Name: weak base ph and kb calculations
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 21 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

Weak Base Solutions

Слабое основание, такое как аммиак, представляет собой основание Бренстеда, которое принимает протон из воды для образования гидроксид-иона. Слабые основания частично реагируют с водой в соответствии с их константой диссоциации оснований Kb, которая составляет 1, 76 10⁻⁵ для аммиака. Kb для аммиака можно выразить как концентрацию иона аммония, умноженную на концентрацию гидроксид-ионов, деленную на концентрацию аммиака в состоянии равновесия.Kb можно использовать для определения концентрации гидроксид-ионов в слабом растворе основания и, следовательно, pOH и pH раствора. Концентрацию гидроксид-ионов и значение pH 0, 23 М раствора аммиака можно определить, используя его основную константу диссоциации и составив таблицу концентраций, содержащую начальные и равновесные значения аммиака, ионов аммония и гидроксид-ионов. Подставляя равновесные концентрации в выражение Kb, Kb равно x, умноженному на x, деленному на 0, 23 минус x.Поскольку слабые основания демонстрируют частичную диссоциацию, 0, 23 минус x можно рассматривать как приблизительно 0, 23. При решении уравнения получаем x равно 2 10⁻³ моль. Приближение 0, 23 минус x равно 0, 23, так как концентрация гидроксид-иона составляет всего 0, 86%от 0, 23 моль на литр.Чтобы рассчитать pH этого раствора, сначала определите pOH, взяв отрицательный логарифм концентрации гидроксид-иона, который равен 2, 70. Значение pH можно определить по формуле:pH плюс pOH, равное 14 и рассчитанное как 11, 30. Kb для слабого основного раствора можно рассчитать, если известен pH слабого основного раствора.Метиламин слабое основание, которое частично диссоциирует в воде на ионы метиламмония и гидроксид-ионы. Kb для метиламина можно выразить как концентрацию иона метиламмония, умноженную на концентрацию гидроксид-ионов, деленную на концентрацию метиламина в состоянии равновесия. Чтобы рассчитать Kb для 0, 040 М раствора метиламина с pH 11, 6, сначала необходимо рассчитать pOH, а затем концентрацию его гидроксид-иона.Поскольку pH равен 11, 60, pOH составляет 2, 40, а его концентрация гидроксид-ионов составляет 4, 0 10⁻³. Таблица концентраций может быть построена по начальной и равновесной концентрациям метиламина, метиламмония и гидроксида. Подстановка равновесных концентраций в выражение для Kb дает значение для Kb, которое составляет 4, 4 10⁻⁴.

Растворы слабых оснований

Некоторые соединения производят ионы гидроксида при растворении химически реагируя с молекулами воды. Во всех случаях эти соединения реагируют только частично и так классифицируются как слабые основания. Эти типы соединений также изобилуют в природе и важных товарах в различных технологиях. Например, глобальное производство слабого аммиака основание, как правило, значительно превышает 100 метрических тонн в год, широко используется в качестве сельскохозяйственных удобрений, сырья для химического синтеза других соединений и активного ингредиента бытовых чистящих средств. При растворении в воде аммиак частично реагирует на ионы гидроксида, как показано ниже: 
 <img alt="Eq1" src="/files/ftp_upload/11401/11401_Equation_1.png" style="height: 50px;" />
 Это, по определению, реакция кислотно-основная, в данном случае включающая перенос ионов H+ из молекул воды в молекулы аммиака. В типичных условиях в качестве ионов NH4+ присутствует только около 1% растворенного аммиака. 
 Расчет концентраций ионов гидроксида и Poh в слабой основание раствор 
 Найдите концентрацию гидроксидного иона, пуха и pH 0.25 M раствор триметиламина, слабого основание: 
 <img alt="Eq2" src="/files/ftp_upload/11401/11401_Equation_2.png" style="height: 50px;" />
 Таблица ICE для этой системы 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;">(CH3)3N (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">(CH3)3NH+ (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">OH- (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;">0.25 </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;">0.25 - x. </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0 + x. </td>
 <td style="color: black; border: 1px solid black; text-align: center;">~0 + x. </td>
 </tr>
 </tbody>
 </table>
 Подстановка терминами равновесной концентрации в выражение Kb дает 
 <img alt="Eq3" src="/files/ftp_upload/11401/11401_Equation_3.png" style="height: 90px;" />
 Предполагая x << 0.25 и решая для получения х урожаев 
 <img alt="Eq4" src="/files/ftp_upload/11401/11401_Equation_4.png" style="height: 50px;" />
 Это значение меньше 5% от начальной концентрации (0.25), поэтому предположение оправдано. 
 Как определено в таблице ЛЬДА, x равно равновесной концентрации гидроксидного иона: 
 <img alt="Eq5" src="/files/ftp_upload/11401/11401_Equation_5.png" style="height: 50px;" />
 Расчетное значение PoH составляет 
 <img alt="Eq6" src="/files/ftp_upload/11401/11401_Equation_6.png" style="height: 50px;" />
 С помощью связи; 
 <img alt="Eq7" src="/files/ftp_upload/11401/11401_Equation_7.png" style="height: 50px;" />
 Позволяет вычислить pH: 
 <img alt="Eq8" src="/files/ftp_upload/11401/11401_Equation_8.png" style="height: 50px;" />
 Определение Kb от pH 
 Если pH 0.28 M раствор этиламина (C2H5NH2) составляет 12.10, что это за Kb? 
 <img alt="Eq9" src="/files/ftp_upload/11401/11401_Equation_9.png" style="height: 50px;" />
 Для расчета Kb этиламина сначала необходимо определить концентрацию Poh и ионов гидроксида. Поскольку pH составляет 12.10, PoH можно рассчитать следующим образом: 
 <img alt="Eq10" src="/files/ftp_upload/11401/11401_Equation_10.png" style="height: 50px;" />
 Поскольку Poh равно 1.90, концентрация ионов гидроксида раствор может быть вычислена по формуле 
 <img alt="Eq11" src="/files/ftp_upload/11401/11401_Equation_11.png" style="height: 50px;" />
 Для этой системы можно построить ледяной стол следующим образом 
 <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;">C2H5NH2 (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">C2H5NH3+ (aq) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">OH- (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;">0.28 </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;">0.0126 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+0,0126 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+0,0126 </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;">0.28 - 0.0126 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.0126 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.0126 </td>
 </tr>
 </tbody>
 </table>
 Так как 0.0126 м составляет 4.5% от 0.28 м, 0.28 – 0.0126 можно считать почти равным 0.28 м по правилу 5%. 
 После подстановки указанных выше значений в выражении для Kb этиламина, 
 <img alt="Eq12" src="/files/ftp_upload/11401/11401_Equation_12.png" style="height: 90px;" />
 Этот текст адаптирован из Openstax, Химия 2е изд.<a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions"> раздел 4.2:</a><a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions"> Классификация химических реакций</a> и <a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"> 14.3 относительных сильных сторон кислот и оснований. </a>

Некоторые соединения производят гидроксид-ионы при растворении в результате химической реакции с молекулами воды. Во всех случаях эти соединения вступают в реакцию лишь частично и...

Education

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Chemistry

Химия

Один

Acids and Bases

Кислоты и основания

KEY TERMS AND CONCEPTS

ОСНОВНЫЕ ТЕРМИНЫ И ПОНЯТИЯ

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 chemical synthesis, and an ingredient in household cleaners.

When ammonia dissolves in water, it reacts only partially to form hydroxide ions. This is an acid-base reaction because H+ ions move from water molecules to ammonia molecules. Under typical conditions, only about 1% of the dissolved ammonia is present as NH4+ ions.

The video also shows how to calculate hydroxide ion concentration, pOH, and pH for a weak base solution. For a 0.25 M trimethylamine solution, an ICE table is used to track initial, change, and equilibrium concentrations. The Kb expression is then written with the equilibrium terms, and the x &lt;&lt; 0.25 assumption is checked with the 5% rule before solving for x as the hydroxide ion concentration. From there, pOH is found and pH is calculated.

A second example shows how to determine Kb from pH. For a 0.28 M ethylamine solution with a pH of 12.10, the pOH is first found, then the hydroxide ion concentration is calculated. An ICE table is built for ethylamine, ethylammonium ion, and hydroxide ion. After applying the 5% rule, the values are substituted into the Kb expression to find the base dissociation constant.

Weak Base pH and Kb Calculations

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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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

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How Ka and Kb Show Acid-Base Strength

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

strong acid and base solutions

Strong Acids, Strong Bases, and pH

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

weak base solutions

Weak base pH and Kb calculations 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

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

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

Acid and Base Strength in Water

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

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How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

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 weak bases form hydroxide ions, then use ICE tables to find pOH, pH, and Kb for trimethylamine and ethylamine examples.

Weak Base pH and Kb Calculations | JoVE K12

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New York State Science Learning Standards

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Phase Transitions: Sublimation and Deposition

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Physical Properties of Matter

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

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The Atomic Theory of Matter

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Ions and Ionic Charges

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The Periodic Table

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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 ...

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.

Weak Base pH and Kb Calculations

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