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

Os ácidos e bases podem ser categorizados por serem ou não um ácido forte, uma base forte, um ácido fraco, ou uma base fraca. Existem muito poucos ácidos e bases fortes portanto, a maioria dos ácidos e as bases são fracas. Um ácido forte, como o ácido clorídrico, dissocia-se completamente em íons de hidrogénio e íons de cloreto quando dissolvido em água.Uma base forte, como o hidróxido de sódio, dissocia-se completamente em íons de sódio e íons de hidróxido. Os ácidos e bases fracos dissociam-se parcialmente e estão presentes em ambas as formas ionizadas e não ionizadas. Por exemplo, ambos os ácidos acéticos e as suas fracas bases conjugadas, acetato, são encontrados numa solução aquosa.O grau de dissociação de um ácido ou base fraca pode ser medido utilizando a sua constante de equilíbrio. A constante de equilíbrio para ácidos fracos tem um nome especial, a constante de dissociação ácida, ou, Ka.Para um ácido genérico fraco HA, Ka a uma dada temperatura pode ser calculada através de uma equação de equilíbrio:dividindo a concentração de produtos, íon A e íon hidrônico, pela concentração de reagentes, HA e água. Como a água é líquida e a sua concentração permanece quase inalterada na reação, está excluída da equação.Quanto mais alto o Ka, mais forte o ácido. O ácido nitroso é mais forte do que o ácido acético porque o Ka do ácido nitroso é maior do que o Ka do ácido acético. A constante de equilíbrio para bases fracas, a constante de dissociação de base, ou Kb, atua de forma semelhante ao Ka.Para uma base genérica fraca B, Kb a uma dada temperatura pode ser determinado ao dividir a concentração de produtos, íon BH, e íon hidróxido, pela concentração do reagente, B.Tal como os ácidos, a força das bases é também diretamente proporcional ao Kb.Por exemplo, a etilamina é relativamente mais forte que a ureia porque a Kb da etilamina é maior do que o Kb da ureia.A força de um ácido também pode ser expresso em termos de percentagem de ionização. A percentagem de ionização do ácido pode ser calculado ao dividir a concentração de íons de hidrónio em equilíbrio pela concentração ácida inicial e multiplicando-a por cem. Da mesma forma, a percentagem de ionização para bases pode ser calculada ao dividir a concentração de íons hidróxidos em equilíbrio pela concentração inicial da base e multiplicando-a por cem.Quanto maior for a percentagem de ionização, mais forte o ácido ou a base.

forças de Ácidos/bases e constantes de dissociação

A força relativa de um ácido ou base é a extensão em que se ionizam quando dissolvidos em água. Se a reação de ionização for essencialmente completa, o ácido ou a base é denominado forte; se relativamente pouca ionização ocorrer, o ácido ou a base é fraco. Há muito mais ácidos e bases fracos do que fortes. Os ácidos e bases fortes mais comuns estão listados abaixo:
<table style="margin-left: auto; margin-right: auto;">
<tbody>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Ácidos Fortes</td>
<td style="color: black; border: 1px solid black; text-align: center;">Bases Fortes</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>
As forças relativas dos ácidos podem ser quantificadas medindo as suas constantes de equilíbrio em soluções aquosas. Em soluções com a mesma concentração, ácidos mais fortes ionizam-se em maior medida e, por isso, produzem concentrações mais elevadas de iões hidrónio do que ácidos mais fracos. A constante de equilíbrio para um ácido é chamada a constante de ionização do ácido, Ka. Para a reação de um ácido HA:  
<img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />
a constante de ionização do ácido é escrita como 
<img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />
onde as concentrações são aquelas em equilíbrio. Embora a água seja um reagente na reação, é também o solvente, então não incluímos [H2O] na equação. Quanto maior a Ka de um ácido, maior a concentração de H3O+ e A− em relação à concentração do ácido não ionizado, HA, em uma mistura de equilíbrio, e mais forte o ácido. Um ácido é classificado como “forte” quando é submetido a ionização completa, caso em que a concentração de HA é zero e a constante de ionização do ácido é imensamente grande (Ka ≈ ∞). Os ácidos que são parcialmente ionizados são chamados de “fracos”, e as suas constantes de ionização de ácido podem ser medidas experimentalmente.
Para ilustrar esta idéia, três equações de ionização de ácido e valores de Ka são mostrados abaixo. As constantes de ionização aumentam da primeira para a última das equações listadas, indicando que a força relativa do ácido aumenta na ordem CH3CO2H < HNO2 < HSO4−.
<img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />
Outra medida da força de um ácido é a sua ionização percentual. A ionização percentual de um ácido fraco é definida em termos da composição de uma mistura de equilíbrio: 
<img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />
onde o numerador é equivalente à concentração da base conjugada do ácido (por estequiometria, [A−] = [H3O+]). Ao contrário do valor de Ka, a ionização percentual de um ácido fraco varia com a concentração inicial de ácido, diminuindo normalmente à medida que a concentração aumenta.
Tal como para ácidos, a força relativa de uma base reflete-se na magnitude da sua constante de ionização de base (Kb) em soluções aquosas. Em soluções com a mesma concentração, as bases mais fortes ionizam-se em maior medida e, por conseguinte, produzem concentrações de iões hidróxido mais elevadas do que as bases mais fracas. Uma base mais forte tem uma constante de ionização maior do que uma base mais fraca. Para a reação de uma base, B: 
<img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />
a constante de ionização é escrita como 
<img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />
A inspeção dos dados para três bases fracas apresentadas abaixo mostra que a força da base aumenta na ordem NO2− < CH2 CO2− < NH3.
<img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />
Como para os ácidos, a força relativa de uma base também é refletida na sua ionização percentual, computada como
<img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />
mas irá variar dependendo da constante de ionização da base e da concentração inicial da solução.
Este texto é adaptado de <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>

Forças de Ácidos/Bases e Constantes de Dissociação

A força relativa de um ácido ou base é a extensão em que ele ioniza quando dissolvido em água. Se a reação de ionização estiver essencialmente 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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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...

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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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