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

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North Carolina K-12 Science Standard Course of Study

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Physical Science

Matter and its Interactions

PS.PSc.2.5

Determining the pH of Salt Solutions

Солевые растворы могут быть кислыми, основными или нейтральными. Можно исследовать отдельные ионы, чтобы определить, будет ли pH его раствора ниже, выше или равным семи. Соли, содержащие катионы и анионы с нейтральным pH, образуют нейтральные растворы.Эти соли состоят из противоположно заряженных ионов сильной кислоты и сильного основания. Чистый водный раствор нитрата калия будет иметь pH равный 7, поскольку ни калий, ни нитрат не обладают кислотными или основными свойствами. Соли, содержащие катион, являющийся противоположно заряженным ионом слабого основания, и анион, являющийся противоположно заряженным ионом сильной кислоты, будут иметь pH менее 7.В растворе бромида аммония ионы бромида имеют нейтральный pH, тогда как ионы аммония являются кислыми и отдают протоны молекулам воды. Соли, содержащие катион, являющийся противоположно заряженным ионом сильного основания, и анион, являющийся противоположно заряженным ионом слабой кислоты, будут иметь pH более 7. В растворе ацетата натрия ионы натрия имеют нейтральный pH, тогда как ионы ацетата являются основными и принимают протоны от молекул воды.Некоторые соли содержат катион и анион, которые являются противоположно заряженными ионами слабой кислоты и слабого основания соответственно. Раствор будет кислым, если Ka катиона больше, чем Kb аниона;основной, если Kb аниона больше, чем Ka катиона;или нейтрально, если Ka и Kb равны. В растворе нитрита аммония Ka для аммония выше, чем Kb для нитрит-ионов;следовательно, раствор будет кислым.Точный pH раствора соли, содержащего кислотный или основной ион, можно определить с использованием константы диссоциации для сопряженной кислоты или основания этого иона. pH 0, 35 М раствора цианида натрия можно определить, рассчитав Kb цианида из Ka его сопряженной кислоты синильной кислоты и построив таблицу концентраций для определения равновесной концентрации. Поскольку катионы натрия не реагируют с водой, они не влияют на pH, и их можно не учитывать.Напротив, ионы цианида принимают протоны от молекул воды и образуют гидроксид-ионы. Kb для цианид-ионов можно определить с помощью уравнения Ka, умноженного на Kb, равное Kw.Поскольку Ka для синильной кислоты составляет 4, 90 10⁻¹⁰, Kb для цианид-ионов составляет 2, 04 10⁻⁵. Kb равен концентрации синильной кислоты, умноженной на концентрацию гидроксид-ионов, деленной на концентрацию цианид-ионов.Таблица концентраций может быть построена для выражения начальной и равновесной концентраций. Подставляя равновесные концентрации в выражение, Kb равно x, умноженному на x, деленному на 0, 35, что можно проверить позже с помощью правила 5%При решении уравнения получаем x равно 2, 7 10⁻³ моль. Поскольку x составляет всего 0, 77%от 0, 35 M, приближение 0, 35 минус x равно 0, 35.pOH раствора можно рассчитать, взяв отрицательный логарифм из 2, 7 10⁻³ M, который равен 2, 57. pH раствора определяется с использованием уравнения pH плюс pOH, равного 14;следовательно, pH этого раствора цианида натрия составляет 11, 43.

Определение ph солевых растворов

PH соли раствор определяется его компонентными анионами и катионами. Соли, содержащие нейтральные по pH анионы и ионообразующие гидроний катионы, образуют раствор с pH менее 7. Например, в нитрате аммония (NH4NО3) раствор ионы NО3- не реагируют на воду, тогда как ионы NH4+ производят ионы гидрония, образующие кислотный раствор.  В отличие от этого, соли, содержащие pH-нейтральные катионы, и анионы, производящие гидроксид, образуют раствор с pH больше 7. Например, в растворе фторида натрия (NaF) раствор Na+ нейтрален по pH, но F- производит ионы гидроксида и образует основной раствор. Контраоны сильной кислоты или основание являются pH-нейтральными, а соли, образованные такими контраонами, образуют нейтральный раствор с pH равным 7. Например, в KBR катион K+ инертен и не влияет на pH. Ион бромистого вещества является конъюгатом основание сильной кислоты, и поэтому он имеет силу пренебрежимый основание (никакой заметной ионизации основание). раствор находится в нейтральном положении. 
 Некоторые соли содержат как кислый катион, так и основной анион. Общая кислотность или основность раствор определяется относительной силой катиона и аниона, которую можно сравнить с помощью Ка и Кбайт. Например, в NH4F ион NH4+ является кислотным, а ион F- является основным (конъюгатный основание слабой кислоты HF). Сравнение двух констант ионизации: Ka of NH4+ составляет 5.6 × 10-10, а Kb of F- 1.6 × 10-11, поэтому раствор является кислотным, так как Ka > Kb. 
 Расчет pH кислой соли раствор 
 Анилин — это амин, который используется для изготовления красителей. Он изолирован как хлорид анилиния, [C6H5NH3+]CL, соль, приготовленная в результате реакции слабого анилина основание и соляной кислоты. Что такое pH 0.233 M раствор хлорида анилиния? 
 <img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />
 Ка для иона анилиния выводится из Кбайт для его конъюгата основание, анилина: 
 <img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />
 С помощью предоставленной информации подготовлена таблица ICE для данной системы: 
 <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;">Начальная концентрация (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;">Изменение (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;">Равновесная концентрация (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>
 Подстановка этих равновесных терминов концентрации в выражение Ка дает 
 <img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />
 Предположим, что x << 0.233, уравнение упрощено и решено для 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;" />
 В таблице ЛЬДА x определяется как молярность ионов гидрония, поэтому pH вычисляется как 
 <img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />
 Гидролиз [Al(H2O)6]3+ 
 Рассчитайте pH 0.10 M раствор хлорида алюминия, который полностью растворяется, чтобы дать гидрированный алюминиевый ион [Al(H2O)6]3+ в раствор. 
 Уравнение для реакции и Ка: 
 <img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />
 Таблица ICE с предоставленной информацией составляет 
 <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;">Начальная концентрация (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;">Изменение (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;">Равновесная концентрация (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>
 Подстановка выражения для равновесных концентраций в уравнение для константы ионизации дает: 
 <img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />
 Предполагая x << 0.10 и решая упрощенное уравнение, можно: 
 <img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />
 Таблица ЛЬДА, определенная x как равная концентрации ионов гидрония, и таким образом, значение pH рассчитывается как 2.92, а раствор является кислотным. 
 <img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />
 Этот текст адаптирован из<a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, раздел 14.4: Гидролиз солей</a>.

Определение pH солевых растворов

pH солевого раствора определяется входящими в него анионами и катионами. Соли, содержащие pH-нейтральные анионы и ионобразующие катионы гидроксония ...

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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 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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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...

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

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Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

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

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

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 ...

Subatomic Particles

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 ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

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 ...

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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