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

Кислоты и основания можно разделить на категории по тому, являются ли они сильной кислотой, сильным основанием, слабой кислотой или слабым основанием. Сильных кислот и оснований очень мало, поэтому большинство кислот и оснований слабые. Сильная кислота, такая как соляная кислота, при растворении в воде полностью диссоциирует на ионы водорода и ионы хлора.Сильное основание, такое как гидроксид натрия, полностью диссоциирует на ионы натрия и гидроксид-ионы. Слабые кислоты и основания частично диссоциируют и присутствуют как в ионизированной, так и в неионизированной форме. Например, и уксусная кислота, и слабое сопряженное с ней основание, ацетат, находятся в водном растворе.Степень диссоциации слабой кислоты или основания можно измерить, используя ее константу равновесия. Константа равновесия слабых кислот имеет особое название константа диссоциации кислоты, или Ka.Для обычной слабой кислоты в форме НА, Ka при заданной температуре можно рассчитать по уравнению равновесия:разделив концентрацию продуктов, иона A и иона гидроксония, на концентрацию исходных веществ, HA и воды. Поскольку вода является жидкой и ее концентрация в реакции практически не меняется, она исключается из уравнения.Чем выше Ка, тем сильнее кислота. Азотистая кислота сильнее уксусной кислоты, потому что Ка азотистой кислоты больше Ка уксусной кислоты. Константа равновесия для слабых оснований, константа диссоциации оснований, или Kb, действует аналогично Ka.Для обычного слабого основания B, Kb при данной температуре может быть определено путем деления концентрации продуктов, иона BH и гидроксид-иона, на концентрацию реагента B.Подобно кислотам, сила оснований также прямо пропорциональна Kb.Например, этиламин относительно сильнее мочевины, потому что Kb этиламина больше, чем Kb мочевины.Сила кислоты также может быть выражена в процентах ионизации. Процент ионизации кислоты можно рассчитать, разделив концентрацию ионов гидроксония в состоянии равновесия на начальную концентрацию кислоты и умножив ее на сто. Точно так же процент ионизации для оснований можно рассчитать, разделив концентрацию гидроксид-иона в состоянии равновесия на исходную концентрацию основания и умножив ее на сто.Чем выше процент ионизации, тем сильнее кислота или основание.

Кислотно-щелочная сила и константы диссоциации

Относительная прочность кислоты или основание - это степень ее ионизации при растворении в воде. Если ионизационная реакция по существу завершена, кислота или основание называют сильной; если происходит относительно небольшая ионизация, кислота или основание слабы. Существует гораздо больше слабых кислот и оснований, чем сильных. Ниже перечислены наиболее распространенные сильные кислоты и основания: 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Сильные кислоты </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Сильное основание </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;">HNО3</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>
 Относительные сильные стороны кислот можно количественно оценить, измерив их константы равновесия в водных растворах. В растворах той же концентрации более сильные кислоты ионизируются в большей степени и, таким образом, дают более высокую концентрацию ионов гидрония, чем более слабые кислоты. Константа равновесия для кислоты называется константой кислотоионизации, Ка. Для реакции кислоты HA:   
 <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />
 константа ионизации кислоты записывается как  
 <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />
 где концентрации находятся в равновесии. Несмотря на то, что вода является реагент в реакции, она также является растворителем, поэтому мы не включаем [H2O] в уравнение. Чем больше Ка кислоты, тем больше концентрация H3O+ и A- относительно концентрации неионизированной кислоты, ГК, в равновесной смеси, и тем сильнее кислота. Кислота классифицируется как «сильная», когда она подвергается полной ионизации, в этом случае концентрация ГК равна нулю, а константа ионизации кислоты неизмеримо велика (Ka ≈ ∞). Частично ионизированные кислоты называются “слабыми”, и их константы ионизации кислоты могут быть экспериментально измерены. 
 Чтобы проиллюстрировать эту идею, ниже показаны три уравнения ионизации кислоты и значения Ка. Константы ионизации увеличиваются с первого до последнего из перечисленных уравнений, указывая на увеличение относительной кислотной силы в порядке CH3CO2H < HNО2 < HSO4-. 
 <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />
 Другой мерой силы кислоты является ее процентная ионизация. Процентная ионизация слабой кислоты определяется по составу равновесной смеси:  
 <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />
 Где числитель эквивалентен концентрации конъюгата кислоты основание (по стехиометрии, [A-] = [H3O+]). В отличие от значения Ка, процентная ионизация слабой кислоты меняется с начальной концентрацией кислоты, обычно уменьшающейся по мере увеличения концентрации. 
 Так же, как и кислоты, относительная прочность основание отражается в величине его константы базовой ионизации (Kb) в водных растворах. В растворах с такой же концентрацией более сильные основания ионируют в большей степени, и таким образом дают более высокую концентрацию ионов гидроксида, чем более слабые основания. Более сильный основание имеет большую константу ионизации, чем более слабый основание. Для реакции основание, B:  
 <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />
 константа ионизации записывается как  
 <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />
 Проверка данных по трем слабым основаниям, представленная ниже, показывает, что сила основание увеличивается в порядке NО2- < CH2 CO2- < NH3. 
 <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />
 Что касается кислот, относительная сила основание также отражается в его процентной ионизации, вычисленной как 
 <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />
 но будет меняться в зависимости от константы ионизации основание и начальной концентрации раствор. 
 Этот текст адаптирован из<a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"> Openstax, Химия 2е изд., раздел 14.3: Относительные силы кислот и оснований. </a>

Относительная сила кислоты или основания — это степень, в которой она ионизируется при растворении в воде. Если реакция ионизации по существу завершена, то ...

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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...

water: a bronsted-lowry acid and base

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...

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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...

relative strengths of conjugate acid-base pairs

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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

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...

weak acid solutions

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...

weak base solutions

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...

ions as acids and bases

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...

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...

polyprotic acids

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...

acid strength and molecular structure

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...

lewis acids and bases

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 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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Acids and Bases: Percent Dissociation and pH

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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Acid and Base Strength in Water

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