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

As soluções salinas podem ser ácidas, básicas ou neutras. Os íons individuais podem ser examinados para determinar se o pH da sua solução será abaixo, acima, ou igual a sete. Os sais que contêm catíons e aníons com pH-neutro formam soluções neutras.Estes sais são compostos por contrarreferências de um ácido forte e uma base forte. Uma solução aquosa pura de nitrato de potássio terá um pH de 7, uma vez que nem o potássio nem o nitrato tem propriedades ácidas ou básicas. Os sais que contêm um catíon que é o contra-íon de uma base fraca e um aníon que é o contra-íon de um ácido forte terá um pH inferior a 7.Numa solução de brometo de amónio, os íons de brometo têm pH neutro, enquanto que os íons de amónio são ácidos e doam prótons às moléculas de água. Os sais que contêm um catíon que é um contra-íon de uma base forte e um aníon que é o contra-íon de um ácido fraco terá um pH superior a 7. Numa solução de acetato de sódio, os íons de sódio têm pH neutro, enquanto que os íons de acetato são básicos e aceitam prótons das moléculas de água.Alguns sais contêm um catíon e um aníon que são contra-íons de um ácido fraco e base fraca, respectivamente. A solução será ácida se o Ka do catíon for maior do que o Kb do aníon;básico se o Kb do aníon for maior do que o Ka do catíon;ou neutro se o Ka e o Kb forem iguais. Numa solução de nitrito de amónio, o Ka para o amónio é mais elevado do que o Kb para os íons nitritos;portanto, a solução será ácida.O pH exato de uma solução de sal que contém um íon ácido ou básico pode ser determinada utilizando a dissociação constante para o ácido conjugado ou base desse íon. O pH de 0, 35 M de cianeto de sódio pode ser determinado através do cálculo do Kb do cianeto do Ka do seu ácido conjugado ácido cianídrico e a criação de uma tabela ICE para determinar a concentração de equilíbrio. Como os catíons de sódio não reagem com a água, não afetam o pH e podem ser omitidos.Em contraste, os íons de cianeto aceitam prótons de moléculas de água e geram íons hidróxidos. O Kb para os íons de Cianeto podem ser determinados utilizando a equação Ka vezes Kb, igual a Kw.Como o Ka para o ácido hidrociânico é de 4, 90 10-¹⁰, o Kb para os íons de cianeto é de 2, 04 10-⁵. O Kb é igual à concentração do ácido cianídrico vezes a concentração de íons hidróxidos divididos pela concentração de íons de cianeto.Uma tabela ICE pode ser construída para expressar as concentrações iniciais e de equilíbrio. Substituindo a concentrações de equilíbrio na expressão, Kb é igual a x vezes x dividido por 0, 35, e pode ser verificada mais tarde, pela regra dos 5%Ao resolver a equação, x é igual a 2, 7 10-³ molar. Como x é apenas 0, 77%de 0, 35 mols, a aproximação 0, 35 menos x é igual a 0, 35 é válido.O pOH da solução pode ser calculado tomando o registo negativo de 2, 7 10-³ mols, o que equivale a 2, 57. O pH da solução é determinado utilizando a equação pH mais pOH, igual a 14;portanto, o pH desta solução de sódio de cianeto é 11, 43.

determinação do ph de soluções salinas

O pH de uma solução salina é determinado pelos seus aniões e catiões componentes. Os sais que contêm aniões de pH neutro e catiões que produzem iões hidrónio formam uma solução com um pH inferior a 7. Por exemplo, em solução de nitrato de amónio (NH4NO3), iões NO3− não reagem com água, enquanto que iões NH4+ produzem iões hidrónio, resultando em solução ácida.  Em contraste, os sais que contêm catiões de pH neutro e aniões que produzem iões hidróxido formam uma solução com um pH superior a 7. Por exemplo, em solução de fluoreto de sódio (NaF), a Na+ tem pH neutro, mas F- produz iões hidróxido e forma a solução básica. Os contraiões de um ácido ou de uma base forte são neutros em termos de pH e os sais formados por esses contraiões formam uma solução neutra com um pH igual a 7. Por exemplo, no KBr, o catião K+ é inerte e não afeta o pH. O ião brometo é a base conjugada de um ácido forte e, por isso, tem força básica insignificante (sem ionização básica apreciável). A solução é neutra.
Alguns sais contêm tanto um catião ácido como um anião básico. A acidez ou a basicidade total de uma solução é determinada pela força relativa do catião e do anião, que pode ser comparada usando Ka e Kb. Por exemplo, em NH4F, o ião NH4+ é ácido e o ião F− é básico (base conjugada do ácido fraco HF). Comparando as duas constantes de ionização: Ka do NH4+ é 5,6 × 10−10 e Kb do F− é 1,6 × 10−11, pelo que a solução é ácida, uma vez que Ka > Kb.
Cálculo do pH de uma Solução Salina Ácida
A anilina é uma amina que é utilizada para fabricar corantes. É isolada como cloreto de anilínio, [C6H5NH3+]Cl, um sal preparado pela reação da base fraca anilina com ácido clorídrico. Qual é o pH de uma solução de cloreto de anilínio a 0,233 M?
<img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />
A Ka para o ião anilínio é derivado da Kb para a sua base conjugada, anilina:
<img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />
Utilizando as informações fornecidas, é preparada uma tabela ICE para este sistema:
<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;">Concentração Inicial (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;">Alteração (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;">Concentração em Equilíbrio (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>
Substituindo estes termos de concentração de equilíbrio na expressão de Ka obtemos
<img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />
Assumindo que x << 0,233, a equação é simplificada e resolvida para 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;" />
A tabela ICE define x como a molaridade de iões hidrónio e, assim, o pH é calculado como
<img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />
Hidrólise de [Al(H2O)6]3+
Cálculo do pH de uma solução de cloreto de alumínio a 0,10 M, que se dissolve completamente para dar iões de alumínio hidratado [[Al(H2O)6]3+ em solução.
A equação para a reação e Ka são:
<img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />
Uma tabela ICE com as informações fornecidas é
<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;">Concentração Inicial (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;">Alteração (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;">Concentração em Equilíbrio (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>
Substituindo as expressões das concentrações de equilíbrio na equação para a constante de ionização obtemos:
<img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />
Assumindo que x << 0,10 e resolvendo a equação simplificada obtemos:
<img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />
A tabela ICE definiu x como sendo igual à concentração de iões hidrónio, e então o pH é calculado como sendo 2,92, e a solução é ácida.
<img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />
Este texto é adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>.

Determinação do pH de Soluções Salinas

O pH de uma solução salina é determinado por seus ânions e cátions componentes. Os sais que contêm ânions de pH neutro e os cátions produtores de íons hidrônio ...

Education

JoVE Core

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Ácidos e Bases

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

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

bronsted-lowry acids and bases

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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

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strong acid and base solutions

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weak base solutions

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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...

ions as acids and bases

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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 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

acidbase-strengths-and-dissociation-constants

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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

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Salt Hydrolysis and pH in Solutions | JoVE K12

chemistry

JoVE Core - Química dá vida a conceitos gerais de química usando vídeos de animação fáceis de entender. Além disso, nos vídeos Cientistas em ação, demonstramos experimentos de pesquisa clássicos e originais realizados atualmente por cientistas em laboratórios em todo o mundo.

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Matter and Its Interactions

9-12.C.1.6

9-12.C.1.6.d

9-12.PS.3.6.c

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Molecules and Compounds

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Colloids

Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera ...

Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

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Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

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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

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

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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Intermolecular Forces

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

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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 ...

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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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