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

Uma molécula anfotérica é capaz de agir como um ácido e uma base. A água é um exemplo de uma molécula anfotérica. Numa solução aquosa de amoníaco, a água pode atuar como um ácido através da doação de um próton ao amoníaco, uma base.Em contraste, a água atua como uma base numa solução aquosa de ácido clorídrico aceitando um próton do ácido. Porque é anfotérico, a água pode ser submetida a autoionização. Neste processo, uma molécula da água atua como o ácido doando um próton a outra molécula de água que atua como uma base ao aceitar esse próton.Isto resulta na produção de um íon hidrônico e um íon hidróxido. A constante de equilíbrio para a autoionização da água, Kᴡ, também conhecida como a constante íon-produto para a água, pode ser expressa como Kᴡ e tem um valor de 1 10-¹⁴. A sua expressão de equilíbrio é escrito como a concentração dos íons hidrônicos vezes a concentração dos íons hidróxidos, sem denominador uma vez que ambos os reagentes são líquidos.Na água pura a 25 graus Celsius, as concentrações dos íons hidrônicos e hidróxidos são iguais que é 1 10-⁷ M.Kᴡ pode ser utilizado para calcular a concentração de hidrónio e íons hidróxidos numa solução e para determinar se uma solução é ácida ou básica. Se uma solução for ácida, a concentração de íons hidrônicos será superior a íons hidróxidos. Em contraste, se uma solução for básica, a concentração de íons hidróxidos será superior aos íons hidrônicos.Se a concentração de íons hidrônicos na solução for 5 10-⁷ M, a concentração de íons hidróxidos pode ser determinada utilizando Kᴡ.Como os valores de Kᴡ e os íons hidrônicos são conhecidos, a concentração de íons de hidróxidos pode ser calculada para ser 2 10-⁸ M.Como a concentração de íons hidrônicos, 5 10-⁷ M, é mais elevada do que a concentração de íons hidróxidos, 2 10-⁸ M, a solução é ácida.

Água: um Ácido e base de bronsted-lowry

A reação entre um ácido de Brønsted-Lowry e água é chamada ionização ácida. Por exemplo, quando o fluoreto de hidrogénio se dissolve em água e ioniza, os protões são transferidos das moléculas de fluoreto de hidrogénio para as moléculas de água, produzindo iões hidrónio e iões fluoreto:
 <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />
A ionização básica de uma espécie ocorre quando ela aceita protões de moléculas de água. No exemplo abaixo, moléculas de piridina, C5NH5, sofrem ionização básica quando dissolvidas em água, produzindo iões hidróxido e piridínio:
 <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />
As reações de ionização anteriores sugerem que a água pode funcionar tanto como uma base (como na sua reação com fluoreto de hidrogénio) como um ácido (como na sua reação com amoníaco). As espécies capazes de doar ou aceitar protões são chamadas de anfipróticas, ou mais geralmente, anfotéricas, termo que pode ser usado para ácidos e bases por definições que não a de Brønsted-Lowry. As equações abaixo mostram as duas possíveis reações ácido-base para duas espécies anfipróticas, ião bicarbonato, e água:
 <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />
A primeira equação representa a reação do bicarbonato como ácido com água como base, enquanto que a segunda representa a reação de bicarbonato como base com água como ácido. Quando o bicarbonato é adicionado à água, ambos os equilíbrios são estabelecidos simultaneamente e a composição da solução resultante pode ser determinada através de cálculos de equilíbrio adequados. No estado líquido, as moléculas de uma substância anfiprótica podem reagir umas com as outras, conforme ilustrado para a água nas equações abaixo:
 <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />
O processo no qual moléculas semelhantes reagem aos iões produzidos é chamado de autoionização. A água líquida é submetida a autoionização em uma extensão muito pequena; a 25 °C, aproximadamente duas em cada mil milhões de moléculas de água são ionizadas. A extensão do processo de autoionização da água reflete-se no valor da sua constante de equilíbrio, a constante do produto de iões para a água, KW:
 <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />
A ligeira ionização da água pura reflete-se no pequeno valor da constante de equilíbrio; a 25 °C, KW tem um valor de 1,0 × 10−14.
 <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />
O processo é endotérmico, e assim a extensão da ionização e as concentrações resultantes do ião hidrónio e do ião hidróxido aumentam com a temperatura. Por exemplo, a 100 °C, o valor para KW é cerca de 5,6 × 10−13, aproximadamente 50 vezes maior do que o valor a 25 °C.
A autoionização da água produz o mesmo número de iões hidrónio e hidróxido. Por conseguinte, em água pura a 25 °C:
 <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />
As concentrações desses iões em uma solução são muitas vezes determinantes críticos das propriedades da solução e dos comportamentos químicos dos seus outros solutos, e um vocabulário específico foi desenvolvido para descrever essas concentrações em termos relativos. Uma solução é neutra se contiver concentrações iguais de iões hidrónio e hidróxido; ácida se contiver uma concentração superior de iões hidrónio do que iões hidróxido; e básica se contiver uma concentração inferior de iões hidrónio do que iões hidróxido.
Resumo de Relações para Soluções Ácidas, Básicas, e Neutras
<table style="margin-left: auto; margin-right: auto;">
<tbody>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Classificação</td>
<td style="color: black; border: 1px solid black; text-align: center;">Concentrações Relativas de Iões</td>
<td style="color: black; border: 1px solid black; text-align: center;">pH a 25 °C</td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">ácida</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;">neutra</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;">básica</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>
Este texto é adaptado de<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>, e <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Section 14.2: pH and pOH</a>.

Água: Um Ácido e Base de Bronsted-Lowry

A reação entre um ácido de Brønsted-Lowry e a água é chamada de ionização ácida. Por exemplo, quando o fluoreto de hidrogênio se dissolve na água e ioniza, ...

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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

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...

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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pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

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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...

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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 explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

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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...

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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. <br...

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How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

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Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

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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.

Water as an Amphiprotic Substance | JoVE K12

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Water as an Amphiprotic Substance

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