Name: acid and base strength in water
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Acid/Base Strengths and Dissociation Constants

Gli acidi e le basi possono essere classificati in base al fatto che siano un acido forte, una base forte, un acido debole, o una base debole. Ci sono pochissimi acidi e basi forti, pertanto la maggior parte degli acidi e delle basi sono deboli. Un acido forte, come l'acido cloridrico, si dissocia completamente in ioni idrogeno e ioni cloruro quando disciolto in acqua.

Una base forte, come l'idrossido di sodio, si dissocia completamente in ioni sodio e ioni idrossido. Gli acidi e le basi deboli si dissociano parzialmente e sono presenti sia in forma ionizzata, che non ionizzata. Per esempio, sia l'acido acetico che la sua base coniugata debole, l'acetato, si trovano in una soluzione acquosa.

Il grado di dissociazione di un acido o di una base debole può essere misurato usando la sua costante di equilibrio. La costante di equilibrio per gli acidi deboli ha un nome speciale:la costante di dissociazione acida, o Ka.Per un generico HA acido debole, Ka a una data temperatura può essere calcolato da un'equazione di equilibrio:dividendo la concentrazione di prodotti, ione A e ione idronio, per la concentrazione di reagenti, HA e acqua. Poiché l'acqua è liquida e la sua concentrazione rimane pressoché invariata nella reazione, viene esclusa dall'equazione.

Più alto è il Ka, più forte è l'acido. L'acido nitroso è più forte dell'acido acetico, perché il Ka dell'acido nitroso è superiore del Ka dell'acido acetico. La costante di equilibrio per le basi deboli, la costante di dissociazione di base, o Kb, agisce in modo simile a Ka.Per una base debole generica B, Kb a una data temperatura può essere determinata dividendo la concentrazione dei prodotti, ione BH e ione idrossido, per la concentrazione del reagente, B.Come gli acidi, anche la forza delle basi è direttamente proporzionale alla Kb.Per esempio, l'etilammina è relativamente più forte dell'urea, perché il Kb dell'etilammina è maggiore del Kb dell'urea.

La forza di un acido può anche essere espressa in termini di ionizzazione percentuale. La percentuale di ionizzazione dell'acido può essere calcolata dividendo la concentrazione di ioni idronio in equilibrio per la concentrazione iniziale di acido, e moltiplicandola per cento. Allo stesso modo, la ionizzazione percentuale per le basi, può essere calcolata dividendo la concentrazione di ioni idrossido all'equilibrio per la concentrazione iniziale di base e moltiplicandola per cento.

Maggiore è la percentuale di ionizzazione, più forte è l'acido o la base.

forze acido/base e costanti di dissociazione

La forza relativa di un acido o di una base è la misurazione in cui si ionizza quando disciolto in acqua. Se la reazione di ionizzazione è sostanzialmente completa, l'acido o la base sono detti forti; se si verifica una ionizzazione relativamente scarsa, l'acido o la base sono deboli. Gli acidi e le basi deboli sono molti di più di quelli forti. Gli acidi e le basi forti più comuni sono elencati di seguito:

<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Strong Acids</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Strong Bases</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">HClO4</td>
			<td style="color: black; border: 1px solid black; text-align: center;">LiOH</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">HCl</td>
			<td style="color: black; border: 1px solid black; text-align: center;">NaOH</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">HBr</td>
			<td style="color: black; border: 1px solid black; text-align: center;">KOH</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">HI</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ca(OH)2</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">HNO3</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Sr(OH)2</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">H2SO4</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Ba(OH)2</td>
		</tr>
	</tbody>
</table>

Le forze relative degli acidi possono essere quantificate misurando le loro costanti di equilibrio in soluzioni acquose. Nelle soluzioni della stessa concentrazione, gli acidi più forti ionizzano in misura maggiore e quindi producono concentrazioni più elevate di ioni idronio rispetto agli acidi più deboli. La costante di equilibrio di un acido è chiamata costante di ionizzazione acida, Ka. Per la reazione di un acido HA:

<img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />

la costante di ionizzazione acida è scritta come

<img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />

dove le concentrazioni sono quelle all’equilibrio. Sebbene l'acqua sia un reagente nella reazione, è anche il solvente, quindi non includiamo [H2O] nell'equazione. Maggiore è la Ka di un acido, maggiore è la concentrazione di H_3O^+ e A^− rispetto alla concentrazione dell'acido non ionizzato, HA, in una miscela in equilibrio, e più forte è l'acido. Un acido è classificato come “forte” quando subisce una ionizzazione completa, nel qual caso la concentrazione di HA è zero e la costante di ionizzazione dell’acido è incommensurabilmente grande (K_a ≈ ∞). Gli acidi parzialmente ionizzati sono detti “deboli” e le loro costanti di ionizzazione acida possono essere misurate sperimentalmente.

Per illustrare questa idea, di seguito sono mostrate tre equazioni di ionizzazione acida e valori di K_a. Le costanti di ionizzazione aumentano dalla prima all'ultima delle equazioni elencate, indicando che la forza relativa dell'acido aumenta nell'ordine CH_3CO_2H < HNO_2 < HSO_4−.

<img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />

Un'altra misurazione della forza di un acido è la sua percentuale di ionizzazione. La percentuale di ionizzazione di un acido debole è definita in termini di composizione di una miscela in equilibrio:

<img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />

dove il numeratore è equivalente alla concentrazione della base coniugata dell'acido (per stechiometria, [A^−] = [H_3O^+]). A differenza del valore K_a, la percentuale di ionizzazione di un acido debole varia con la concentrazione iniziale dell'acido, tipicamente diminuendo all'aumentare della concentrazione.

Proprio come per gli acidi, la forza relativa di una base si riflette nell'entità della sua costante di ionizzazione della base (K_b) nelle soluzioni acquose. Nelle soluzioni della stessa concentrazione, le basi più forti si ionizzano in misura maggiore e quindi producono concentrazioni di ioni idrossido più elevate rispetto alle basi più deboli. Una base più forte ha una costante di ionizzazione maggiore rispetto a una base più debole. Per la reazione di una base, B:

<img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />

la costante di ionizzazione è scritta come

<img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />

L'ispezione dei dati per tre basi deboli presentate di seguito mostra che la forza della base aumenta nell'ordine NO_2− < CH_2 CO_2− < NH_3.

<img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />

Come per gli acidi, la forza relativa di una base si riflette anche nella sua percentuale di ionizzazione, calcolata come

<img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />

ma varierà a seconda della costante di ionizzazione della base e della concentrazione iniziale della soluzione.

Questo testo è adattato da <a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases">Openstax, Chemistry 2e, Section 14.3: Relative Strengths of Acids and Bases.</a>

Forze acido/base e costanti di dissociazione

La forza relativa di un acido o di una base è la misura in cui ionizza quando viene disciolto in acqua. Se la reazione di ionizzazione è sostanzialmente completa, ...

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acid and base strength in water

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.

Acid strength can be measured with the acid-ionization constant, Ka. For an acid HA in water, Ka compares the concentrations of the products and the nonionized acid at equilibrium. Water is a reactant in the reaction, but it is not included in the equation because it is the solvent. A larger Ka means more H3O+ and A− relative to HA, so the acid is stronger.

A strong acid is considered completely ionized. In that case, the concentration of HA is zero, and Ka is immeasurably large, or approximately infinite. Weak acids ionize only partially, so their Ka values can be measured in the lab. The relative acid strengths in the examples increase in the order CH3CO2H &lt; HNO2 &lt; HSO4−.

Percent ionization is another way to describe weak acid strength. It is based on the amount of acid that ionizes at equilibrium. For a weak acid, the percent ionization changes with the starting concentration and usually gets smaller as the concentration gets higher. This makes percent ionization different from Ka.

Base strength is measured in a similar way with the base-ionization constant, Kb. For a base B in water, a larger Kb means the base ionizes more and produces a higher hydroxide ion concentration. A stronger base has a larger ionization constant than a weaker base.

The examples of weak bases show the strength order NO2− &lt; CH2CO2− &lt; NH3. Base strength can also be described with percent ionization. As with weak acids, this value depends on both the base-ionization constant and the initial concentration of the solution.

Acid and Base Strength in Water

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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 acid and base strength in water depends on ionization, Ka, Kb, and percent ionization, with examples of strong and weak acids and bases.

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Acid and Base Strength in Water

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