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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Physical Science

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PS.PSc.2.5

Determining the pH of Salt Solutions

Salzlösungen können sauer, basisch oder neutral sein. Die einzelnen Ionen können untersucht werden, um festzustellen, ob der pH-Wert der Lösung unter, über oder gleich sieben liegen wird.
Salze, die pH-neutrale Kationen und Anionen enthalten, bilden neutrale Lösungen. Diese Salze setzen sich aus den Gegenionen einer starken Säure und einer starken Base zusammen. Eine reine wässrige Lösung von Kaliumnitrat hat einen pH-Wert von 7, da weder Kalium noch Nitrat saure oder basische Eigenschaften haben.
Salze, die ein Kation enthalten, das das Gegenion einer schwachen Base ist, und ein Anion, das das Gegenion einer starken Säure ist, haben einen pH-Wert von weniger als 7. In einer Lösung von Ammoniumbromid sind die Bromid-Ionen pH-neutral, während die Ammonium-Ionen sauer sind und Protonen an die Wassermoleküle abgeben.
Salze, die ein Kation enthalten, das das Gegenion einer starken Base ist, und ein Anion, das das Gegenion einer schwachen Säure ist, haben einen pH-Wert von mehr als 7. In einer Natriumacetatlösung sind die Natriumionen pH-neutral, während die Acetationen basisch sind und Protonen aus den Wassermolekülen aufnehmen.
Einige Salze enthalten ein Kation und ein Anion, die Gegenionen einer schwachen Säure bzw. einer schwachen Base sind. Die Lösung ist sauer, wenn das Ka des Kations größer ist als das Kb des Anions; basisch, wenn das Kb des Anions größer ist als das Ka des Kationen; oder neutral, wenn Ka und Kb gleich sind.
In einer Lösung von Ammoniumnitrit ist das Ka für Ammonium höher als das Kb für Nitritionen, daher ist die Lösung sauer.
Der genaue pH-Wert einer Salzlösung, die ein saures oder basisches Ion enthält, kann unter Verwendung der Dissoziationskonstante für die konjugierte Säure oder Base dieses Ions bestimmt werden.
Der pH-Wert von 0,35 M Natriumcyanid kann bestimmt werden, indem der K b des Cyanids aus dem Ka seiner konjugierten Säure - Blausäure - berechnet und eine ICE-Tabelle zur Bestimmung der Gleichgewichtskonzentration erstellt wird. 
Da Natriumkationen nicht mit Wasser reagieren, beeinflussen sie den pH-Wert nicht und können weggelassen werden. Im Gegensatz dazu nehmen Cyanid-Ionen Protonen aus Wassermolekülen auf und erzeugen Hydroxid-Ionen.
Der Kb für Cyanid-Ionen kann mit der Gleichung K a × Kb = KW bestimmt werden. Da der Ka für Blausäure 4,90 × 10−10 beträgt, beträgt der Kb für Cyanidionen 2,04 × 10−5.
K b ist gleich der Konzentration von Blausäure multipliziert mit der Konzentration der Hydroxidionen dividiert durch die Konzentration der Cyanidionen.
Eine ICE-Tabelle kann erstellt werden, um die Anfangs- und Gleichgewichtskonzentrationen auszudrücken. Setzt man die Gleichgewichtskonzentrationen in den Ausdruck ein, so ist Kb gleich x mal x geteilt durch 0,35, was später durch die 5%-Regel überprüft werden kann.
Beim Lösen der Gleichung ist x gleich 2,7 × 10−3 molaren. Da x nur 0,77% von 0,35 M ist, ist die Näherung 0,35 minus x ist gleich 0,35 gültig.
Der pOH der Lösung kann berechnet werden, indem der negative Logarithmus von 2,7 × 10−3 M genommen wird, was 2,57 entspricht.
Der pH-Wert der Lösung wird mit der Gleichung pH plus pOH gleich 14 bestimmt, daher beträgt der pH-Wert dieser Natriumcyanidlösung 11,43.

bestimmung des ph-wertes von salzlösungen

Der pH-Wert einer Salzlösung wird durch die Anionen und Kationen ihrer Bestandteile bestimmt. Salze, die pH-neutrale Anionen und die Hydroniumionen erzeugenden Kationen enthalten, bilden eine Lösung mit einem pH-Wert von weniger als 7. Beispielsweise reagieren in einer Ammoniumnitratlösung (NH4NO3) NO3−-Ionen nicht mit Wasser, während NH4+-Ionen die Hydroniumionen erzeugen Es entsteht eine saure Lösung. Im Gegensatz dazu bilden Salze, die pH-neutrale Kationen und die Hydroxidionen erzeugenden Anionen enthalten, eine Lösung mit einem pH-Wert von mehr als 7. Beispielsweise ist in einer Natriumfluoridlösung (NaF) das Na+ pH-neutral, aber das F- erzeugt das Hydroxidionen und bildet die basische Lösung. Die Gegenionen einer starken Säure oder Base sind pH-neutral und die von solchen Gegenionen gebildeten Salze bilden eine neutrale Lösung mit einem pH-Wert von 7. Beispielsweise ist in KBr das K+-Kation inert und hat keinen Einfluss auf den pH-Wert. Das Bromidion ist die konjugierte Base einer starken Säure und hat daher eine vernachlässigbare Basenstärke (keine nennenswerte Basenionisierung). Die Lösung ist neutral. Einige Salze enthalten sowohl ein saures Kation als auch ein basisches Anion. Der Gesamtsäuregehalt oder die Basizität einer Lösung wird durch die relative Stärke von Kation und Anion bestimmt, die mithilfe von Ka und Kb verglichen werden kann. Beispielsweise ist in NH4F das NH4+-Ion sauer und das F−-Ion basisch (konjugierte Base der schwachen Säure HF). Vergleich der beiden Ionisationskonstanten: Ka von NH4+ beträgt 5,6 × 10−10 und Kb von F− beträgt 1,6 × 10−11, die Lösung ist also sauer, da Ka > Kb. Berechnung des pH-Werts einer sauren Salzlösung Anilin ist ein Amin, das zur Herstellung von Farbstoffen verwendet wird. Es wird als Aniliniumchlorid, [C6H5NH3+]Cl, isoliert, ein Salz, das durch die Reaktion der schwachen Base Anilin und Salzsäure hergestellt wird. Wie hoch ist der pH-Wert einer 0,233 M Lösung von Aniliniumchlorid? <img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;"> Das Ka für Aniliniumion leitet sich vom Kb für seine konjugierte Base Anilin ab: <img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;"> Anhand der bereitgestellten Informationen wird eine ICE-Tabelle für dieses System erstellt: <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> Das Einsetzen dieser Gleichgewichtskonzentrationsterme in den Ka-Ausdruck ergibt <img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;"> Unter der Annahme, dass x << 0,233 ist, wird die Gleichung vereinfacht und nach x aufgelöst: <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;"> Die ICE-Tabelle definiert x als die Hydroniumionenmolarität und daher wird der pH-Wert berechnet als <img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;"> Hydrolyse von [Al(H2O)6]3+ Berechnen Sie den pH-Wert einer 0,10 M Lösung von Aluminiumchlorid, die sich vollständig auflöst und das hydratisierte Aluminiumion [Al(H2O)6]3+ in Lösung ergibt. Die Gleichung für die Reaktion und Ka lautet: <img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;"> Eine ICE-Tabelle mit den bereitgestellten Informationen ist <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> Wenn man die Ausdrücke für die Gleichgewichtskonzentrationen in die Gleichung für die Ionisationskonstante einsetzt, erhält man: <img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;"> Wenn x << 0,10 angenommen wird und die vereinfachte Gleichung gelöst wird, ergibt sich: <img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;"> Die ICE-Tabelle definiert x als gleich der Hydroniumionenkonzentration, daher wird der pH-Wert mit 2,92 berechnet und die Lösung ist sauer. <img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;"> Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>

Bestimmung des pH-Wertes von Salzlösungen

Der pH-Wert einer Salzlösung wird durch ihre Bestandteile Anionen und Kationen bestimmt. Salze, die pH-neutrale Anionen und die Hydroniumionen-produzierenden Kationen ...

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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...

water: a bronsted-lowry acid and base

Water as an Amphiprotic Substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

ph scale

pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

relative strengths of conjugate acid-base pairs

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

How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong Acids, Strong Bases, and pH

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weak acid solutions

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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...

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pH of Acid Mixtures

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

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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Acid and Base Strength in Water

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polyprotic acids

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How Bonding Affects Acid Strength

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lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how 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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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

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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.

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Phase Transitions

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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

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 ...

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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

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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.

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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

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 ...

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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