Name: proton transfer in acids and bases
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 58 s
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Chemistry

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Bronsted-Lowry Acids and Bases

Arrhenius asit, suda çözüldüğünde bir adet hidrojen iyonu üreten bir maddedir ve Arrhenius bazı, bir OH⁻veya hidroksit iyonu üreten bir maddedir. Hidroklorik asit, suda çözündüğünde bir hidrojen iyonu ve bir klorür iyonuna ayrıştığı için bir Arrhenius asididir. Sodyum hidroksit, suda çözündüğünde bir sodyum iyonu ve bir hidroksit iyonuna ayrıştığı için bir Arrhenius bazıdır.Bununla birlikte, bu tanım, sulu bir çözelti içinde olmayan asitleri ve bazları veya hidroksit iyonları içermeyen bazları tanımlamak için kullanılamaz. Brønsted ve Lowry tarafından yapılan daha geniş bir tanım, bir asidi bir hidrojen iyonu veya proton vericisi olarak tanımlarken, bir baz bir proton alıcısıdır. Hidroklorik asit suda çözüldüğünde, suya bir proton vererek bir hidronyum iyonu ve bir klorür iyonu üreterek bir asit görevi görür.Amonyak suda çözüldüğünde bir baz görevi görür ve sudan bir proton kabul ederek bir amonyum iyonu ve bir hidroksit iyonu üretir. Bir Brønsted-Lowry asidi her zaman bir Brønsted-Lowry bazıyla reaksiyona girer ve bunun tersi de geçerlidir. Bir asit, örneğin asetik asit, protonunu verdiğinde, su bir baz görevi görür ve protonu kabul eder.Asetik asit bir eşlenik baza, asetata dönüştürülür ve su bir eşlenik aside, bir hidronyum iyonuna dönüştürülür. Bir protonun aktarımı nedeniyle birbirinden farklı olan asitler ve bazlar, eşlenik asit-baz çiftleri olarak adlandırılır. Ters reaksiyonda, eşlenik asit, hidronyum, bir proton vericisi olarak işlev görür ve eşlenik baz, asetat, bir protonu kabul eder.Bir asidin gücü, bir proton verme yeteneği ile belirlenirken, bir bazın gücü bir protonu kabul etme yeteneği ile belirlenir. Daha güçlü bir asit, zayıf bir asite göre daha çok proton verir. Benzer şekilde, daha güçlü bir bazın bir protonu kabul etme olasılığı daha zayıf bir bazdan daha fazladır.Bir asidin ve eşlenik bazının gücü ters orantılıdır. Güçlü bir asit çözelti içinde tamamen ayrışır ve ortaya çıkan eşlenik baz bir protonu kabul etmek için çok zayıftır. Aynısı güçlü bir baz ve bunun eşlenik asidi için de geçerlidir.Öte yandan zayıf bir asit, çözelti içinde kısmen ayrışır. Zayıf bir asidin eşlenik bazı da nispeten zayıftır;bu nedenle, çözülmemiş zayıf asit ve onun zayıf eşlenik bazının bir karışımı dengede mevcut olacaktır. Aynı fenomen, zayıf bir baz ve onun zayıf eşlenik asidi durumunda da ortaya çıkar.

<ol>
	<li>Hikaye, David A. "Tezgahtan başucu incelemesi: Klinik asit-bazın kısa bir tarihi." Yoğun Bakım 8, hayır. 4 (2004): 253.</li>
</ol>

bronsted-lowry asitleri ve bazları

Asit-baz reaksiyon sınıfı oldukça uzun bir süredir incelenmiştir. 1680'de Robert Boyle, birçok maddeyi çözme, bazı doğal boyaların renklerini değiştirme ve alkali (baz) çözeltilerle temas ettikten sonra bu özellikleri kaybetme yeteneklerini içeren asit çözeltilerinin özelliklerini bildirdi. On sekizinci yüzyılda, asitlerin ekşi bir tada sahip olduğu, gaz halindeki bir maddeyi (şimdi CO2 olarak bilinir) serbest bırakmak için kireçtaşı ile reaksiyona girdiği ve nötr maddeler oluşturmak için alkalilerle etkileşime girdiği kabul edildi. 1815'te Humphry Davy, hidrojenin asitlerin temel bileşeni olduğunu göstererek modern asit-baz kavramının gelişimine büyük katkıda bulundu. Aynı zamanda, Joseph Louis Gay-Lussac, asitlerin bazları nötralize edebilen maddeler olduğu ve bu iki madde sınıfının sadece birbirleri açısından tanımlanabileceği sonucuna varmıştır. Hidrojenin önemi, 1884 yılında Svante Arrhenius'un bir asidi hidrojen katyonları (şimdi hidronyum iyonları olarak kabul edilir) elde etmek için suda çözünen bir bileşik ve hidroksit anyonları elde etmek için suda çözünen bir bileşik olarak bir baz olarak tanımladığı zaman yeniden vurgulanmıştır.
 
 
 Brønsted-Lowry Asit ve Bazları
 
 
 Johannes Brønsted ve Thomas Lowry, 1923'te asitlerin ve bazların hidrojen iyonlarının H+ transferi açısından tanımlandığı daha genel bir açıklama önerdi. (Bu hidrojen iyonlarına genellikle basitçe protonlar olarak atıfta bulunulduğuna dikkat edin, çünkü bu atom altı parçacık, en bol hidrojen izotopundan, 1 H'den türetilen katyonların tek bileşenidir.) Başka bir bileşiğe Brønsted-Lowry asidi adı verilir ve bir protonu kabul eden bir bileşiğe Brønsted-Lowry bazı adı verilir. Bu nedenle bir asit-baz reaksiyonu, bir protonun bir vericiden (asit) bir alıcıya (baza) aktarılmasıdır.
 
 
 Eşlenik çiftleri kavramı, Brønsted-Lowry asit-baz reaksiyonlarını (ve diğer tersinir reaksiyonları) tanımlamada yararlıdır. Bir asit H+ verdiğinde, geriye kalan türlere asidin eşlenik tabanı denir, çünkü ters reaksiyonda bir proton alıcısı olarak reaksiyona girer. Benzer şekilde, bir baz H+ kabul ettiğinde, eşlenik asidine dönüştürülür. Su ve amonyak arasındaki reaksiyon, bu fikri aşağıda gösterildiği gibi ifade etmektedir.
 
 
  <img alt=""Eq1"" src=""/files/ftp_upload/11394/11394_Equation_1.png"" style=""height: 50px;"" />
 
 
 İleri yönde, su, bir protonu amonyağa bağışlayarak ve daha sonra bir hidroksit iyonu OH−, suyun eşlenik tabanı haline getirerek bir asit görevi görür. Amonyak, bu protonu kabul etmede bir baz görevi görür ve bir amonyum iyonu, NH4+, amonyağın eşlenik asidi haline gelir. Ters yönde, bir hidroksit iyonu, bir asit gibi davranan bir amonyum iyonundan bir protonu kabul etmede bir baz görevi görür.
 
 
 Güçlü asitler ve bazlar bir çözelti içinde tamamen ayrışır. Eşlenik asitler ve bazlar son derece zayıftır ve ters reaksiyonu gerçekleştirmek için sırasıyla protonları bağışlayamaz veya kabul edemez; bu nedenle, güçlü asitler ve bazlar içeren reaksiyonlar esasen sulu bir çözelti içindeyken tamamlanır. Öte yandan, zayıf asitler ve bazlar çözeltilerde kısmen ayrışır ve sırasıyla zayıf eşlenik bazları ve asitleri üretir. Bu zayıf eşlenik asitler veya bazlar ters reaksiyonu gerçekleştirebilir ve böylece zayıf asit ve baz reaksiyonları, zayıf asitlerin ve bazların nispi kuvvetlerine bağlı olarak bir dengeye ulaşır. Özetlemek gerekirse, daha güçlü bir asit eşit derecede zayıf eşlenik bazını üretirken, daha güçlü bir baz eşit derecede zayıf eşlenik asidini üretecektir ve bunun tersi de geçerlidir. Tablo 1, farklı eşlenik asit-baz çiftleri arasındaki ilişkiyi göstermektedir.
 <table style=""margin-left: auto; margin-right: auto;"">
 <tbody>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Güçlü Asit</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Çok Zayıf Eşlenik Baz</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HCl</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Cl−</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HNO3</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">NO3−</td>
 </tr>
 <tr>
 <td colspan=""2""></td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Zayıf Asit</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Zayıf Eşlenik Baz</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">HF</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">F−</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">NH4+</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">NH3</td>
 </tr>
 <tr>
 <td colspan=""2""></td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Çok Zayıf Asit</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Güçlü Eşlenik Baz</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">OH−</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">O2−</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">CH4</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">CH3−</td>
 </tr>
 </tbody>
 </table>
 
 
 Tablo 1: Birkaç eşlenik asit-baz çiftinin nispi gücü.
 
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"">Openstax, Chemistry 2e, Section 14.4 Brønsted-Lowry Acid and Bases</a>."

Bronsted-Lowry Asitleri ve Bazları

Asit-baz reaksiyon sınıfı oldukça uzun bir süredir incelenmektedir. 1680'de Robert Boyle, asit çözeltilerinin özelliklerini bildirdi ve bu da onların ...

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Asitler ve Bazlar

KEY TERMS AND CONCEPTS

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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 bases. In 1884, Svante Arrhenius defined acids as compounds that produce hydrogen cations in water and bases as compounds that produce hydroxide anions.

Brønsted and Lowry gave a broader definition in 1923. A Brønsted-Lowry acid donates a proton, and a Brønsted-Lowry base accepts a proton. An acid-base reaction is the transfer of that proton from the donor to the acceptor. The hydrogen ion, H+, is often called a proton because it is the only particle in the most common hydrogen isotope.

Conjugate pairs help describe these reactions. After an acid donates H+, the species left behind is its conjugate base. After a base accepts H+, it becomes its conjugate acid. Water and ammonia show this clearly. In the forward direction, water donates a proton to ammonia, so water acts as an acid and becomes hydroxide, OH−, while ammonia acts as a base and becomes ammonium, NH4+.

The reverse reaction also fits the same pattern. Hydroxide can accept a proton, so it acts as a base. Ammonium can donate a proton, so it acts as an acid. Strong acids and strong bases dissociate completely in solution, and their conjugate acids and bases are extremely weak. That is why reactions with strong acids and bases in water usually go to completion.

Weak acids and weak bases behave differently. They only partially dissociate in solution and form weak conjugate bases or weak conjugate acids. These conjugate species can take part in the reverse reaction, so weak acid-base reactions reach equilibrium. In general, a stronger acid gives a weaker conjugate base, and a stronger base gives a weaker conjugate acid.

Proton Transfer in Acids and Bases

bronsted-lowry 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

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 Brønsted-Lowry acids and bases work through proton transfer, conjugate pairs, and the difference between strong and weak acid-base reactions.

Proton Transfer in Acids and Bases | JoVE K12

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JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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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 ...

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

Analyze the structure of atoms and isotopes.

Proton Transfer in Acids and Bases

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