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

Le soluzioni saline possono essere acide, basiche o neutre. I singoli ioni possono essere esaminati per determinare se il pH della sua soluzione sarà inferiore, superiore, o uguale a sette. I sali che contengono cationi e anioni a pH neutro formano soluzioni neutre.

Questi sali sono composti dai controioni di un acido forte e di una base forte. Una soluzione acquosa pura di nitrato di potassio avrà un pH di 7, poiché né il potassio, né il nitrato hanno proprietà acide o basiche. I sali che contengono un catione, che è il controione di una base debole, e un anione, che è il controione di un acido forte, avranno un pH inferiore a 7.

In una soluzione di bromuro di ammonio, gli ioni bromuro sono a pH neutro, mentre gli ioni di ammonio sono acidi e donano protoni alle molecole d'acqua. I sali che contengono un catione, che è il controione di una base forte, e un anione, che è il controione di un acido debole, avranno un pH maggiore di 7. In una soluzione di acetato di sodio, gli ioni del sodio sono a pH neutro, mentre gli ioni di acetato sono basici e accettano protoni dalle molecole d'acqua.

Alcuni sali contengono un catione e un anione, i quali sono controioni, rispettivamente, di un acido debole e di una base debole. La soluzione sarà acida se il valore della Ka del catione è maggiore del valore della Kb dell'anione;basica se il valore della Kb dell'anione è superiore al valore della Ka del catione;oppure neutro se Ka e Kb sono uguali. In una soluzione di nitrito di ammonio, la Ka per l'ammonio è superiore alla Kb per gli ioni nitrito;dunque la soluzione sarà acida.

Il pH esatto di una soluzione salina contenente uno ione acido o basico può essere determinato utilizzando la costante di dissociazione per l'acido coniugato o per la base di quello ione. Il pH del cianuro di sodio 0, 35 M può essere determinato calcolando il valore della Kb del cianuro dalla Ka del suo acido coniugato acido cianidrico e impostando una tabella ICE per determinare la concentrazione di equilibrio. Poiché i cationi di sodio non reagiscono con l'acqua, non influenzano il pH e possono essere omessi.

Al contrario, gli ioni cianuro accettano protoni dalle molecole d'acqua e generano ioni idrossido. La Kb per gli ioni di cianuro può essere determinata utilizzando l'equazione Ka per Kb è uguale a Kw.Poiché la Ka per l'acido cianidrico è 4, 90 10⁻¹⁰, la Kb per gli ioni cianuro è 2, 04 10⁻⁵. Lal Kb è uguale alla concentrazione di acido cianidrico moltiplicata per la concentrazione di ioni idrossido divisa per la concentrazione di ioni cianuro.

È possibile costruire una tabella ICE per illustrare le concentrazioni iniziale e di equilibrio. Sostituendo le concentrazioni di equilibrio nell'espressione, Kb è uguale a x volte x diviso per 0, 35, che può essere verificato in seguito con la regola del 5 percento. Dopo aver risolto l'equazione, x è uguale a 2, 7 10⁻³ molare.

Poiché x è solo lo 0, 77%di 0, 35 M, l'approssimazione 0, 35 meno x è uguale a 0, 35 è valida. Il pOH della soluzione può essere calcolato prendendo il log negativo di 2, 7 10⁻³ M, che è uguale a 2, 57. Il pH della soluzione viene determinato utilizzando l'equazione pH più pOH è uguale a 14;pertanto, il pH di questa soluzione di cianuro di sodio è 11, 43.

determinazione del ph delle soluzioni saline

Il pH di una soluzione salina è determinato dai suoi componenti anioni e cationi. I sali che contengono anioni a pH neutro e i cationi che producono ioni idronio formano una soluzione con un pH inferiore a 7. Ad esempio, nella soluzione di nitrato di ammonio (NH_4NO_3), gli ioni NO_3^− non reagiscono con l'acqua mentre gli ioni NH_4^+ producono gli ioni idronio ottenendo la soluzione acida. Al contrario, i sali che contengono cationi a pH neutro e anioni che producono ioni idrossido formano una soluzione con un pH maggiore di 7. Ad esempio, nella soluzione di fluoruro di sodio (NaF), l’Na^+ è a pH neutro ma l'F^- produce il ioni idrossido e forma la soluzione basica. I controioni di un acido o di una base forte sono a pH neutro e i sali formati da tali controioni formano una soluzione neutra con un pH pari a 7. Ad esempio, in KBr, il catione K^+ è inerte e non influenza il pH. Lo ione bromuro è la base coniugata di un acido forte, e quindi ha una forza basica trascurabile (nessuna ionizzazione apprezzabile della base). La soluzione è neutra.

Alcuni sali contengono sia un catione acido che un anione basico. L'acidità o la basicità complessiva di una soluzione è determinata dalla forza relativa del catione e dell'anione, che può essere confrontata utilizzando K_a e K_b. Ad esempio, in NH_4F, lo ione NH_4^+ è acido e lo ione F^− è basico (base coniugata dell'acido debole HF). Confrontando le due costanti di ionizzazione: la K_a di NH_4^+ è 5,6 × 10^−10 e la K_b di F^− è 1,6 × 10^−11, quindi la soluzione è acida, poiché K_a > K_b.

Calcolo del pH di una soluzione salina acida

L'anilina è un'ammina utilizzata per produrre coloranti. Viene isolato come cloruro di anilinio, [C_6H_5NH_3^+]Cl, un sale preparato dalla reazione della base debole anilina e acido cloridrico. Qual è il pH di una soluzione 0,233 M di cloruro di anilinio?

<img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />

La K_a dello ione anilinio deriva dalla K_b della sua base coniugata, l'anilina:

<img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />

Utilizzando le informazioni fornite, viene preparata una tabella ICE per questo 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;">Initial Concentration (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;">Change (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;">Equilibrium Concentration (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>

Sostituendo questi termini di concentrazione all'equilibrio nell'espressione K_a si ottiene

<img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />

Assumendo x << 0,233, l'equazione viene semplificata e risolta per 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;" />

La tabella ICE definisce x come la molarità degli ioni idronio, quindi il pH viene calcolato come

<img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />

Idrolisi di [Al(H_2O)_6]_3^+

Calcolare il pH di una soluzione 0,10 M di cloruro di alluminio, che si dissolve completamente per dare lo ione alluminio idratato [Al(H2O)6]3+ in soluzione.

L'equazione per la reazione e K_a è:

<img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />

È disponibile una tabella ICE con le informazioni fornite

<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;">Initial Concentration (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;">Change (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;">Equilibrium Concentration (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>

Sostituendo le espressioni per le concentrazioni di equilibrio nell'equazione per la costante di ionizzazione si ottiene:

<img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />

Assumendo x << 0,10 e risolvendo l'equazione semplificata si ottiene:

<img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />

La tabella ICE definisce x come uguale alla concentrazione di ioni idronio, quindi il pH calcolato è 2,92 e la soluzione è acida.

<img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />

Questo testo è adattato da <a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>

Determinazione del pH delle soluzioni saline

Il pH di una soluzione salina è determinato dagli anioni e dai cationi che lo compongono. I sali che contengono anioni a pH neutro e i cationi che producono ioni idronio ...

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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

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

pH and pOH in Water

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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

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...

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

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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

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: Chimica illustra concetti chiave di chimica attraverso video animazioni concise e di immediata comprensione. Inoltre, i video della sezione "scienziati in azione" mostrano procedure metodologiche realizzate da ricercatori provenienti dai migliori laboratori internazionali.

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9-12.C.1.6

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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
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Colloids

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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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Phase Transitions

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Phase Transitions: Vaporization and Condensation

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Clausius-Clapeyron Equation

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

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Heating and Cooling Curves

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Physical and Chemical Properties of Matter

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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

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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 ...

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Emission Spectra

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The de Broglie Wavelength

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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.

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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 ...

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PS.PSc.1.5

The Periodic Table

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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 ...

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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