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

Een Arrhenius-zuur is een stof die een hydronium-ion produceert wanneer het in water wordt opgelost, en een Arrhenius-base is een stof die een OH⁻of hydroxide-ion produceert. Zoutzuur is een Arrhenius-zuur omdat het uiteenvalt in een hydronium-ion en een chloride-ion wanneer het in water wordt opgelost. Natriumhydroxide is een Arrhenius-base omdat het dissocieert in een natriumion en een hydroxide-ion wanneer het wordt opgelost in water.Deze definitie kan echter niet worden gebruikt om zuren en basen te beschrijven die zich niet in een waterige oplossing bevinden of basen die geen hydroxide-ionen bevatten. Een bredere definitie van Brønsted en Lowry definieert een zuur als een hydronium-ion of protondonor, terwijl een base een protonacceptor is. Wanneer zoutzuur wordt opgelost in water, werkt het als een zuur door een proton aan water te doneren, waardoor een hydronium-ion en een chloride-ion worden geproduceerd.Wanneer ammoniak wordt opgelost in water, fungeert het als een base en accepteert het een proton uit water, waarbij het een ammoniumion en een hydroxide-ion produceert. Een Brønsted-Lowry-zuur zal altijd reageren met een Brønsted-Lowry-base en vice versa. Wanneer een zuur, bijvoorbeeld azijnzuur, zijn proton afstaat, werkt water als base en accepteert het het proton.Azijnzuur wordt omgezet in een geconjugeerde base, acetaat, en water wordt omgezet in een geconjugeerd zuur, een hydronium-ion. Zuren en basen die van elkaar verschillen door de overdracht van een proton, worden geconjugeerde zuur-basenparen genoemd. In de omgekeerde reactie werkt het geconjugeerde zuur, hydronium, als een protondonor en zal de geconjugeerde base, acetaat, een proton accepteren.De sterkte van een zuur wordt bepaald door zijn vermogen om een proton af te staan, terwijl de sterkte van een base wordt bepaald door zijn vermogen om een proton te accepteren. Een sterker zuur zal eerder een proton afstaan dan een zwakker zuur. Evenzo staat een sterkere basis eerder een proton af dan een zwakkere basis.De sterkte van een zuur en zijn geconjugeerde base zijn omgekeerd evenredig. Een sterk zuur dissocieert volledig in oplossing en de resulterende geconjugeerde base is te zwak om een proton te accepteren. Hetzelfde geldt in het geval van een sterke base en zijn geconjugeerde zuur.Aan de andere kant dissocieert een zwak zuur gedeeltelijk in oplossing. De geconjugeerde base van een zwak zuur is ook relatief zwak;daarom zal een mengsel van het niet-gedissocieerde zwakke zuur en zijn zwakke geconjugeerde base in evenwicht aanwezig zijn. Hetzelfde fenomeen doet zich voor in het geval van een zwakke base en zijn zwak geconjugeerd zuur.

brønsted-lowry-zuren en basen

De zuur-base-reactieklasse wordt al geruime tijd bestudeerd. In 1680 rapporteerde Robert Boyle eigenschappen van zure oplossingen, waaronder hun vermogen om veel stoffen op te lossen, om de kleuren van bepaalde natuurlijke kleurstoffen te veranderen, en om deze eigenschappen te verliezen nadat ze in contact kwamen met alkalische (base) oplossingen. In de achttiende eeuw werd erkend dat zuren een zure smaak hebben, reageren met kalksteen om een gasvormige substantie vrij te maken (nu bekend als CO2) en interageren met alkaliën om neutrale stoffen te vormen. In 1815 heeft Humphry Davy in grote mate bijgedragen aan de ontwikkeling van het moderne zuur-base-concept door aan te tonen dat waterstof het essentiële bestanddeel van zuren is. Rond diezelfde tijd concludeerde Joseph Louis Gay-Lussac dat zuren stoffen zijn die basen kunnen neutraliseren en dat deze twee klassen van stoffen alleen in termen van elkaar kunnen worden gedefinieerd. De betekenis van waterstof werd opnieuw benadrukt in 1884 toen Svante Arrhenius een zuur definieerde als een verbinding die oplost in water om waterstofkationen op te leveren (nu erkend als hydroniumionen) en een base als een verbinding die oplost in water om hydroxide-anionen op te leveren. 

 Brønsted-Lowry-zuren en basen 


 Johannes Brønsted en Thomas Lowry stelden in 1923 een meer algemene beschrijving voor waarin zuren en basen werden gedefinieerd in termen van de overdracht van waterstofionen, H+. (Merk op dat deze waterstofionen vaak eenvoudigweg protonen worden genoemd, aangezien dat subatomaire deeltje de enige component is van kationen die zijn afgeleid van de meest voorkomende waterstofisotoop, 1H.) Een verbinding die een proton aan een andere verbinding doneert, wordt een Brønsted-Lowry genoemd. zuur, en een verbinding die een proton accepteert, wordt een Brønsted-Lowry-base genoemd. Een zuur-base-reactie is dus de overdracht van een proton van een donor (zuur) naar een acceptor (base). 

 Het concept van conjugaatparen is nuttig bij het beschrijven van Brønsted-Lowry zuur-base-reacties (en ook andere omkeerbare reacties). Wanneer een zuur H+ afstaat, wordt de soort die overblijft de geconjugeerde base van het zuur genoemd, omdat het reageert als een protonacceptor in de omgekeerde reactie. Op dezelfde manier wordt een base, wanneer deze H+ accepteert, omgezet in zijn geconjugeerde zuur. De reactie tussen water en ammoniak illustreert dit idee, zoals hieronder weergegeven. 

  <img alt="Eq1" src="/files/ftp_upload/11394/11394_Equation_1.png" style="height: 50px;"> 

 In de voorwaartse richting gedraagt water zich als een zuur door een proton te doneren aan ammoniak en vervolgens een hydroxide-ion te worden, OH-, de geconjugeerde base van water. De ammoniak fungeert als een base bij het accepteren van dit proton en wordt een ammoniumion, NH4+, het geconjugeerde zuur van ammoniak. In de omgekeerde richting fungeert een hydroxide-ion als een base bij het accepteren van een proton van ammoniumion, dat als een zuur werkt. 

 Sterke zuren en basen dissociëren volledig in een oplossing. Hun geconjugeerde zuren en basen zijn extreem zwak en kunnen de protonen niet respectievelijk doneren of accepteren om de omgekeerde reactie uit te voeren; daarom verlopen reacties waarbij sterke zuren en basen betrokken zijn in wezen voltooid wanneer ze zich in een waterige oplossing bevinden. Aan de andere kant dissociëren zwakke zuren en basen gedeeltelijk in oplossingen en produceren respectievelijk zwakke geconjugeerde basen en zuren. Deze zwakke geconjugeerde zuren of basen kunnen de omgekeerde reactie uitvoeren, en dus bereiken reacties van zwakke zuren en basen een evenwicht, afhankelijk van de relatieve sterkte van de zwakke zuren en basen. Samenvattend: een sterker zuur zal de even zwakkere geconjugeerde base produceren, terwijl een sterkere base het even zwakkere geconjugeerde zuur zal produceren en omgekeerd. Tabel 1 geeft de relatie weer tussen verschillende geconjugeerde zuur-base-paren. 

 <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Strong Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Very Weak Conjugate Base</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;">Weak Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Weak Conjugate Base</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;">Very Weak Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Strong Conjugate Base</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> Tabel 1: Relatieve sterkte van enkele geconjugeerde zuur-base-paren. Deze tekst is aangepast van <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 en Basen</a>.

Brønsted-Lowry-zuren en basen

The acid-base reaction class has been studied for quite some time. In 1680, Robert Boyle reported traits of acid solutions that included their ability to ...

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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...

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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...

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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...

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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...

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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...

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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...

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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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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 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...

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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...

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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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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...

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

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Proton Transfer in Acids and Bases

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