Name: acid and base strength in water
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Acid/Base Strengths and Dissociation Constants

Zuren en basen kunnen worden ingedeeld op basis van of ze een sterk zuur, een sterke base, een zwak zuur of een zwakke base zijn. Er zijn zeer weinig sterke zuren en basen, dus de meeste zuren en basen zijn zwak. Een sterk zuur, zoals zoutzuur, valt volledig uiteen in hydronium-ionen en chloride-ionen wanneer het wordt opgelost in water.Een sterke base, zoals natriumhydroxide, dissocieert volledig in natriumionen en hydroxide-ionen. Zwakke zuren en basen dissociëren gedeeltelijk en zijn aanwezig in zowel geïoniseerde als niet-geïoniseerde vormen. Zowel azijnzuur als zijn zwakke geconjugeerde base, acetaat, worden bijvoorbeeld aangetroffen in een waterige oplossing.De mate van dissociatie van een zwak zuur of zwakke base kan worden gemeten aan de hand van de evenwichtsconstante. De evenwichtsconstante voor zwakke zuren heeft een speciale naam, de zuurconstante of, Ka.Voor een generiek zwak zuur HA kan Ka bij een bepaalde temperatuur worden berekend door een evenwichtsvergelijking:de concentratie van producten, A-ion en hydronium-ion, wordt gedeeld door de concentratie van reactanten, HA en water. Omdat water vloeibaar is en de concentratie ervan nagenoeg ongewijzigd blijft tijdens de reactie, wordt het uitgesloten van de vergelijking.Hoe hoger de Ka, hoe sterker het zuur. Salpeterigzuur is sterker dan azijnzuur omdat de Ka van salpeterigzuur groter is dan de Ka van azijnzuur. De evenwichtsconstante voor zwakke basen, de baseconstante, of Kb, werkt op dezelfde manier als Ka.Voor een generieke zwakke base B kan Kb bij een bepaalde temperatuur worden bepaald door de concentratie van producten, BH-ion en hydroxide-ion te delen door de concentratie van reactant B.Net als zuren is ook de sterkte van de basen recht evenredig met de Kb.Ethylamine is bijvoorbeeld relatief sterker dan ureum omdat de Kb van ethylamine groter is dan de Kb van ureum.De sterkte van een zuur kan ook worden uitgedrukt in procent ionisatie. Het percentage ionisatie van zuur kan worden berekend door de hydronium-ionenconcentratie bij evenwicht te delen door de aanvankelijke zuurconcentratie en deze te vermenigvuldigen met honderd. Evenzo kan het ionisatiepercentage voor basen worden berekend door de hydroxide-ionenconcentratie bij evenwicht te delen door de beginconcentratie van base en deze te vermenigvuldigen met honderd.Hoe hoger het ionisatiepercentage, hoe sterker het zuur of de base.

zuur-/basesterkten en dissociatieconstanten

De relatieve sterkte van een zuur of base is de mate waarin het ioniseert wanneer het in water wordt opgelost. Als de ionisatiereactie in wezen voltooid is, wordt het zuur of de base sterk genoemd; als er relatief weinig ionisatie optreedt, is het zuur of de base zwak. Er zijn veel meer zwakke zuren en basen dan sterke. De meest voorkomende sterke zuren en basen staan hieronder vermeld: <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Strong Acids</td> <td style="color: black; border: 1px solid black; text-align: center;">Strong Bases</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HClO4</td> <td style="color: black; border: 1px solid black; text-align: center;">LiOH</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;">NaOH</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HBr</td> <td style="color: black; border: 1px solid black; text-align: center;">KOH</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HI</td> <td style="color: black; border: 1px solid black; text-align: center;">Ca(OH)2</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;">Sr(OH)2</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">H2SO4</td> <td style="color: black; border: 1px solid black; text-align: center;">Ba(OH)2</td> </tr> </tbody> </table> De relatieve sterkten van zuren kunnen worden gekwantificeerd door hun evenwichtsconstanten in waterige oplossingen te meten. In oplossingen met dezelfde concentratie ioniseren sterkere zuren in grotere mate en leveren dus hogere concentraties hydroniumionen op dan zwakkere zuren. De evenwichtsconstante voor een zuur wordt de zuurionisatieconstante, Ka, genoemd. Voor de reactie van een zuur HA: <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;"> de zuurionisatieconstante wordt geschreven als <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;"> waarbij de concentraties die in evenwicht zijn. Hoewel water een reactant is in de reactie, is het ook het oplosmiddel, dus we nemen [H2O] niet op in de vergelijking. Hoe groter de Ka van een zuur, hoe groter de concentratie van H3O+ en A− in verhouding tot de concentratie van het niet-geïoniseerde zuur, HA, in een evenwichtsmengsel, en hoe sterker het zuur. Een zuur wordt geclassificeerd als “sterk” wanneer het volledige ionisatie ondergaat, in welk geval de concentratie van HA nul is en de zuurionisatieconstante onmeetbaar groot is (Ka ≈ ∞). Zuren die gedeeltelijk geïoniseerd zijn, worden 'zwak' genoemd en hun zuurionisatieconstanten kunnen experimenteel worden gemeten. Om dit idee te illustreren worden hieronder drie zuurionisatievergelijkingen en Ka-waarden weergegeven. De ionisatieconstanten nemen toe van de eerste tot de laatste van de vermelde vergelijkingen, wat aangeeft dat de relatieve zuursterkte toeneemt in de volgorde CH3CO2H < HNO2 < HSO4−. <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;"> Een andere maatstaf voor de sterkte van een zuur is het percentage ionisatie. Het percentage ionisatie van een zwak zuur wordt gedefinieerd in termen van de samenstelling van een evenwichtsmengsel: <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;"> waarbij de teller equivalent is aan de concentratie van de geconjugeerde base van het zuur (per stoichiometrie, [A−] = [H3O+]). In tegenstelling tot de Ka-waarde varieert het percentage ionisatie van een zwak zuur met de initiële zuurconcentratie, en neemt doorgaans af naarmate de concentratie toeneemt. Net als bij zuren wordt de relatieve sterkte van een base weerspiegeld in de grootte van de base-ionisatieconstante (Kb) in waterige oplossingen. In oplossingen met dezelfde concentratie ioniseren sterkere basen in grotere mate, en leveren dus hogere hydroxide-ionconcentraties op dan zwakkere basen. Een sterkere base heeft een grotere ionisatieconstante dan een zwakkere base. Voor de reactie van een base, B: <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;"> de ionisatieconstante wordt geschreven als <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;"> De onderstaande inspectie van de gegevens voor drie zwakke basen toont de toename van de basissterkte in de volgorde NO2− < CH2 CO2− < NH3. <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;"> Wat zuren betreft, wordt de relatieve sterkte van een base ook weerspiegeld in het percentage ionisatie ervan, berekend als <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;"> maar zal variëren afhankelijk van de base-ionisatieconstante en de initiële concentratie van de oplossing. Deze tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases">Openstax, Chemistry 2e, Sectie 14.3: Relatieve Sterkten van Zuren en Basen.</a>

Zuur-/basesterkten en dissociatieconstanten

The relative strength of an acid or base is the extent to which it ionizes when dissolved in water. If the ionization reaction is essentially complete, ...

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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.

Acid strength can be measured with the acid-ionization constant, Ka. For an acid HA in water, Ka compares the concentrations of the products and the nonionized acid at equilibrium. Water is a reactant in the reaction, but it is not included in the equation because it is the solvent. A larger Ka means more H3O+ and A− relative to HA, so the acid is stronger.

A strong acid is considered completely ionized. In that case, the concentration of HA is zero, and Ka is immeasurably large, or approximately infinite. Weak acids ionize only partially, so their Ka values can be measured in the lab. The relative acid strengths in the examples increase in the order CH3CO2H &lt; HNO2 &lt; HSO4−.

Percent ionization is another way to describe weak acid strength. It is based on the amount of acid that ionizes at equilibrium. For a weak acid, the percent ionization changes with the starting concentration and usually gets smaller as the concentration gets higher. This makes percent ionization different from Ka.

Base strength is measured in a similar way with the base-ionization constant, Kb. For a base B in water, a larger Kb means the base ionizes more and produces a higher hydroxide ion concentration. A stronger base has a larger ionization constant than a weaker base.

The examples of weak bases show the strength order NO2− &lt; CH2CO2− &lt; NH3. Base strength can also be described with percent ionization. As with weak acids, this value depends on both the base-ionization constant and the initial concentration of the solution.

Acid and Base Strength in Water

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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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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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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

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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Learn how acid and base strength in water depends on ionization, Ka, Kb, and percent ionization, with examples of strong and weak acids and bases.

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Acid and Base Strength in Water

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