 17:25, 26 July 2023

Water can behave as an acid or a base and is therefore called an amphoteric substance.

The ability of a chemical to behave as both an acid and a base is called amphoterism, and this type of substance is known as an amphoteric substance.^[1] Generally, such a substance acts as an acid in the presence of a base, and it acts as a base in the presence of an acid.

Examples of amphoteric substances include water, amino acids, and proteins. Many metals (such as zinc, tin, lead, aluminum, and beryllium) and most metalloids have amphoteric oxides.

Reactions of some amphoteric substances

The simplest example of an amphoteric substance is water. In the presence of an acid, it behaves as a base (proton acceptor); in the presence of a base, it behaves as an acid (proton donor). In particular, when hydrochloric acid (HCl) is dissolved in water, water acts as a base. The chemical reaction can be written as:

H₂O + HCl → H₃O⁺ + Cl⁻

In its reaction with ammonia (NH₃, a weak base), water acts as an acid, as follows:

H₂O + NH₃ → NH₄⁺ + OH⁻

Furthermore, water molecules can exchange protons with one another. In this case, water behaves as both an acid and a base simultaneously.

2H₂O → H₃O⁺ + OH⁻

Zinc oxide (Zn O) is another amphoteric substance. Its behavior as an acid or base depends on the pH of the solution. In an acidic solution, it reacts as a base; in a basic solution, it reacts as an acid. The chemical reactions can be written as:

ZnO + 2H⁺ → Zn²⁺ + H₂O

ZnO + H₂O + 2OH^- → [Zn(OH)₄]^2-

This property can be used to separate different cations, such as zinc from manganese.

A third example of an amphoteric substance is aluminum hydroxide (Al(OH)₃). It can react with hydrochloric acid or sodium hydroxide (NaOH), represented as follows:

Al(OH)₃ + 3HCl → AlCl₃ + 3H₂O

Al(OH)₃ + NaOH → NaAl(OH)₄

Likewise, beryllium hydroxide (Be(OH)₂) is amphoteric:

Be(OH)₂ + 2HCl → BeCl₂ + 2H₂O

Be(OH)₂ + 2NaOH → Na₂Be(OH)₄

Amphiprotic substances

Many amphoteric substances are also described as amphiprotic—that is, they can donate or accept a proton, thus acting as acids or bases. Water, amino acids, hydrogen carbonate (bicarbonate) ions, and hydrogen sulfate ions are examples of amphiprotic species. Because they can donate a proton, all amphiprotic substances contain a hydrogen atom.

It should be noted that all amphoteric substances are not amphiprotic. For instance, if a substance can accept or donate a pair of electrons, (thus acting as a Lewis acid or base), it would be amphoteric but not amphiprotic.

Reactions of an amphiprotic substance

A common example of an amphiprotic substance is the hydrogen carbonate ion. It can accept a proton, thus acting as a base; or it can donate a proton, thus acting as an acid. Its reactions with water can be written as follows:

HCO₃^- + H₂O → H₂CO₃ + OH^-

HCO₃^- + H₂O → CO₃^2- + H₃O⁺

Notes

↑ According to the Brønsted-Lowry theory of acids and bases, acids are proton donors and bases are proton acceptors. In the Lewis theory of acids and bases, acids are electron pair acceptors and bases are electron pair donors.

References
ISBN links support NWE through referral fees

Brown, Theodore E., H. Eugene LeMay, and Bruce E. Bursten. 2005. Chemistry: The Central Science. 10th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 1110131704
Chang, Raymond. 2006. Chemistry. 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031
McMurry, John, and Robert C. Fay. 2004. Chemistry. 4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080
Moore, John W., Conrad L. Stanitski, and Peter C. Jurs. 2002. Chemistry: The Molecular Science. New York: Harcourt College. ISBN 0030320119
Oxlade, Chris. 2007. Acids and Bases. Chemicals in Action. Oxford: Heinemann Library. ISBN 1432900579

External links

All links retrieved July 26, 2023.

Amphoteric IUPAC Compendium of Chemical Terminology, Electronic version.

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[1] According to the Brønsted-Lowry theory of acids and bases, acids are proton donors and bases are proton acceptors. In the Lewis theory of acids and bases, acids are electron pair acceptors and bases are electron pair donors.

[1]

@@ Line 1: / Line 1: @@
-{{redirect|Amphoteric}}
+{{Copyedited}}{{Paid}}{{Images OK}}{{Submitted}}{{Approved}}
+[[Image:Water drop animation enhanced small.gif|thumb|200px|Water can behave as an acid or a base and is therefore called an amphoteric substance.]]
-In [[chemistry]], an '''amphoteric''' substance is one that can react as either an [[acid]] or [[base (chemistry)|base]].
+The ability of a chemical to behave as both an [[acid]] and a [[base (chemistry)|base]] is called '''amphoterism''', and this type of substance is known as an ''amphoteric'' substance.<ref>According to the Brønsted-Lowry theory of acids and bases, acids are proton donors and bases are proton acceptors. In the Lewis theory of acids and bases, acids are electron pair acceptors and bases are electron pair donors.</ref> Generally, such a substance acts as an acid in the presence of a base, and it acts as a base in the presence of an acid.
+{{toc}}
+Examples of amphoteric substances include [[water]], [[amino acid]]s, and [[protein]]s. Many [[metal]]s (such as [[zinc]], [[tin]], [[lead]], [[aluminum]], and [[beryllium]]) and most [[metalloid]]s have amphoteric [[oxide]]s.
-==Examples==
+== Reactions of some amphoteric substances ==
-Examples include [[amino acid]]s, [[protein]]s, and [[water]]. Many metals (such as [[zinc]], [[tin]], [[lead]], [[aluminium]], and [[beryllium]]) and most [[metalloid]] have amphoteric oxides.
+The simplest example of an amphoteric substance is [[water]]. In the presence of an acid, it behaves as a base (proton acceptor); in the presence of a base, it behaves as an acid (proton donor). In particular, when [[hydrochloric acid]] (HCl) is dissolved in water, water acts as a base. The chemical reaction can be written as:
+:H<sub>2</sub>O + HCl → H<sub>3</sub>O<sup>+</sup> + Cl<sup>−</sup>
-For example, zinc oxide ([[zinc|Zn]][[oxygen|O]]) reacts differently depending on the [[pH]] of the solution:
+In its reaction with [[ammonia]] (NH<sub>3</sub>, a weak base), water acts as an acid, as follows:
+:H<sub>2</sub>O + NH<sub>3</sub> → NH<sub>4</sub><sup>+</sup> + OH<sup>−</sup>
-'''In acids:''' ZnO + 2H<sup>+</sup> → Zn<sup>2+</sup> + H<sub>2</sub>O
+Furthermore, water [[molecule]]s can exchange [[proton]]s with one another. In this case, water behaves as both an acid and a base simultaneously.
+:2H<sub>2</sub>O → H<sub>3</sub>O<sup>+</sup> + OH<sup>−</sup>
-'''In bases:''' ZnO + H<sub>2</sub>O + 2OH<sup>-</sup> → [Zn(OH)<sub>4</sub>]<sup>2-</sup>
+Zinc oxide ([[zinc|Zn]][[oxygen|O]]) is another amphoteric substance. Its behavior as an acid or base depends on the [[pH]] of the solution. In an acidic solution, it reacts as a base; in a basic solution, it reacts as an acid. The chemical reactions can be written as:
+:ZnO + 2H<sup>+</sup> → Zn<sup>2+</sup> + H<sub>2</sub>O
+:ZnO + H<sub>2</sub>O + 2OH<sup>-</sup> → [Zn(OH)<sub>4</sub>]<sup>2-</sup>
+This property can be used to separate different [[cation]]s, such as zinc from [[manganese]].
-This effect can be used to separate different [[cation]]s, such as zinc from [[manganese]].
+A third example of an amphoteric substance is [[aluminum hydroxide]] (Al(OH)<sub>3</sub>). It can react with hydrochloric acid or sodium hydroxide (NaOH), represented as follows:
+:Al(OH)<sub>3</sub> + 3HCl → AlCl<sub>3</sub> + 3H<sub>2</sub>O
+:Al(OH)<sub>3</sub> + NaOH → NaAl(OH)<sub>4</sub>
-There are many other examples of chemical compounds which are also amphoteric, for the simplest example water:
+Likewise, [[beryllium hydroxide]] (Be(OH)<sub>2</sub>) is amphoteric:
+:Be(OH)<sub>2</sub> + 2HCl → BeCl<sub>2</sub> + 2H<sub>2</sub>O
+:Be(OH)<sub>2</sub> + 2NaOH → Na<sub>2</sub>Be(OH)<sub>4</sub>
-'''BASE (Proton Acceptor):''' H<sub>2</sub>O + HCl → H<sub>3</sub>O<sup>+</sup> + Cl<sup>−</sup>
+== Amphiprotic substances ==
-'''ACID (Proton Donor):''' H<sub>2</sub>O + NH<sub>3</sub> → NH<sub>4</sub><sup>+</sup> + OH<sup>−</sup>
+Many amphoteric substances are also described as ''amphiprotic''&mdash;that is, they can donate or accept a [[proton]], thus acting as [[acid]]s or [[Base (chemistry)|base]]s. [[Water]], [[amino acid]]s, [[bicarbonate|hydrogen carbonate]] (bicarbonate) ions, and hydrogen sulfate ions are examples of amphiprotic species. Because they can donate a proton, all amphiprotic substances contain a hydrogen atom.
-:(Indeed, it can do both at once: 2H<sub>2</sub>O → H<sub>3</sub>O<sup>+</sup> + OH<sup>−</sup>)
+It should be noted that all amphoteric substances are not amphiprotic. For instance, if a substance can accept or donate a pair of electrons, (thus acting as a Lewis acid or base), it would be amphoteric but not amphiprotic.
-[[Aluminium hydroxide]] is as well:
+=== Reactions of an amphiprotic substance ===
-'''Acid:''' Al(OH)<sub>3</sub> + 3HCl → AlCl<sub>3</sub> + 3H<sub>2</sub>O
+A common example of an amphiprotic substance is the hydrogen carbonate ion. It can accept a proton, thus acting as a base; or it can donate a proton, thus acting as an acid. Its reactions with water can be written as follows:
+:HCO<sub>3</sub><sup>-</sup> + H<sub>2</sub>O → H<sub>2</sub>CO<sub>3</sub> + OH<sup>-</sup>
+:HCO<sub>3</sub><sup>-</sup> + H<sub>2</sub>O → CO<sub>3</sub><sup>2-</sup> + H<sub>3</sub>O<sup>+</sup>
-'''Base:''' Al(OH)<sub>3</sub> + NaOH → NaAl(OH)<sub>4</sub>
+==See also==
+* [[Acid]]
+* [[Base (chemistry)]]
+* [[Brønsted-Lowry Theory]]
+* [[Oxide]]
+* [[Water]]
+== Notes ==
+<references/>
-[[Beryllium hydroxide]] is also amphoteric:
+==References==
-'''Acid:''' Be(OH)<sub>2</sub> + 2HCl → BeCl<sub>2</sub> + 2H<sub>2</sub>O
+* Brown, Theodore E., H. Eugene LeMay, and Bruce E. Bursten. 2005. ''Chemistry: The Central Science''. 10th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 1110131704
+* Chang, Raymond. 2006. ''Chemistry''. 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031
+* McMurry, John, and Robert C. Fay. 2004. ''Chemistry''. 4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080
+* Moore, John W., Conrad L. Stanitski, and Peter C. Jurs. 2002. ''Chemistry: The Molecular Science''. New York: Harcourt College. ISBN 0030320119
+* Oxlade, Chris. 2007. ''Acids and Bases''. Chemicals in Action. Oxford: Heinemann Library. ISBN 1432900579
-'''Base:''' Be(OH)<sub>2</sub> + 2NaOH → Na<sub>2</sub>Be(OH)<sub>4</sub>
+== External links ==
+All links retrieved July 26, 2023.
-==See also==
+* [http://goldbook.iupac.org/A00306.html Amphoteric] IUPAC Compendium of Chemical Terminology, Electronic version.
-*[[Amphiprotic]]
-[[Category:Chemical properties]]
+[[Category:Physical sciences]]
+[[Category:Chemistry]]
-[[ast:Anfóteru]]
+{{credit2|Amphoterism|108642464|Amphiprotic|100067201}}
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