Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 30 s
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Water: A Bronsted-Lowry Acid and Base

Una molecola anfotera è in grado di agire sia come acido, che come base. L'acqua è un esempio di una molecola anfotera. In una soluzione acquosa di ammoniaca, l'acqua può agire come un acido donando un protone all'ammoniaca, una base.

Al contrario, l'acqua agisce come base in una soluzione acquosa di acido cloridrico, accettando un protone dall'acido. Poiché è anfotera, l'acqua può subire l'autoionizzazione. In questo processo, una molecola d'acqua agisce come acido, donando un protone ad un'altra molecola d'acqua che agisce da base, accettando quel protone.

Ciò si traduce nella produzione di uno ione idronio e di uno ione idrossido. La costante di equilibrio per l'autoionizzazione dell'acqua, Kᴡ, nota anche come costante del prodotto ionico per l'acqua, può essere espressa come Kᴡ e ha un valore di 1 10⁻¹⁴. La sua espressione di equilibrio è scritta come la concentrazione degli ioni idronio moltiplicata per la concentrazione degli ioni idrossido, senza denominatore poiché ambo i reagenti sono liquidi.

In acqua pura a 25 gradi Celsius, le concentrazioni di idronio e ioni idrossido sono uguali ossia 1 10⁻⁷ M.Kᴡ può essere utilizzato per calcolare la concentrazione di idronio e di ioni idrossido in una soluzione, e per determinare se una soluzione è acida o basica. Se una soluzione è acida, la concentrazione di ioni idronio sarà superiore a quella degli ioni idrossido. Al contrario, se una soluzione è basica, la concentrazione di ioni idrossido sarà maggiore degli ioni idronio.

Se la concentrazione di ioni idronio in soluzione è 5 10⁻⁷ M, la concentrazione di ioni idrossido può essere determinata usando Kᴡ.Poiché i valori di Kᴡ e ioni idronio sono noti, la concentrazione degli ioni idrossido può essere calcolata pari a 2 10⁻⁸ M.Poiché la concentrazione degli ioni idronio, 5 10⁻⁷ M, è superiore alla concentrazione degli ioni idrossido, 2 10⁻⁸ M, la soluzione è acida.

acqua: un acido e una base di bronsted-lowry

La reazione tra un acido di Brønsted-Lowry e l'acqua è chiamata ionizzazione acida. Ad esempio, quando il fluoruro di idrogeno si dissolve in acqua e si ionizza, i protoni vengono trasferiti dalle molecole di fluoruro di idrogeno alle molecole di acqua, producendo ioni idronio e ioni fluoruro:

 <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />

La ionizzazione delle basi di una specie avviene quando accetta protoni dalle molecole d'acqua. Nell'esempio seguente, le molecole di piridina, C_5NH_5, subiscono la ionizzazione della base quando disciolte in acqua, producendo ioni idrossido e piridinio:

 <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />

Le precedenti reazioni di ionizzazione suggeriscono che l'acqua può funzionare sia come base (come nella sua reazione con acido fluoridrico) sia come acido (come nella sua reazione con l'ammoniaca). Le specie capaci sia di donare che di accettare protoni sono chiamate anfiprotiche, o più in generale, anfotere, termine che può essere utilizzato per acidi e basi per definizioni diverse da quella di Brønsted-Lowry. Le equazioni seguenti mostrano le due possibili reazioni acido-base per due specie anfiprotiche, ione bicarbonato e acqua:

 <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />

La prima equazione rappresenta la reazione del bicarbonato come acido con l'acqua come base, mentre la seconda rappresenta la reazione del bicarbonato come base con l'acqua come acido. Quando si aggiunge bicarbonato all'acqua, entrambi questi equilibri vengono stabiliti contemporaneamente e la composizione della soluzione risultante può essere determinata attraverso opportuni calcoli di equilibrio. Allo stato liquido, le molecole di una sostanza anfiprotica possono reagire tra loro come illustrato per l'acqua nelle equazioni seguenti:

 <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />

Il processo in cui molecole simili reagiscono per produrre ioni è chiamato autoionizzazione. L'acqua liquida subisce un'autoionizzazione in misura molto lieve; a 25 °C, circa due molecole d'acqua su un miliardo sono ionizzate. L'entità del processo di autoionizzazione dell'acqua si riflette nel valore della sua costante di equilibrio, la costante del prodotto ionico per l'acqua, K_W:

 <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />

La leggera ionizzazione dell'acqua pura si riflette nel piccolo valore della costante di equilibrio; a 25 °C, K_W ha un valore di 1,0 × 10^−14.

 <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />

Il processo è endotermico, quindi l'entità della ionizzazione e le risultanti concentrazioni di ioni idronio e ioni idrossido aumentano con la temperatura. Ad esempio, a 100 °C, il valore di K_W è circa 5,6 × 10^−13, circa 50 volte maggiore del valore a 25 °C.

L'autoionizzazione dell'acqua produce lo stesso numero di ioni idronio e idrossido. Pertanto, in acqua pura a 25 °C:

 <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />

Le concentrazioni di questi ioni in una soluzione sono spesso determinanti critici delle proprietà della soluzione e dei comportamenti chimici degli altri soluti, ed è stato sviluppato un vocabolario specifico per descrivere queste concentrazioni in termini relativi. Una soluzione è neutra se contiene uguali concentrazioni di ioni idronio e idrossido; acido se contiene una concentrazione maggiore di ioni idronio rispetto agli ioni idrossido; e basico se contiene una concentrazione minore di ioni idronio rispetto agli ioni idrossido.

Riepilogo delle relazioni per soluzioni acide, basiche e neutre

<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Classification</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Relative Ion Concentrations</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH at 25 °C</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">acidic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] > [OH−]</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH < 7</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">neutral</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] = [OH−]</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH = 7</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">basic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] < [OH−]</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH > 7</td>
		</tr>
	</tbody>
</table>

Questo testo è adattato da <a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chemistry 2e, Section 14.1: Brønsted-Lowry Acids and Bases</a>, and <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Section 14.2: pH and pOH</a>

Acqua: un acido e una base di Bronsted-Lowry

La reazione tra un acido di Brønsted-Lowry e l'acqua è chiamata ionizzazione acida. Ad esempio, quando il fluoruro di idrogeno si dissolve in acqua e si ionizza, ...

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water as an amphiprotic substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions.

Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions.

These reactions show that water can play either role. A substance that can donate or accept protons is called amphiprotic. The broader term amphoteric is also used for substances that can act as acids or bases under different definitions. Bicarbonate ion is another amphiprotic species. It can react with water as an acid or as a base, and both equilibria can be present at the same time in solution.

Liquid water can also react with itself. This process is called autoionization. It happens only to a very small extent. At 25 °C, about two out of every billion water molecules are ionized. The equilibrium constant for this process is the ion-product constant for water, K_w, and its value is 1.0 × 10^-14 at 25 °C.

Autoionization is endothermic, so more ionization occurs as temperature rises. At 100 °C, K_w is about 5.6 × 10^-13, which is roughly 50 times larger than at 25 °C. Pure water always produces equal amounts of hydronium and hydroxide ions through this process. A solution is neutral when these ion concentrations are equal. It is acidic when hydronium ion concentration is greater than hydroxide ion concentration, and basic when hydroxide ion concentration is greater. At 25 °C, acidic solutions have pH below 7, neutral solutions have pH 7, and basic solutions have pH above 7.

Water as an Amphiprotic Substance

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Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

water: a bronsted-lowry acid and base

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

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Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

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Learn how water can act as both an acid and a base, why it is amphiprotic, and how autoionization affects hydronium, hydroxide, and pH.

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Water as an Amphiprotic Substance

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