Name: salt hydrolysis and ph in solutions
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 4 min 8 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.5

Determining the pH of Salt Solutions

塩溶液は、酸性、塩基性、または中性にすることができます。個々のイオンを調べて、その溶液のpHが7未満、7以上、または等しいかどうかを判断できます。
pH 中性の陽イオンと陰イオンを含む塩は、中性溶液を形成します。これらの塩は、強酸と強塩基の対イオンで構成されています。硝酸カリウムの純粋な水溶液は、カリウムも硝酸塩も酸性または塩基性の特性を持たないため、pHは7になります。
弱塩基の対イオンである陽イオンと強酸の対イオンである陰イオンを含む塩のpHは7未満になります。臭化アンモニウムの溶液では、臭化物イオンはpH中性ですが、アンモニウムイオンは酸性で、水分子にプロトンを供与します。
強塩基の対イオンであるカチオンと弱酸の対イオンである陰イオンを含む塩のpHは7より大きくなります。酢酸ナトリウム溶液では、ナトリウムイオンはpH中性ですが、酢酸イオンは塩基性で、水分子からプロトンを受け入れます。
一部の塩には、弱酸と弱塩基の対イオンである陽イオンと陰イオンが含まれています。陽イオンのKAが陰イオンのKBよりも大きい場合、溶液は酸性になります。陰イオンのKbが陽イオンのKAより大きい場合の基本。または、KAとKBが等しい場合は中立です。
亜硝酸アンモニウムの溶液では、アンモニウムのKaは亜硝酸イオンのKbよりも高いため、溶液は酸性になります。
酸性イオンまたは塩基性イオンを含む塩溶液の正確なpHは、そのイオンの共役酸または塩基の解離定数を使用して決定できます。
0.35 Mシアン化ナトリウムのpHは、その共役酸(青酸)のKAからシアン化物のKbを計算し、平衡濃度を決定するためのICEテーブルを設定することで決定できます。 
ナトリウムカチオンは水と反応しないため、pHに影響を与えず、省略できます。対照的に、シアン化物イオンは水分子からプロトンを受け入れ、水酸化物イオンを生成します。
シアン化物イオンのKbは、Ka × Kb = KWの式を使用して決定できます。青酸のKaが10−10×4.90であるのに対し、シアン化物イオンのKbは10−5×2.04である。
Kbは、青酸の濃度に水酸化物イオンの濃度を掛けたものをシアン化物イオンの濃度で割ったものに等しくなります。
ICEテーブルは、初期濃度と平衡濃度を表すように構築できます。平衡濃度を式に代入すると、Kb は x x x を 0.35 で割ったものに等しく、これは後で 5% ルールによって検証できます。
この方程式を解くと、x は 2.7 × 10-3 モルに等しくなります。x は 0.35 M の 0.77% にすぎないため、0.35 から x を引いた近似は 0.35 に等しくなります。
溶液のpOHは、2.7 × 10-3 Mの負の対数を取ることによって計算でき、これは2.57に相当します。
溶液のpHは、pHプラスpOHが14に等しいという式を用いて決定され、したがって、このシアン化ナトリウム溶液のpHは11.43である。

塩水溶液のphの決定

塩の水溶液のpHは、構成要素である陰イオンと陽イオンによって決まります。pH的に中性の陰イオンと、ヒドロニウムイオンを生成する陽イオンを含む塩は、pH7以下の溶液を生成します。例えば、硝酸アンモニウム（NH4NO3）溶液では、NO3−イオンは水と反応せず、NH4+イオンはヒドロニウムイオンを生成して酸性溶液となります。例えば、フッ化ナトリウム（NaF）溶液では、Na+はpH中性ですが、F-は水酸化物イオンを生成して塩基性溶液を生成します。強酸または強塩基の対イオンはpH中性であり、そのような対イオンによって形成される塩は、pHが7に等しい中性溶液を生成します。例えば、KBrでは、K+陽イオンは加水分解反応に対して不活性のため、pHに影響を与えません。臭化物イオンは、強酸の共役塩基であるため、塩基強度は無視できるほど小さく、溶液は中性となります。
 塩の中には、酸性の陽イオンと塩基性の陰イオンの両方を含むものがあります。溶液の全体的な酸性度または塩基性度は、それらの陽イオンと陰イオンの相対的な強さによって決定され、KaとKbを用いて比較することができます。例えば、NH4Fでは、NH4+イオンが酸性で、F−イオンが塩基性（弱酸HFの共役塩基）となります。2つの解離定数を比較すると、NH4+のKaは5.6 × 10−10であり、F−のKbは1. 6 ×10−11なので、Ka >Kbなので、この溶液は酸性です。
 酸性塩水溶液のpH計算
 アニリンは染料の製造に使われるアミンの一種です。アニリンは、弱塩基のアニリンと塩酸を反応させた塩である塩化アニリニウム[C6H5NH3+]Clとして単離されます。塩化アニリニウムの0.233 M溶液のpHはいくらでしょうか？
 <img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />
 アニリニウムイオンのKaは、その共役塩基であるアニリンのKbから導出されます。
 <img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />
 Using the provided information, an ICE table for this system is prepared:
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C6H5NH3+ (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">C6H5NH2 (aq)</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">初期濃度 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.233</td>
 <td style="color: black; border: 1px solid black; text-align: center;">~0</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">濃度変化 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">平衡濃度 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.233 − x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 </tr>
 </tbody>
 </table>
 これらの平衡濃度の項をKaの式に代入すると、
 <img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />
 Assuming x << 0.233, the equation is simplified and solved for x: 
 <img alt="Eq4" src="/files/ftp_upload/11404/11404_Equation_4.png" style="height: 90px;" />
 <img alt="Eq5" src="/files/ftp_upload/11404/11404_Equation_5.png" style="height: 50px;" />
 ICE表では、xをヒドロニウムイオンの物質量として定義しているので、pHは次のように計算されます。
 <img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />
 [Al(H2O)6]3+の電離
 塩化アルミニウムの0.10 M溶液は、完全に溶解して水和アルミニウムイオン[Al(H2O)6]3+を生成するため、その溶液のpHを計算します。
 反応の式とKaは、
 <img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />
 An ICE table with the provided information is
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)63+ (aq)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)5(OH)2+ (aq)</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">初期濃度 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.10</td>
 <td style="color: black; border: 1px solid black; text-align: center;">~0</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">濃度変化 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">平衡濃度 (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.10 − x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 </tr>
 </tbody>
 </table>
 これらの平衡濃度の式をイオン化定数の式に代入すると、
 <img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />
 Assuming x << 0.10 となり、簡略化した式を書くと、
 <img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />
 ICE表では、xがヒドロニウムイオン濃度に等しいと定義されているため、pHは2.92と計算され、溶液は酸性です。
 <img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />
 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/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>.

塩水溶液のpHの決定

塩溶液のpHは、その成分であるアニオンとカチオンによって決まります。pH中性の陰イオンとヒドロニウムイオン生成陽イオンを含む塩...

Education

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Acids and Bases

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主要用語と概念

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 contain pH-neutral cations and anions that produce hydroxide ions. These salts form basic solutions with pH above 7. Sodium fluoride is an example. In NaF, Na+ is pH-neutral, while F− reacts with water to produce hydroxide ions.

Salts made from the counterions of a strong acid or a strong base are usually neutral. Their solutions have a pH of 7. In KBr, K+ is inert and does not change the pH. Br− is the conjugate base of a strong acid, so it has negligible base strength and does not appreciably ionize in water.

Some salts contain both an acidic cation and a basic anion. In those cases, the overall pH depends on which ion is stronger. The ionization constants Ka and Kb are used to compare them. For NH4F, NH4+ is acidic and F− is basic. Because Ka for NH4+ is 5.6 × 10−10 and Kb for F− is 1.6 × 10−11, the solution is acidic since Ka is greater than Kb.

The pH of an acidic salt solution can be calculated with an ICE table. Anilinium chloride, [C6H5NH3+]Cl, comes from the weak base aniline and hydrochloric acid. For a 0.233 M solution, the Ka value for the anilinium ion is found from the Kb of aniline. The ICE table gives x as the hydronium ion concentration, and the pH is then calculated from that value.

Hydrolysis of the hydrated aluminum ion works the same way. Aluminum chloride dissolves completely to give [Al(H2O)6]3+ in solution. For a 0.10 M solution, the reaction and Ka are set up in an ICE table. After assuming x is much smaller than 0.10 and solving the simplified equation, the hydronium ion concentration gives a pH of 2.92. The solution is acidic.

Salt Hydrolysis and pH in Solutions

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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 and pOH in Water

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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

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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 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...

determining the ph of salt 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

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key terms and concepts

Learn how salt ions affect pH, from acidic ammonium salts and basic fluoride salts to neutral salts and pH calculations with ICE tables.

Salt Hydrolysis and pH in Solutions | 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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Classifying Matter by State

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Matter: Pure Substances and Mixtures
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Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

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Vapor Pressure

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

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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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Intermolecular Forces

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

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The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

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Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

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Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

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

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

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

PS.PSc.1.5

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Alkali Metals

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 ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

IUPAC Nomenclature of Ketones

Like aldehydes, ketones are named using IUPAC rules; in this case, by replacing &#8220;e&#8221; in the name of the longest hydrocarbon chain with ...

IUPAC Nomenclature of Carboxylic Acids

IUPAC names of carboxylic acids are systematically derived following a few rules discussed below.
For acyclic saturated monocarboxylic acids, the longest ...

nomenclature-of-aromatic-compounds-with-a-single-substituent

Nomenclature of Aromatic Compounds with a Single Substituent

Benzene is the simplest aromatic hydrocarbon or arene. The IUPAC names for simple monosubstituted benzene derivatives are derived by adding the ...

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.

Salt Hydrolysis and pH in Solutions

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