Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
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Water: A Bronsted-Lowry Acid and Base

يستطيع جزيء مذبذب أن يؤدي دور الحمض والقاعدة على حد سواء. الماء مثال على الجزيء المذبذب. في محلول الأمونيا المائي،يستطيع الماء أن يؤدي دور الحمض بمنحه بروتونًا للأمونيا،التي هي قاعدة.وعلى عكس ذلك،يؤدي الماء دور القاعدة في محلول الهيدروكلوريك المائي بأتن يستقبل بروتونًا من الحمض. لأنه مذبذب،يستطيع الماء أن يتأين تلقائيًا. في هذه العملية،جزيء واحد من الماء يؤدي دور الحمض عبر منحه بروتونًا لجزيء آخر من الماء،والذي بدوره يؤدي دور القاعدة عبر استقباله ذلك البروتون.ينتج عن هذا أيون هيدرونيوم وأيون هيدروكسيد. ثابت التوازن للتأين التلقائي للماء،Kw،الذي يُعرف كذلك بثابت ناتج الأيونات للماء،يمكن التعبير عنه بـ Kw وقيمته 1 10⁻¹⁴. تُكتب معادلة توازنه بتركيز أيونات الهيدرونيوم مضروبًا بتركيز أيونات الهيدروكسيد،دون وجود مقام،لأن كلتا المادتين المتفاعلتين من السوائل.في الماء النقي عند درجة حرارة 25 مئوية،يتساوى تركيز أيونات الهيدرونيوم والهيدروكسيد وتكون قيمتها 1 10⁻⁷ مولار. يمكن استخدام Kw لحساب تركيز أيونات الهيدرونيوم والهيدروكسيد في محلول وتحديد نوع المحلول ما إذا كان حمضيًا أم قاعديًا. إذا كان المحلول حمضيًا،يكون تركيز أيونات الهيدرونيوم أعلى من تركيز أيونات الهيدروكسيد.وعلى العكس،إذا كان المحلول قاعديًا،يكون تركيز أيونات الهيدروكسيد أعلى من تركيز أيونات الهيدرونيوم. إذا كان تركيز أيونات الهيدرونيوم في محلول يساوي 5 10⁻⁷ مولار،يمكن تحديد تركيز أيونات الهيدروكسيد باستخدام Kw.بما أن قيم Kw وأيونات الهيدرونيوم معروفة،يمكن حساب تركيز أيونات الهيدروكسيد ليكون 2 10⁻⁸ مولار. وبما أن تركيز أيونات الهيدرونيوم وقيمته 5 10⁻⁷،أعلى من تركيز أيونات الهيدروكسيد التي قيمتها 2 10⁻⁸ مولار،يكون المحلول حمضيًا.

الماء: حمض وقاعدة برونستيد-لوري

يسمى التفاعل بين حمض برونستيدø-لوري والماء بتأين الحمض. على سبيل المثال، عندما يذوب فلوريد الهيدروجين في الماء ويتأين، يتم نقل البروتونات من جزيئات فلوريد الهيدروجين إلى جزيئات الماء، مما ينتج عنه أيونات الهيدرونيوم وأيونات الفلوريد:  <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" /> يحدث التأين الأساسي لأحد الأنواع عندما يقبل البروتونات من جزيئات الماء. في المثال أدناه، تخضع جزيئات البيريدين، C5NH5، للتأين الأساسي عند إذابتها في الماء، مما ينتج عنه أيونات الهيدروكسيد والبيريدينيوم:  <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" /> تشير تفاعلات التأين السابقة إلى أن الماء قد يعمل كقاعدة (كما في تفاعله مع فلوريد الهيدروجين) وحمض (كما في تفاعله مع الأمونيا). الأنواع القادرة على التبرع بالبروتونات أو قبولها تسمى برمائية، أو بشكل أعم، مذبذبة، وهو مصطلح يمكن استخدامه للأحماض والقواعد حسب التعريفات بخلاف برونستيدø-لوري. توضح المعادلات أدناه التفاعلين الحمضيين القاعدين المحتملين لنوعين برمائيات ، أيون البيكربونات والماء:  <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" /> تمثل المعادلة الأولى تفاعل البيكربونات كحمض مع الماء كقاعدة، بينما تمثل المعادلة الثانية تفاعل البيكربونات كقاعدة مع الماء كحامض. عند إضافة البيكربونات إلى الماء، يتم إنشاء هذين التوازن في وقت واحد ويمكن تحديد تكوين المحلول الناتج من خلال حسابات التوازن المناسبة. في الحالة السائلة ، يمكن أن تتفاعل جزيئات مادة برمائية مع بعضها البعض كما هو موضح للمياه في المعادلات أدناه:  <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" /> تسمى العملية التي تتفاعل فيها الجزيئات المتشابهة مع إنتاج الأيونات بالتأين الذاتي. يخضع الماء السائل للتأين الذاتي إلى حد ضئيل للغاية 25 °C، يتأين ما يقرب من اثنين من كل مليار جزيء ماء. ينعكس مدى عملية التأين الذاتي للماء في قيمة ثابت التوازن ، ثابت المنتج الأيوني للماء W: <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" /> ينعكس التأين الطفيف للمياه النقية في القيمة الصغيرة لثابت التوازن ؛ في 25 °C, KW لها قيمة 1.0 × 10−14. <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" /> هذه العملية ماصة للحرارة، وبالتالي يزداد مدى التأين والتركيزات الناتجة من أيون الهيدرونيوم وأيون الهيدروكسيد مع زيادة درجة الحرارة. على سبيل المثال، عند 100 °C، تكون قيمة KW حوالي 5.6 × 10−13، تقريبًا أكبر بمقدار 50 مرة من القيمة عند 25 °C. ينتج عن التأين الذاتي للماء نفس عدد أيونات الهيدرونيوم والهيدروكسيد. لذلك، في الماء النقي عند 25 °C: <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" /> غالبًا ما تكون تركيزات هذه الأيونات في المحلول محددات حاسمة لخصائص المحلول والسلوكيات الكيميائية لمذاباته الأخرى، وقد تم تطوير مفردات محددة لوصف هذه التركيزات بمصطلحات نسبية. يكون المحلول متعادلاً إذا كان يحتوي على تركيزات متساوية من أيونات الهيدرونيوم والهيدروكسيد؛ حمضي إذا كان يحتوي على تركيز أيونات الهيدرونيوم أكبر من أيونات الهيدروكسيد؛ وأساسي إذا كان يحتوي على تركيز أقل من أيونات الهيدرونيوم من أيونات الهيدروكسيد. 
 ملخص العلاقات للحلول الحمضية والأساسية والمحايدة <table style="margin-left: auto; margin-right: auto;"><tbody><tr><td style="color: black; border: 1px solid black; text-align: center;">التصنيف </td><td style="color: black; border: 1px solid black; text-align: center;">تركيزات الأيون النسبية </td><td style="color: black; border: 1px solid black; text-align: center;">درجة حموضة 25 °C </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">حمضي </td><td style="color: black; border: 1px solid black; text-align: center;">[H3O+] > [OH−] </td><td style="color: black; border: 1px solid black; text-align: center;">الرقم الهيدروجيني < 7 </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">الوضع المحايد </td><td style="color: black; border: 1px solid black; text-align: center;">[H3O+] = [OH−] </td><td style="color: black; border: 1px solid black; text-align: center;">الرقم الهيدروجيني = 7 </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">أساسي </td><td style="color: black; border: 1px solid black; text-align: center;">[H3O+] < [OH−] </td><td style="color: black; border: 1px solid black; text-align: center;">الرقم الهيدروجيني > 7 </td></tr></tbody></table>تم اقتباس هذا النص من <a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chemistry 2e, Section 14.1: Brønsted-Lowry Acids and Bases</a>, and <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Section 14.2: pH and pOH</a>.

يسمى التفاعل بين حمض برونستيد-لوري والماء بالتأين الحمضي. على سبيل المثال ، عندما يذوب فلوريد الهيدروجين في الماء ويتأين ، ...

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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 can donate or accept protons is called amphiprotic. The broader term amphoteric is also used for substances that can act as acids or bases under different definitions. Bicarbonate ion is another amphiprotic species. It can react with water as an acid or as a base, and both equilibria can be present at the same time in solution.

Liquid water can also react with itself. This process is called autoionization. It happens only to a very small extent. At 25 °C, about two out of every billion water molecules are ionized. The equilibrium constant for this process is the ion-product constant for water, K_w, and its value is 1.0 × 10^-14 at 25 °C.

Autoionization is endothermic, so more ionization occurs as temperature rises. At 100 °C, K_w is about 5.6 × 10^-13, which is roughly 50 times larger than at 25 °C. Pure water always produces equal amounts of hydronium and hydroxide ions through this process. A solution is neutral when these ion concentrations are equal. It is acidic when hydronium ion concentration is greater than hydroxide ion concentration, and basic when hydroxide ion concentration is greater. At 25 °C, acidic solutions have pH below 7, neutral solutions have pH 7, and basic solutions have pH above 7.

Water as an Amphiprotic Substance

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 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

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

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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...

acid strength and molecular structure

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 water can act as both an acid and a base, why it is amphiprotic, and how autoionization affects hydronium, hydroxide, and pH.

Water as an Amphiprotic Substance | JoVE K12

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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 ...

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

Analyze the structure of atoms and isotopes.

Water as an Amphiprotic Substance

Description

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