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

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Bronsted-Lowry Acids and Bases

Kwas Arrheniusa to substancja, która po rozpuszczeniu w wodzie wytwarza jon wodorowy, a zasada Arrheniusa to substancja, która wytwarza jon OH− lub jon wodorotlenkowy.
Kwas solny jest kwasem Arrheniusa, ponieważ po rozpuszczeniu w wodzie dysocjuje na jon wodorowy i jon chlorkowy. Wodorotlenek sodu jest zasadą Arrheniusa, ponieważ po rozpuszczeniu w wodzie dysocjuje na jon sodu i jon wodorotlenkowy.
Definicja ta nie może być jednak stosowana do opisu kwasów i zasad, które nie znajdują się w roztworze wodnym lub zasad, które nie zawierają jonów wodorotlenkowych.
Szersza definicja Brønsteda i Lowry'ego definiuje kwas jako donor jonów wodorowych lub protonów, podczas gdy zasada jest akceptorem protonów.
Kiedy kwas solny rozpuszcza się w wodzie, działa jak kwas, oddając proton wodzie, wytwarzając jon hydroniowy i jon chlorkowy. Kiedy amoniak rozpuszcza się w wodzie, działa jak zasada i przyjmuje proton z wody, wytwarzając jon amonowy i jon wodorotlenkowy.
Kwas Brønsteda-Lowry'ego zawsze będzie reagował z zasadą Brønsted-Lowry'ego i odwrotnie. Gdy kwas, na przykład kwas octowy, oddaje swój proton, woda działa jak zasada i przyjmuje proton. Kwas octowy jest przekształcany w sprzężoną zasadę, octan, a woda jest przekształcana w sprzężony kwas, jon hydroniowy.
Kwasy i zasady, które różnią się od siebie ze względu na przenoszenie protonu, nazywane są sprzężonymi parami kwasowo-zasadowymi. W reakcji odwrotnej sprzężony kwas, hydroni, działa jako donor protonów, a sprzężona zasada, octan, zaakceptuje proton. 
Siła kwasu zależy od jego zdolności do oddawania protonu, podczas gdy siła zasady zależy od jej zdolności do przyjęcia protonu. Silniejszy kwas jest bardziej skłonny do oddania protonu niż słabszy kwas. Podobnie, silniejsza zasada jest bardziej skłonna zaakceptować proton niż słabsza zasada.
Siła kwasu i jego sprzężona zasada są odwrotnie powiązane. Mocny kwas dysocjuje całkowicie w roztworze, a powstała sprzężona zasada jest zbyt słaba, aby przyjąć proton. To samo dotyczy mocnej zasady i jej sprzężonego kwasu.
Z drugiej strony słaby kwas częściowo dysocjuje w roztworze. Sprzężona zasada słabego kwasu jest również stosunkowo słaba; Dlatego mieszanina niezdysocjowanego słabego kwasu i jego słabej sprzężonej zasady będzie obecna w równowadze. To samo zjawisko występuje w przypadku słabej zasady i jej słabego sprzężonego kwasu.

<ol>
	<li>Historia, David A. "Przegląd od ławki do łóżka: krótka historia klinicznej zasady kwasowej". Critical Care 8, nr 4 (2004): 253.</li>
</ol>

kwasy i zasady bronsteda-lowry’ego

Klasa reakcji kwasowo-zasadowej jest badana od dłuższego czasu. W 1680 roku Robert Boyle opisał cechy roztworów kwasów, w tym ich zdolność do rozpuszczania wielu substancji, zmiany koloru niektórych naturalnych barwników i utraty tych cech po kontakcie z roztworami alkalicznymi (zasadowymi). W XVIII wieku uznano, że kwasy mają kwaśny smak, reagują z wapieniem, uwalniając substancję gazową (obecnie znaną jako CO2) i oddziałują z zasadami, tworząc substancje obojętne. W 1815 roku Humphry Davy w znacznym stopniu przyczynił się do rozwoju nowoczesnej koncepcji kwasowo-zasadowej, wykazując, że wodór jest podstawowym składnikiem kwasów. Mniej więcej w tym samym czasie Joseph Louis Gay-Lussac doszedł do wniosku, że kwasy to substancje, które mogą neutralizować zasady i że te dwie klasy substancji można zdefiniować jedynie w odniesieniu do siebie nawzajem. Znaczenie wodoru zostało ponownie podkreślone w 1884 r., kiedy Svante Arrhenius zdefiniował kwas jako związek, który rozpuszcza się w wodzie, tworząc kationy wodoru (obecnie uznawane za jony hydroniowe), a zasadę jako związek, który rozpuszcza się w wodzie, tworząc aniony wodorotlenkowe.

Kwasy i zasady Brønsteda-Lowry'ego

W 1923 roku Johannes Brønsted i Thomas Lowry zaproponowali bardziej ogólny opis, w którym kwasy i zasady zdefiniowano w kategoriach przenoszenia jonów wodorowych, H+. (Zauważmy, że te jony wodoru są często określane po prostu jako protony, ponieważ ta cząstka subatomowa jest jedynym składnikiem kationów pochodzących z najobficiej występującego izotopu wodoru, 1H). Związek, który przekazuje proton innemu związkowi, nazywany jest Brønstedem-Lowrym kwasem, a związek, który przyjmuje proton, nazywany jest zasadą Brønsteda-Lowry'ego. Reakcja kwasowo-zasadowa polega zatem na przeniesieniu protonu od donora (kwasu) do akceptora (zasady).

Pojęcie par koniugatów jest przydatne w opisywaniu reakcji kwasowo-zasadowych Brønsteda-Lowry'ego (a także innych reakcji odwracalnych). Kiedy kwas oddaje H+, pozostała substancja nazywana jest sprzężoną zasadą kwasu, ponieważ reaguje jako akceptor protonów w reakcji odwrotnej. Podobnie, gdy zasada przyjmuje H+, jest przekształcana w sprzężony kwas. Reakcja wody i amoniaku ilustruje tę ideę, jak pokazano poniżej.

 <img alt="Eq1" src="/files/ftp_upload/11394/11394_Equation_1.png" style="height: 50px;" />

W kierunku do przodu woda działa jak kwas, oddając proton amoniakowi, a następnie stając się jonem wodorotlenkowym OH-, czyli sprzężoną zasadą wody. Amoniak działa jako zasada przyjmująca ten proton, stając się jonem amonowym, NH4+, czyli sprzężonym kwasem amoniaku. W odwrotnym kierunku jon wodorotlenkowy działa jak zasada, przyjmując proton z jonu amonowego, który działa jak kwas.

Silne kwasy i zasady całkowicie dysocjują w roztworze. Ich sprzężone kwasy i zasady są wyjątkowo słabe i nie mogą odpowiednio oddawać ani przyjmować protonów w celu przeprowadzenia reakcji odwrotnej; dlatego reakcje z udziałem mocnych kwasów i zasad zasadniczo kończą się w roztworze wodnym. Z drugiej strony słabe kwasy i zasady częściowo dysocjują w roztworach i wytwarzają odpowiednio słabe sprzężone zasady i kwasy. Te słabe sprzężone kwasy lub zasady mogą przeprowadzić reakcję odwrotną, a zatem reakcje słabego kwasu i zasady osiągają równowagę w zależności od względnej mocy słabych kwasów i zasad. Podsumowując, silniejszy kwas wytworzy równie słabszą sprzężoną zasadę, podczas gdy mocniejsza zasada wytworzy równie słabszy sprzężony kwas i odwrotnie. Tabela 1 przedstawia zależność pomiędzy różnymi sprzężonymi parami kwas-zasada.

<div class="overflow">
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Mocny kwas Bardzo</td>
			<td style="color: black; border: 1px solid black; text-align: center;">słaba zasada koniugatu</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;">Słaby kwas</td>
			<td style="color: black; border: 1px solid black; text-align: center;">słaba zasada koniugatu</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;">Bardzo słaby kwas</td>
			<td style="color: black; border: 1px solid black; text-align: center;">silna zasada koniugatu</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>
</div>

Tabela 1: Siła względna kilku sprzężonych par kwas-zasada.

Kwasy i zasady Bronsteda-Lowry’ego

Klasa reakcji kwasowo-zasadowej jest badana od dłuższego czasu. W 1680 roku Robert Boyle zgłosił cechy roztworów kwasów, które obejmowały ich zdolność do ...

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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

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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...

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...

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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...

ions as acids and bases

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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

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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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:


	...

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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