Name: weak acid equilibrium in water
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 4 min 2 s
Channel: JoVE

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Chemistry

Matter and its Interactions

PS.Chm.6.3

Weak Acid Solutions

Слабая кислота, такая как синильная кислота, является кислотой Бренстеда, поскольку она отдает протон молекуле воды и образует ион гидроксония. Слабая кислота частично диссоциирует в воде в соответствии с ее константой кислотной диссоциации Ka, которая составляет 4, 9 10⁻¹⁰ для синильной кислоты. Для синильной кислоты Ka равен концентрации гидроксония, умноженной на концентрацию цианид-ионов, деленную на концентрацию синильной кислоты.Константа кислотной диссоциации Ka может использоваться для определения концентрации иона гидроксония в слабом кислотном растворе и, следовательно, pH раствора. Концентрация ионов гидроксония и значение pH 0, 15 М раствора синильной кислоты могут быть рассчитаны с использованием его выражения равновесия и данных таблицы концентраций. Концентрации синильной кислоты, гидроксония и цианида в исходном состоянии и в состоянии равновесия могут быть выражены в таблице, которая показывает начальную, изменяющуюся и равновесную концентрации каждой из молекул.Для достижения равновесия начальная концентрация исходных веществ уменьшается по мере того, как начальная концентрация продуктов увеличивается в соответствии с их молярными соотношениями. Это изменение концентрации исходных веществ и продуктов обозначается x. Подстановка равновесных концентраций в выражение для Ka дает x, умноженное на x, деленное на 0, 15 минус x.Во многих слабых кислотах x, степень диссоциации, вероятно, будет очень маленькой по сравнению с начальной концентрацией 0, 15 моль на литр. 0, 15 минус x можно принять равным приблизительно 0, 15. При решении уравнения получаем x равно 8, 6 10⁻⁶ моль.Приближение 0, 15 минус x, равное 0, 15, допустимо только в том случае, если x меньше 5%от 0, 15 моль. Здесь x составляет 0, 0057%от 0, 15 моль, и, следовательно, это приближение справедливо. Следовательно, концентрация гидроксония составляет 8, 6 10⁻⁶ моль.Чтобы определить pH, возьмите отрицательный логарифм концентрации иона гидроксония. Решение этой проблемы показывает, что значение pH 0, 15 М раствора синильной кислоты составляет 5, 07. pH раствора можно использовать для определения Ka слабой кислоты.Например, уксусная кислота частично диссоциирует на ионы гидроксония и ионы ацетата при растворении в воде. Ка для уксусной кислоты может быть выражено как концентрация иона гидроксония, умноженная на концентрацию ацетат-иона, деленная на концентрацию уксусной кислоты. Если pH у 0, 20 М раствора уксусной кислоты составляет 2, 72, можно вычислить его концентрацию гидроксония, которая составляет 1, 9 10⁻³ моль.Таблица концентраций может быть построена на основе начальной и равновесной концентраций уксусной кислоты, ионов гидроксония и ацетат-ионов. Используя значащие цифры, 0, 20 минус 1, 9 10⁻³ по существу равно 0, 20. Подставляя значения равновесия в выражение Ka, получаем Ka равняется 1, 8 10⁻⁵.

Растворы слабой кислоты

Лишь немногие соединения действуют как сильные кислоты. Гораздо большее количество соединений ведут себя как слабые кислоты и лишь частично реагируют с водой, оставляя большое количество растворенных молекул в их первоначальном виде и генерируя относительно небольшое количество ионов гидрония. Слабые кислоты обычно встречаются в природе, будучи веществами, частично ответственными за тангеный вкус цитрусовых, жжение укусов насекомых, а также неприятные запахи, связанные с запахом тела. Знакомым примером слабой кислоты является уксусная кислота, основной ингредиент уксуса: 
 <img alt="Eq1" src="/files/ftp_upload/11400/11400_Equation_1.png" style="height: 50px;" />
 Использование двойной стрелки в приведенном выше уравнении обозначает аспект частичной реакции этого процесса. При растворении в воде в обычных условиях в ионизированной форме присутствует только около 1% молекул уксусной кислоты CH3COO. 
 Расчет концентрации ионов гидрония и pH слабой кислоты раствор 
 Формальная кислота, HCO2H, является одним раздражающим веществом, вызывающим реакцию организма на некоторые мутные укусы и стинги. Какова концентрация ионов гидрония и pH 0.534-M раствор формальной кислоты? 
 <img alt="Eq2" src="/files/ftp_upload/11400/11400_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;"> HCO2H (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;">HCO2- (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;">0.534 </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;">0.534 - x. </td>
 <td style="color: black; border: 1px solid black; text-align: center;">x </td>
 <td style="color: black; border: 1px solid black; text-align: center;">x </td>
 </tr>
 </tbody>
 </table>
 Подстановка равновесных терминов концентрации в выражение Ka дает 
 <img alt="Eq3" src="/files/ftp_upload/11400/11400_Equation_3.png" style="height: 90px;" />
 Относительно большая начальная концентрация и небольшая константа равновесия позволяют упростить предположение, что x будет значительно меньше 0.534, и таким образом уравнение становится 
 <img alt="Eq4" src="/files/ftp_upload/11400/11400_Equation_4.png" style="height: 90px;" />
 Решение уравнения для получения х урожаев 
 <img alt="Eq5" src="/files/ftp_upload/11400/11400_Equation_5.png" style="height: 90px;" />
 Чтобы проверить предположение, что x невелик по сравнению с 0.534, его относительную величину можно оценить: 
 <img alt="Eq6" src="/files/ftp_upload/11400/11400_Equation_6.png" style="height: 90px;" />
 Поскольку x меньше 5% от начальной концентрации, предположение верно. Как определено в таблице ЛЬДА, x равно равновесной концентрации гидрония иона: 
 <img alt="Eq7" src="/files/ftp_upload/11400/11400_Equation_7.png" style="height: 50px;" />
 Наконец, рассчитывается pH 
 <img alt="Eq8" src="/files/ftp_upload/11400/11400_Equation_8.png" style="height: 50px;" />
 Определение Ка от рН 
 PH 0.0516 M раствор закиси азота, HNО2, составляет 2.34. Что такое Ка? 
 <img alt="Eq9" src="/files/ftp_upload/11400/11400_Equation_9.png" style="height: 50px;" />
 Концентрация закиси азота является формальной концентрацией, которая не учитывает никаких химических равновесий, которые могут быть установлены в раствор. Такие концентрации рассматриваются как “начальные” значения для расчетов равновесия с использованием таблицы ICE. Обратите внимание, что начальное значение иона гидрония указано как приблизительно нулевое, так как имеется небольшая концентрация H3O+ (1 × 10-7 M) из-за автоматической ионизации воды. Во многих случаях эта концентрация намного меньше, чем та, которая образуется при ионизации указанной кислоты (или основание), и ее можно игнорировать. 
 Полученный pH является логарифмической мерой концентрации ионов гидрония, полученной в результате кислотной ионизации зационной кислоты, и таким образом представляет собой «равновесное» значение для ледяной таблицы: 
 <img alt="Eq1" src="/files/ftp_upload/11400/11400_Equation_10.png" style="height: 50px;" />
 В этом случае 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;"> HNО2 (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;">NО2- (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;">0.0516 </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;">0.0046 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+0.0046 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+0.0046 </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;">0.0470 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.0046 </td>
 <td style="color: black; border: 1px solid black; text-align: center;">0.0046 </td>
 </tr>
 </tbody>
 </table>
 Наконец, рассчитайте значение константы равновесия, используя данные в таблице: 
 <img alt="Eq11" src="/files/ftp_upload/11400/11400_Equation_11.png" style="height: 90px;" />
 Этот текст адаптирован из<a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions"> Openstax, Химия 2е изд., раздел 4.2: Классификация химических реакций</a> и <a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"> Openstax, Химия 2е изд.,14.3 относительные сильные стороны кислот и оснований. </a>

Немногие соединения действуют как сильные кислоты. Гораздо большее количество соединений ведут себя как слабые кислоты и лишь частично реагируют с водой, оставляя подавляющее большинство ...

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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 water is only partial. Under typical conditions, only about 1% of acetic acid molecules are present as the ionized form, CH3COO−.

Weak acid problems often use an ICE table to find hydronium ion concentration and pH. Formic acid, HCO2H, is one example because it can cause the irritation from some ant bites and stings. For a 0.534-M formic acid solution, the ICE table starts with formic acid, H3O+, and HCO2−, then tracks the change as x forms and the equilibrium amounts are written in terms of x. The Ka expression is set up from those equilibrium concentrations.

Because the initial formic acid concentration is much larger than the amount that reacts, x is assumed to be much less than 0.534. That lets the expression simplify and makes the calculation easier. After solving for x, the result is checked against the 5% rule. Since x is less than 5% of the initial concentration, the assumption is valid. The value of x equals the equilibrium hydronium ion concentration, and the pH is then calculated from that concentration.

The same ICE table method can also be used in reverse to find Ka from pH. For nitrous acid, HNO2, the given pH is 2.34 for a 0.0516-M solution. That concentration is a formal concentration, which means it does not include any equilibrium changes. In these setups, the initial hydronium ion is shown as approximately zero because water already contains a very small amount, about 1 × 10−7 M, from autoionization. In many cases, that amount is much smaller than the acid-produced hydronium ion and can be ignored.

The pH gives the equilibrium hydronium ion concentration for the nitrous acid solution. The ICE table then shows HNO2, H3O+, and NO2− changing to equilibrium values. Using those values in the equilibrium expression gives the Ka of the acid. This approach shows how pH and Ka connect to the behavior of weak acids in water.

Weak Acid Equilibrium in Water

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 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

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 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

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...

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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

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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

Explore how weak acids partially ionize in water, use ICE tables to find hydronium ion concentration and pH, and calculate Ka from pH.

Weak Acid Equilibrium in Water | JoVE K12

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Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

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 ...

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 ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

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 ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

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 ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

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 ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

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

Intermolecular vs Intramolecular Forces

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

Intermolecular Forces

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

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

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

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

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Weak Acid Equilibrium in Water

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