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

Los ácidos y las bases se pueden clasificar según sean un ácido fuerte, una base fuerte, un ácido débil o una base débil. Hay muy pocos ácidos y bases fuertes, por lo que la mayoría de los ácidos y bases son débiles. Un ácido fuerte, como el ácido clorhídrico, se disocia completamente en iones de hidrógeno y en iones de cloruro cuando se disuelve en agua.Una base fuerte, como el hidróxido de sodio, se disocia completamente en iones de sodio y en iones de hidróxido. Los ácidos y bases débiles se disocian parcialmente y están presentes tanto en formas ionizadas como no ionizadas. Por ejemplo, tanto el ácido acético como su base conjugada débil, el acetato, se encuentran en una solución acuosa.El grado de disociación de un ácido o base débil se puede medir usando su constante de equilibrio. La constante de equilibrio para los ácidos débiles tiene un nombre especial, la constante de disociación ácida, o Ka.Para un ácido débil genérico HA, la Ka a una temperatura dada se puede calcular mediante una ecuación de equilibrio:dividiendo la concentración de productos, el ion A y el ion de hidronio, por la concentración de reactivos, HA y agua. Como el agua es líquida y su concentración permanece casi sin cambios en la reacción, se excluye de la ecuación.Cuanto mayor sea la Ka, más fuerte será el ácido. El ácido nitroso es más fuerte que el ácido acético porque la Ka del ácido nitroso es mayor que la Ka del ácido acético. La constante de equilibrio para bases débiles, la constante de disociación de las bases, o Kb, actúa de manera similar a Ka.Para una base débil genérica B, se puede determinar Kb a una temperatura dada dividiendo la concentración de productos, el ion BH y el ion de hidróxido, por la concentración de reactivo, B.Al igual que los ácidos, la fuerza de las bases también es directamente proporcional al Kb.Por ejemplo, la etilamina es relativamente más fuerte que la urea porque el Kb de la etilamina es mayor que el Kb de la urea.La fuerza de un ácido también se puede expresar en términos de porcentaje de ionización. El porcentaje de ionización del ácido se puede calcular dividiendo la concentración de iones de hidronio en equilibrio por la concentración de ácido inicial y multiplicándola por cien. De manera similar, el porcentaje de ionización de las bases se puede calcular dividiendo la concentración de iones de hidróxido en equilibrio por la concentración inicial de base y multiplicándola por cien.Cuanto mayor sea el porcentaje de ionización, más fuerte será el ácido o la base.

fuerzas de Ácidos/bases y constantes de disociación

La fuerza relativa de un ácido o una base es el grado en que este se ioniza cuando se disuelve en agua. Si la reacción de ionización es esencialmente completa, el ácido o la base se denomina fuerte; si ocurre relativamente poca ionización, el ácido o la base es débil. Hay muchos más ácidos y bases débiles que fuertes. A continuación se enumeran los ácidos y bases fuertes más comunes:
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Ácidos fuertes</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Bases fuertes</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;">H 2SO4</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Ba(OH)2</td>
 </tr>
 </tbody>
 </table>
 Las fuerzas relativas de los ácidos pueden cuantificarse midiendo sus constantes de equilibrio en soluciones acuosas. En soluciones de la misma concentración, los ácidos más fuertes ionizan en mayor medida y por lo tanto producen concentraciones más altas de iones de hidronio que los ácidos más débiles. La constante de equilibrio para un ácido se llama constante de ionización ácida, Ka. Para la reacción de un ácido HA:  
 <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />
 la constante de ionización ácida se escribe como 
 <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />
 donde las concentraciones son aquellas que están en equilibrio. Aunque el agua es un reactivo en la reacción, también es el solvente, por lo que no incluimos [H2O] en la ecuación. Cuanto mayor sea el Ka de un ácido, mayor será la concentración de H3O+ y A− en relación con la concentración del ácido no ionizado, HA, en una mezcla en equilibrio, y más fuerte será el ácido. Un ácido se clasifica como “fuerte” cuando sufre una ionización completa, en cuyo caso la concentración de HA es cero y la constante de ionización ácida es inmensurablemente grande (Ka ≈ ∞). Los ácidos parcialmente ionizados se denominan “débiles” y sus constantes de ionización ácida pueden medirse experimentalmente.
 Para ilustrar esta idea, a continuación se muestran tres ecuaciones de ionización ácida y valores de Ka. Las constantes de ionización aumentan de la primera a la última de las ecuaciones enumeradas, lo que indica que la fuerza relativa del ácido aumenta en el orden CH3CO2H < HNO2 < HSO4−.
 <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />
 Otra medida de la fuerza de un ácido es su porcentaje de ionización. El porcentaje de ionización de un ácido débil se define en términos de la composición de una mezcla en equilibrio: 
 <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />
 Donde el numerador es equivalente a la concentración de la base conjugada del ácido (por estequiometría, [A−] = [H3O+]). A diferencia del valor Ka, el porcentaje de ionización de un ácido débil varía con la concentración inicial del ácido, normalmente disminuyendo a medida que aumenta la concentración.
 Al igual que para los ácidos, la fuerza relativa de una base se refleja en la magnitud de su constante de ionización básica (Kb) en soluciones acuosas. En soluciones de la misma concentración, las bases más fuertes ionizan en mayor medida y, por lo tanto, producen mayores concentraciones de iones de hidróxido que las bases más débiles. Una base más fuerte tiene una constante de ionización más grande que la que tiene una base más débil. Para la reacción de una base, B: 
 <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />
 la constante de ionización se escribe como 
 <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />
 La inspección de los datos de tres bases débiles que se presenta a continuación muestra los aumentos de la fuerza de la base en el orden de NO2− < CH2 CO2− < NH3.
 <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />
 Al igual que para los ácidos, la fuerza relativa de una base también se refleja en su porcentaje de ionización, calculado como
 <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />
 pero variará dependiendo de la constante de ionización básica y de la concentración inicial de la solución.
 Este texto es adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"> Openstax, Química 2e, Sección 14.3: Fuerzas Relativas de Ácidos y Bases.</a>

Fuerzas de Ácidos/Bases y Constantes de Disociación

La fuerza relativa de un ácido o base es el grado en que se ioniza cuando se disuelve en agua. Si la reacción de ionización es esencialmente 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

bronsted-lowry acids and bases

Proton Transfer in Acids and Bases

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...

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How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong Acids, Strong Bases, and pH

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Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

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Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

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Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

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.

Acid and Base Strength in Water | JoVE K12

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Acid and Base Strength in Water

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