Name: water as an amphiprotic substance
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Water: A Bronsted-Lowry Acid and Base

Een amfoteer molecuul kan zowel als zuur als als base werken. Water is een voorbeeld van een amfoteer molecuul. In een waterige oplossing van ammoniak kan water als zuur werken door een proton af te staan aan ammoniak, een base.Water daarentegen werkt als een base in een waterige oplossing van zoutzuur door een proton uit het zuur te accepteren. Omdat het amfoteer is, kan water autoprotolyse ondergaan. In dit proces fungeert één molecuul water als het zuur door een proton af te staan aan een ander watermolecuul dat als basis fungeert door dat proton te accepteren.Dit resulteert in de productie van een hydronium-ion en een hydroxide-ion. De evenwichtsconstante voor de autoprotolyse van water, Kᴡ, ook wel bekend als de autoprotolyseconstante voor water, kan worden uitgedrukt als Kᴡ en heeft een waarde van 1 10⁻¹⁴. De evenwichtsuitdrukking wordt geschreven als de concentratie van de hydronium-ionen maal de concentratie van de hydroxide-ionen, zonder noemer aangezien beide reactanten vloeistoffen zijn.In zuiver water van 25 graden Celsius zijn de concentraties aan hydronium-en hydroxide-ionen gelijk dat wil zeggen 1 10⁻⁷ M.Kᴡ kan worden gebruikt om de concentratie van hydronium-en hydroxide-ionen in een oplossing te berekenen en om te bepalen of een oplossing is zuur of basisch. Als een oplossing zuur is, zal de concentratie van hydronium-ionen hoger zijn dan die van hydroxide-ionen. Als een oplossing daarentegen basisch is, zal de concentratie aan hydroxide-ionen hoger zijn dan de hydronium-ionen.Als de concentratie van hydronium-ionen in oplossing 5 10⁻⁷ M is, kan de hydroxide-ionenconcentratie worden bepaald met Kᴡ.Aangezien de waarden van Kᴡ en hydronium-ionen bekend zijn, kan de concentratie van hydroxide-ionen worden berekend op 2 10⁻⁸ M.Omdat de concentratie aan hydronium-ionen, 5 10⁻⁷ M, hoger is dan de concentratie aan hydroxide-ionen, 2 10⁻⁸ M, is de oplossing zuur.

water: een brønsted-lowry zuur en base

De reactie tussen een Brønsted-Lowry-zuur en water wordt zuurionisatie genoemd. Wanneer waterstoffluoride bijvoorbeeld oplost in water en ioniseert, worden protonen overgebracht van waterstoffluoridemoleculen naar watermoleculen, waardoor hydroniumionen en fluoride-ionen ontstaan:  <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;"> Base-ionisatie van een soort vindt plaats wanneer deze protonen van watermoleculen accepteert. In het onderstaande voorbeeld ondergaan pyridinemoleculen, C5NH5, base-ionisatie wanneer ze worden opgelost in water, wat hydroxide- en pyridiniumionen oplevert:  <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;"> De voorgaande ionisatiereacties suggereren dat water zowel als base (zoals bij de reactie met waterstoffluoride) als als zuur (zoals bij de reactie met ammoniak) kan functioneren. Soorten die protonen kunnen doneren of accepteren, worden amfiprotisch genoemd, of algemener amfoteer, een term die kan worden gebruikt voor zuren en basen volgens andere definities dan die van Brønsted-Lowry. De onderstaande vergelijkingen tonen de twee mogelijke zuur-base-reacties voor twee amfiprotische soorten, bicarbonaationen en water:  <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;"> De eerste vergelijking vertegenwoordigt de reactie van bicarbonaat als zuur met water als base, terwijl de tweede de reactie vertegenwoordigt van bicarbonaat als base met water als zuur. Wanneer bicarbonaat aan water wordt toegevoegd, worden beide evenwichten tegelijkertijd tot stand gebracht en kan de samenstelling van de resulterende oplossing worden bepaald door middel van passende evenwichtsberekeningen. In de vloeibare toestand kunnen moleculen van een amfiprotische stof met elkaar reageren, zoals geïllustreerd voor water in de onderstaande vergelijkingen:  <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;"> Het proces waarbij soortgelijke moleculen reageren en ionen opleveren, wordt auto-ionisatie genoemd. Vloeibaar water ondergaat in zeer geringe mate auto-ionisatie; bij 25 °C zijn ongeveer twee op de miljard watermoleculen geïoniseerd. De omvang van het auto-ionisatieproces van water wordt weerspiegeld in de waarde van de evenwichtsconstante, de ionenproductconstante voor water, KW:  <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;"> De lichte ionisatie van zuiver water wordt weerspiegeld in de kleine waarde van de evenwichtsconstante; bij 25 °C heeft KW een waarde van 1,0 × 10−14.  <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;"> Het proces is endotherm, en dus nemen de mate van ionisatie en de resulterende concentraties hydroniumion en hydroxide-ion toe met de temperatuur. Bij 100 °C is de waarde voor KW bijvoorbeeld ongeveer 5,6 × 10−13, ongeveer 50 keer groter dan de waarde bij 25 °C. De auto-ionisatie van water levert hetzelfde aantal hydronium- en hydroxide-ionen op. Daarom in zuiver water van 25 °C:  <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;"> De concentraties van deze ionen in een oplossing zijn vaak kritische bepalende factoren voor de eigenschappen van de oplossing en het chemische gedrag van de andere opgeloste stoffen, en er is een specifieke woordenschat ontwikkeld om deze concentraties in relatieve termen te beschrijven. Een oplossing is neutraal als deze gelijke concentraties hydronium- en hydroxide-ionen bevat; zuur als het een grotere concentratie hydroniumionen bevat dan hydroxide-ionen; en basisch als het een lagere concentratie hydroniumionen bevat dan hydroxide-ionen. Samenvatting van relaties voor zure, basische en neutrale oplossingen <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Classification</td> <td style="color: black; border: 1px solid black; text-align: center;">Relative Ion Concentrations</td> <td style="color: black; border: 1px solid black; text-align: center;">pH at 25 °C</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">acidic</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;">pH < 7</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">neutral</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;">pH = 7</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">basic</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;">pH > 7</td> </tr> </tbody> </table> Dit tekst is aangepast van<a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chemistry 2e, Sectie 14.1: Brønsted-Lowry-zuren en -basen</a>, en <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Sectie 14.2: pH en pOH</a>.

Water: een Brønsted-Lowry zuur en base

The reaction between a Br&#248;nsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, ...

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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...

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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...

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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, 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...

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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...

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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 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...

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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...

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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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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...

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

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Water as an Amphiprotic Substance

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