Name: weak base ph and kb calculations
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 21 s
Channel: JoVE

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North Carolina K-12 Science Standard Course of Study

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Physical Science

Matter and its Interactions

PS.PSc.2.5

Weak Base Solutions

Een zwakke base, zoals ammoniak, is een Brønsted-base die een proton uit water accepteert om het hydroxide-ion te produceren. Zwakke basen reageren gedeeltelijk met water volgens hun baseconstante, Kb, die 1, 76 10⁻⁵ is voor ammoniak. De Kb voor ammoniak kan worden uitgedrukt als de ammoniumionenconcentratie maal de hydroxideionenconcentratie gedeeld door de ammoniakconcentratie bij evenwicht.Kb kan worden gebruikt om de hydroxide-ionenconcentratie in een zwakke baseoplossing te bepalen en daarmee de pOH en pH van de oplossing. De hydroxide-ionenconcentratie en pH van 0, 23 M ammoniakoplossing kunnen worden bepaald aan de hand van de baseconstante en door een ICE-tabel op te stellen met de begin-en evenwichtswaarden van de ammoniak-ammoniumionen en hydroxide-ionen. Als evenwichtsconcentraties in de Kb-uitdrukking worden vervangen, is Kb gelijk aan x keer x gedeeld door 0, 23 min x.Omdat zwakke basen een gedeeltelijke dissociatie vertonen, kan 0, 23 min x worden beschouwd als ongeveer 0, 23. Als de vergelijking is opgelost, is x gelijk aan 2 10⁻³ molair. De benadering 0, 23 min x is gelijk aan 0, 23 is hier geldig aangezien de hydroxide-ionenconcentratie slechts 0, 86%van 0, 23 molair is.Om de pH van deze oplossing te berekenen, moet je eerst de pOH bepalen door de negatieve log van de hydroxide-ionenconcentratie te nemen, die gelijk is aan 2, 70. De pH kan worden bepaald met de formule:pH plus pOH gelijk aan 14 en berekend op 11, 30. De Kb voor een zwakke base-oplossing kan worden berekend als de pH van de zwakke base-oplossing bekend is.Methylamine is een zwakke base die in water gedeeltelijk dissocieert in methylammoniumionen en hydroxide-ionen. De Kb voor methylamine kan worden uitgedrukt als de methylammoniumionconcentratie maal de hydroxide-ionconcentratie gedeeld door de concentratie methylamine bij evenwicht. Om de Kb van een 0, 040 molaire methylamine-oplossing met pH 11, 6 te berekenen, moet eerst de pOH worden berekend, gevolgd door de hydroxide-ionenconcentratie.Omdat de pH 11, 60 is, is de pOH 2, 40 en de hydroxide-ionenconcentratie is 4, 0 10⁻³. De ICE-tabel kan worden samengesteld uit de begin-en evenwichtsconcentraties van methylamine, methylammonium en hydroxide. Het vervangen van evenwichtsconcentraties in de uitdrukking voor de Kb levert een waarde op voor Kb, die 4, 4 10⁻⁴ is.

zwakke basisoplossingen

Sommige verbindingen produceren hydroxide-ionen wanneer ze worden opgelost door chemisch te reageren met watermoleculen. In alle gevallen reageren deze verbindingen slechts gedeeltelijk en worden daarom geclassificeerd als zwakke basen. Dit soort verbindingen zijn ook overvloedig aanwezig in de natuur en zijn belangrijke grondstoffen in verschillende technologieën. De mondiale productie van de zwakke base ammoniak bedraagt bijvoorbeeld doorgaans ruim 100 ton per jaar, en wordt op grote schaal gebruikt als landbouwmeststof, als grondstof voor de chemische synthese van andere verbindingen en als actief ingrediënt in huishoudelijke schoonmaakmiddelen. Wanneer opgelost in water, reageert ammoniak gedeeltelijk en levert hydroxide-ionen op, zoals hier weergegeven: 

 <img alt="Eq1" src="/files/ftp_upload/11401/11401_Equation_1.png" style="height: 50px;"> 

 Dit is per definitie een zuur-base-reactie, in dit geval met de overdracht van H+-ionen van watermoleculen naar ammoniakmoleculen. Onder typische omstandigheden is slechts ongeveer 1% van de opgeloste ammoniak aanwezig als NH4+-ionen. 

 Berekening van hydroxide-ionconcentraties en pOH in een zwakke basisoplossing 

 Zoek de concentratie van het hydroxide-ion, de pOH en de pH van een 0,25 M oplossing van trimethylamine, een zwakke base: 

 <img alt="Eq2" src="/files/ftp_upload/11401/11401_Equation_2.png" style="height: 50px;"> 

 De ICE-tabel voor dit systeem is 

 <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;"></td> <td style="color: black; border: 1px solid black; text-align: center;">(CH3)3N (aq)</td> <td style="color: black; border: 1px solid black; text-align: center;">(CH3)3NH+ (aq) </td> <td style="color: black; border: 1px solid black; text-align: center;">OH− (aq) </td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Initiële Concentratie (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">0.25</td> <td style="color: black; border: 1px solid black; text-align: center;">0</td> <td style="color: black; border: 1px solid black; text-align: center;">~0</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Verandering (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">−x</td> <td style="color: black; border: 1px solid black; text-align: center;">+x</td> <td style="color: black; border: 1px solid black; text-align: center;">+x</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Evenwichtsconcentratie (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">0.25 − x</td> <td style="color: black; border: 1px solid black; text-align: center;">0 + x</td> <td style="color: black; border: 1px solid black; text-align: center;">~0 + x</td> </tr> </tbody> </table> 


 Het vervangen van de evenwichtsconcentratietermen in de Kb expressie levert op 

 <img alt="Eq3" src="/files/ftp_upload/11401/11401_Equation_3.png" style="height: 90px;"> 

 Aangenomen dat x << 0.25 is en x oplost, levert dit op 

 <img alt="Eq4" src="/files/ftp_upload/11401/11401_Equation_4.png" style="height: 50px;"> 

 Deze waarde is minder dan 5% van de initiële concentratie (0.25), dus de aanname is gerechtvaardigd. 

 Zoals gedefinieerd in de ICE-tabel is x gelijk aan de evenwichtsconcentratie van hydroxide-ionen: 

 <img alt="Eq5" src="/files/ftp_upload/11401/11401_Equation_5.png" style="height: 50px;"> 

 De pOH wordt zo berekend 

 <img alt="Eq6" src="/files/ftp_upload/11401/11401_Equation_6.png" style="height: 50px;"> 

 De relatie gebruiken; 

 <img alt="Eq7" src="/files/ftp_upload/11401/11401_Equation_7.png" style="height: 50px;"> 

 maakt de berekening van de pH mogelijk: 

 <img alt="Eq8" src="/files/ftp_upload/11401/11401_Equation_8.png" style="height: 50px;"> 

 Bepaling van Kb uit pH 

 Als de pH van een 0.28 M oplossing van ethylamine (C2H5NH2) 12.10 is, wat is dan de Kb ervan? 

 <img alt="Eq9" src="/files/ftp_upload/11401/11401_Equation_9.png" style="height: 50px;"> 

 Om de Kb van ethylamine te berekenen, moeten eerst de pOH en de hydroxide-ionenconcentratie worden bepaald. Omdat de pH 12.10 is, kan de pOH als volgt worden berekend: 

 <img alt="Eq10" src="/files/ftp_upload/11401/11401_Equation_10.png" style="height: 50px;"> 

 Omdat de pOH 1.90 is, kan de hydroxide-ionenconcentratie van de oplossing worden berekend met behulp van de formule 

 <img alt="Eq11" src="/files/ftp_upload/11401/11401_Equation_11.png" style="height: 50px;"> 

 De ICE-tafel kan voor dit systeem als volgt worden opgebouwd 

 <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;"></td> <td style="color: black; border: 1px solid black; text-align: center;">C2H5NH2 (aq)</td> <td style="color: black; border: 1px solid black; text-align: center;">C2H5NH3+ (aq)</td> <td style="color: black; border: 1px solid black; text-align: center;">OH− (aq)</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Initiële Concentratie (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">0.28</td> <td style="color: black; border: 1px solid black; text-align: center;">0</td> <td style="color: black; border: 1px solid black; text-align: center;">~0</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Verandering (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">−0.0126</td> <td style="color: black; border: 1px solid black; text-align: center;">+0.0126</td> <td style="color: black; border: 1px solid black; text-align: center;">+0.0126</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Evenwichtsconcentratie (M)</td> <td style="color: black; border: 1px solid black; text-align: center;">0.28 − 0.0126</td> <td style="color: black; border: 1px solid black; text-align: center;">0.0126</td> <td style="color: black; border: 1px solid black; text-align: center;">0.0126</td> </tr> </tbody> </table> 

 Aangezien de 0.0126 M 4.5% van 0.28 M is, kan 0.28 − 0.0126 door de 5%-regel als bijna gelijk aan 0.28 M worden beschouwd. 

 Na vervanging van de bovenstaande waarden in de uitdrukking voor de Kb van ethylamine, 

 <img alt="Eq12" src="/files/ftp_upload/11401/11401_Equation_12.png" style="height: 90px;">

Zwakke basisoplossingen

Some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. In all cases, these compounds react only partially and ...

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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 chemical synthesis, and an ingredient in household cleaners.

When ammonia dissolves in water, it reacts only partially to form hydroxide ions. This is an acid-base reaction because H+ ions move from water molecules to ammonia molecules. Under typical conditions, only about 1% of the dissolved ammonia is present as NH4+ ions.

The video also shows how to calculate hydroxide ion concentration, pOH, and pH for a weak base solution. For a 0.25 M trimethylamine solution, an ICE table is used to track initial, change, and equilibrium concentrations. The Kb expression is then written with the equilibrium terms, and the x &lt;&lt; 0.25 assumption is checked with the 5% rule before solving for x as the hydroxide ion concentration. From there, pOH is found and pH is calculated.

A second example shows how to determine Kb from pH. For a 0.28 M ethylamine solution with a pH of 12.10, the pOH is first found, then the hydroxide ion concentration is calculated. An ICE table is built for ethylamine, ethylammonium ion, and hydroxide ion. After applying the 5% rule, the values are substituted into the Kb expression to find the base dissociation constant.

Weak Base pH and Kb Calculations

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Proton Transfer in Acids and Bases

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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...

weak base solutions

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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key terms and concepts

Learn how weak bases form hydroxide ions, then use ICE tables to find pOH, pH, and Kb for trimethylamine and ethylamine examples.

Weak Base pH and Kb Calculations | JoVE K12

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Understand types, properties, and structure of matter.

Weak Base pH and Kb Calculations

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