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

Амфотерная молекула может проявлять свойства как кислоты и основания. Вода пример амфотерной молекулы. В водном растворе аммиака вода может действовать как кислота, отдавая протон аммиаку, основанию.Напротив, вода действует как основание в водном растворе соляной кислоты, принимая протон от кислоты. Поскольку вода является амфотерной, она может подвергаться автоионизации. В этом процессе одна молекула воды действует как кислота, отдавая протон другой молекуле воды, которая действует как основание, принимая этот протон.Это приводит к образованию иона гидроксония и гидроксид-иона. Константа равновесия для автоионизации воды, Kᴡ, также известная как константа произведения растворимости для воды, может быть выражена как Kᴡ и имеет значение 1 10⁻¹⁴. Выражение ее равновесия записывается как концентрация ионов гидроксония, умноженная на концентрацию гидроксид-ионов, без знаменателя, поскольку оба исходных вещества являются жидкостями.В чистой воде при 25 градусах Цельсия концентрации ионов гидроксония и гидроксида равны то есть 1 10⁻⁷ M.Kᴡ можно использовать для расчета концентрации ионов гидроксония и гидроксида в растворе и для определения того, является ли раствор кислотным или основным. Если раствор кислый, концентрация ионов гидроксония будет выше, чем гидроксид-ионов. Напротив, если раствор является основным, концентрация гидроксид-ионов будет выше, чем иона гидроксония.Если концентрация ионов гидроксония в растворе составляет 5 10⁻⁷ M, концентрацию гидроксид-иона можно определить с помощью Kᴡ.Поскольку значения Kᴡ и ионов гидроксония известны, концентрация гидроксид-ионов может быть рассчитана как 2 10⁻⁸ M.Поскольку концентрация ионов гидроксония, 5 10⁻⁷ M, выше, чем концентрация гидроксид-иона, 2 10⁻⁸ М раствор кислый.

Вода: кислота и основание Бренстеда-Лоури

Реакция между кислотой Брёнстед-Лоури и водой называется кислотной ионизацией. Например, когда фторид водорода растворяется в воде и ионизируется, протоны переносятся из молекул фторида водорода в молекулы воды, образуя ионы гидрония и ионы фторида: 
  <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />
 Ионизация вида основание происходит, когда он принимает протоны из молекул воды. В приведенном ниже примере молекулы пиридина C5NH5 подвергаются ионизации основание при растворении в воде, дающих ионы гидроксида и пиридиния: 
  <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />
 Предшествующие реакции ионизации предполагают, что вода может функционировать как основание (как в его реакции с фторидом водорода), так и как кислота (как в его реакции с аммиаком). Виды, способные либо жертвовать, либо принимать протоны, называются амфипротическими, или, в более общем смысле, амфотерическими, термин, который может использоваться для кислот и оснований в соответствии с определениями, отличными от Брёнстед-Лоури. Приведенные ниже уравнения показывают две возможные реакции кислотно-основная для двух амфипротических видов, бикарбоната иона и воды: 
  <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />
 Первое уравнение представляет реакцию бикарбоната как кислоты с водой как основание, в то время как второе представляет реакцию бикарбоната как основание с водой как кислоты. При добавлении бикарбоната в воду оба этих равновесия устанавливаются одновременно, и состав получаемого раствор может быть определен с помощью соответствующих вычислений равновесия. В жидком состоянии молекулы амфипротического вещества могут вступать в реакцию друг с другом, как показано для воды в уравнениях ниже: 
  <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />
 Процесс, в котором подобно молекулам реагируют на ионы намолота, называется автоматической ионизацией. Жидкая вода подвергается автоматической ионизации в очень небольшой степени; при 25 °C ионизируются приблизительно два из каждых миллиардов молекул воды. Степень процесса автоматической ионизации воды отражается в значении ее равновесной константы, константы ионного продукта для воды, КВТ: 
  <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />
 Небольшая ионизация чистой воды отражается в небольшом значении константы равновесия; при 25 °C, КВТ имеет значение 1.0 × 10-14. 
  <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />
 Этот процесс является эндотермическим, поэтому степень ионизации и результирующие концентрации ионов гидрония и гидроксида увеличиваются при повышении температуры. Например, при 100 °C значение ДЛЯ КВТ составляет около 5.6 × 10-13, примерно в 50 раз больше значения при 25 °C. 
 Аутоионизация воды приводит к тому же количеству ионов гидрония и гидроксида. Поэтому в чистой воде при 25 °C: 
  <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />
 Концентрации этих ионов в раствор часто являются критическими детерминантами свойств решения и химического поведения его других солей, и для описания этих концентраций в относительном выражении был разработан специальный словарь. раствор нейтрален, если он содержит одинаковые концентрации ионов гидрония и гидроксида; кислотен, если он содержит большую концентрацию ионов гидрония, чем ионы гидроксида; и является базовым, если он содержит меньшую концентрацию ионов гидрония, чем ионы гидроксида. 
 Резюме отношений по кислотным, базовым и нейтральным решениям 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Классификация </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Относительные концентрации ионов </td>
 <td style="color: black; border: 1px solid black; text-align: center;">PH при 25 °C. </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">кислый </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;">нейтраль </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;">базовый </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>
 Этот текст адаптирован из<a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Химия 2е изд., раздел 14.1: Bronsted-Lowry кислоты и основания</a>, и <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"> раздел 14.2: PH и Poh</a>.

Реакция между кислотой Брёнстеда-Лоури и водой называется кислотной ионизацией. Например, когда фтористый водород растворяется в воде и ионизируется, ...

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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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Strong Acids, Strong Bases, and pH

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

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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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pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

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Salt Hydrolysis and pH of Solutions

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

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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Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

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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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The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Water as an Amphiprotic Substance

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