Name: acid and base strength in water
Uploaded: 2025-10-30T13:58:47.000Z
Duration: 3 min 2 s
Channel: JoVE

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acidbase-strengths-and-dissociation-constants

Acid/Base Strengths and Dissociation Constants

酸と塩基は、強酸、強塩基、弱酸、弱塩基のいずれであるかによって分類できます。強酸と強塩基は非常に少ないため、酸と塩基の大部分は弱いです。
強酸は塩酸と同様に、水に溶解すると水素イオンと塩化物イオンに完全に解離します。水酸化ナトリウムのような強塩基は、ナトリウムイオンと水酸化物イオンに完全に解離します。
弱酸と弱塩基は部分的に解離し、イオン化型と非イオン化型の両方で存在します。例えば、酢酸とその弱結合塩基である酢酸の両方が水溶液中に見出されます。
弱酸または弱塩基の解離の程度は、その平衡定数を使用して測定できます。弱酸の平衡定数には、酸解離定数、またはKAという特別な名前があります。
一般的な弱酸HAの場合、特定の温度でのKAは、生成物であるAイオンとヒドロニウムイオンの濃度を反応物、HAおよび水の濃度で割る平衡方程式によって計算できます。
水は液体であり、その濃度は反応中でもほとんど変化しないため、方程式から除外されます。
KAが高いほど、酸は強くなります。亜硝酸のKAは酢酸のKaよりも大きいため、亜硝酸は酢酸よりも強いです。 
弱い塩基の平衡定数である塩基解離定数(Kb)は、KAと同様に作用します。一般的な弱塩基Bの場合、特定の温度でのKbは、生成物BHイオンと水酸化物イオンの濃度を反応物Bの濃度で割ることによって決定できます。
酸と同様に、塩基の強度もKbに正比例します。たとえば、エチルアミンのKB は尿素の KB よりも大きいため、エチルアミンは尿素よりも比較的強力です。 
酸の強度は、イオン化率で表すこともできます。酸のイオン化率は、平衡状態のヒドロニウムイオン濃度を初期酸濃度で割り、それに100を掛けることによって計算できます。 
同様に、塩基のイオン化率は、平衡状態の水酸化物イオン濃度を塩基の初期濃度で割り、100を掛けることによって計算できます。イオン化率が高いほど、酸または塩基が強くなります。

酸/塩基強度及び解離定数

酸や塩基の相対的な強さとは、水に溶解させた際のイオン化の度合いのことです。イオン化反応がほとんど完全に進行する場合、それらは強酸や強塩基と呼ばれます。一方、イオン化がほとんど起こらない場合、それらは弱酸や弱塩基と呼ばれます。弱酸・弱塩基は強酸・強塩基よりも多く存在します。代表的な強酸・強塩基は下記の通りです。
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">強酸</td>
 <td style="color: black; border: 1px solid black; text-align: center;">強塩基</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>
 酸の相対的な強さは、水溶液中の平衡定数を解析することで定量化できます。同じ濃度の水溶液中では、強酸は弱酸よりもよりイオン化しており、高濃度のヒドロニウムイオンを生成します。酸の平衡定数を酸解離定数Kaといいます。酸HAの反応に対して:  
 <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />
 酸解離定数は下記のように表されます。 
 <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />
 ここで、濃度は平衡状態のものを指します。水は反応の反応物ですが、溶媒でもあるので、[H2O]は式に含めません。酸のKaが大きいほど、平衡混合物中の非電離酸であるHAの濃度に対して、H3O+とA−の濃度が大きくなり、酸が強くなります。酸が完全に電離した場合にはHAの濃度はゼロとなり、酸解離定数は計り知れないほど大きくなる（Ka ≈ ∞）ため、「強酸」と分類されます。部分的に電離している酸は「弱酸」と呼ばれ、その酸解離定数は実験的に測定することができます。
 この考えを説明するために、3つの酸のイオン化式とKaの値を以下に示します。解離定数は列挙された式の下側に向かって増加しており、CH3CO2H < HNO2 < HSO4−の順に相対的な酸の強さが増加することを示しています。
 <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />
 酸の強さを表すもう一つの指標は、そのイオン化率です。弱酸のイオン化率は、平衡混合物の組成に基づいて定義されます。 
 <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />
 ここで、分子の濃度は酸の共役塩基の濃度に相当する（化学量論的には、[A−] = [H3O+]）。弱酸性のイオン化率はKa値と異なり、酸の初期濃度に応じて変化し、一般的には濃度が高くなるにつれて減少します。
 酸の場合と同様に、塩基の相対的な強さは、水溶液中の塩基解離定数（Kb）の大きさに反映されます。同じ濃度の水溶液では、強塩基は弱塩基よりも大きな割合でイオン化し、水酸化物イオンの濃度が高くなります。強塩基は、弱塩基よりも解離定数が大きいです。塩基Bの反応について: 
 <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />
 解離定数は下記のように表されます。 
 <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />
 以下に示す3つの弱塩基のイオン化式を見ると、NO2− < CH2 CO2− < NH3の順に塩基強度が増加することがわかります。
 <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />
 酸と同様に、塩基の相対的な強さはイオン化率に反映されます。イオン化率の計算式は次の通りです。
 <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />
 この値は、塩基解離定数や溶液の初期濃度によって変化します。
 上記の文章は以下から引用しました。 <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>

酸または塩基の相対的な強さは、水に溶解したときにイオン化する程度です。イオン化反応が本質的に完了している場合、...

Education

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Chemistry

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Acids and Bases

酸と塩基

KEY TERMS AND CONCEPTS

主要用語と概念

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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ph scale

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relative strengths of conjugate acid-base pairs

relative-strengths-of-conjugate-acid-base-pairs

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 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...

mixtures of acids

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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 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...

determining the ph of salt solutions

Salt Hydrolysis and pH in Solutions

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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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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...

key terms and concepts

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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JoVE Core 化学は、簡潔で理解しやすいアニメーションビデオレッスンを使用して、一般的な化学の概念を生き生きとしたものにします。さらに、活動する科学者のビデオでは、現在世界中の実験室で行われている古典的そして独創的な研究・実験をお見せします。

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Acid and Base Structure

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Acids and Bases: Percent Dissociation and pH

Classifying Matter by State

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Classifying Matter by Composition

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Elements: Chemical Symbols and Isotopes

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Molecules and Compounds

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Phase Transitions

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Vapor Pressure

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

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Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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PS.PSc.1.3

The Atomic Theory of Matter

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Subatomic Particles

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The Bohr Model

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Emission Spectra

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The de Broglie Wavelength

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The Uncertainty Principle

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Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

Ions and Ionic Charges

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Use models to compare representations of atoms, ions, and isotopes.

PS.PSc.1.5

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Periodic Classification of the Elements

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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Electron Affinity

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Halogens

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Noble Gases


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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

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Ionic Bonding and Electron Transfer

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Covalent Bonding and Lewis Structures

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Bonding in Metals

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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

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Nomenclature of Alkenes

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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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