Name: ph and poh in water
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 41 s
Channel: JoVE

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North Carolina K-12 Science Standard Course of Study

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PS.Chm.6.3

pH Scale

Die Konzentration von Hydronium-Ionen in einer wässrigen Lösung wird normalerweise mit negativen Exponenten geschrieben und kann so klein wie 1 × 10-14 M sein. Die pH-Skala wurde 1909 von dem Chemiker Søren Sorenson entwickelt, um den Säuregehalt verschiedener Lösungen schneller zu vergleichen.
Der pH-Wert einer Lösung ist der negative Logarithmus ihrer Hydroniumionenkonzentration. Zum Beispiel hat eine Lösung mit einer Hydroniumkonzentration von 1 × 10−5 M einen pH-Wert von 5. Je höher die Hydroniumionenkonzentration einer Lösung ist, desto niedriger ist ihr pH-Wert.
Da der pH-Wert auf einer logarithmischen Skala ausgedrückt wird, entspricht eine Änderung um eine Einheit einer 10-fachen Erhöhung oder Abnahme der Hydroniumionenkonzentration. Eine Lösung mit einem pH-Wert von 3 enthält zehnmal mehr Hydronium-Ionen als eine Lösung mit einem pH-Wert von 4 und hundertmal mehr als eine Lösung mit einem pH-Wert von 5.
Eine saure Lösung hat eine höhere Konzentration an Hydroniumionen als Hydroxidionen und einen pH-Wert von weniger als 7, während eine basische Lösung eine niedrigere Konzentration an Hydroniumionen als Hydroxidionen und einen pH-Wert von mehr als 7 aufweist.
Eine neutrale Lösung mit einer gleichen Konzentration an Hydronium- und Hydroxidionen hat einen pH-Wert von 7.
Die Konzentration von Hydroxidionen kann auch als pOH ausgedrückt werden. pOH ist der negative Logarithmus der Hydroxidionenkonzentration. Je höher die Konzentration der Hydroxidionen, desto niedriger ist ihr pOH-Wert.
Der pH- oder pOH-Wert einer wässrigen Lösung liegt zwischen 0 und 14. Dies liegt daran, dass KW, die Gleichgewichtskonstante für die Autoionisation von Wasser, gleich 1 × 10−14 ist. 
Nimmt man den negativen Logarithmus beider Seiten der Gleichung, erhält man eine Gleichung, in der pKW gleich der Summe von pH und pOH ist. Da der negative Logarithmus von 1 × 10−14 14 ist, beträgt die Summe aus pH und pOH einer wässrigen Lösung immer 14. Damit kann bei bekanntem pOH-Wert der pH-Wert bestimmt werden und umgekehrt.
Zum Beispiel hat eine Lösung mit einem pOH von 10 einen pH-Wert von 4.

<ol>
	<li>van Lubeck, Henk. "Warum nicht pH und pOH durch nur einen echten Säuregrad ersetzen, AG?. " Zeitschrift für chemische Bildung 76, Nr. 7 (1999): 892. <a href="https://pubs.acs.org/doi/pdf/10.1021/ed076p892">https://pubs.acs.org/doi/pdf/10.1021/ed076p892</a></li>
</ol>

ph-skala

Hydronium- und Hydroxidionen sind sowohl in reinem Wasser als auch in allen wässrigen Lösungen vorhanden und ihre Konzentrationen sind umgekehrt proportional, bestimmt durch das Ionenprodukt von Wasser (K_w). Die Konzentrationen dieser Ionen in einer Lösung sind häufig entscheidende Faktoren für die Eigenschaften der Lösung und das chemische Verhalten ihrer anderen gelösten Stoffe. Zwei verschiedene Lösungen können sich in ihren Hydronium- oder Hydroxidionenkonzentrationen um das Millionen-, Milliarden- oder sogar Billionenfache unterscheiden. Ein übliches Mittel zur Darstellung von Größen, die sich über viele Größenordnungen erstrecken können, ist die Verwendung einer logarithmischen Skala. Der pH-Wert einer Lösung ist daher wie hier gezeigt definiert, wobei [H_3O^+] die molare Konzentration von Hydroniumionen in der Lösung ist:  <img alt="Eq1" src="/files/ftp_upload/11397/11397_Equation_1.png" style="height: 50px;"> Wenn man diese Gleichung umstellt, um die Molarität der Hydroniumionen zu isolieren, erhält man den äquivalenten Ausdruck:  <img alt="Eq2" src="/files/ftp_upload/11397/11397_Equation_2.png" style="height: 50px;"> Ebenso kann die Hydroxidionenmolarität als p-Funktion oder pOH ausgedrückt werden:  <img alt="Eq3" src="/files/ftp_upload/11397/11397_Equation_3.png" style="height: 50px;"> oder  <img alt="Eq4" src="/files/ftp_upload/11397/11397_Equation4.png" style="height: 50px;"> Schließlich lässt sich die Beziehung zwischen diesen beiden Ionenkonzentrationen, ausgedrückt als p-Funktionen, leicht aus dem K_W-Ausdruck ableiten:  <img alt="Eq5" src="/files/ftp_upload/11397/11397_Equation_5.png" style="height: 135px;"> Bei 25 °C beträgt der Wert von K_W 1,0 × 10^−14, und somit:  <img alt="Eq6" src="/files/ftp_upload/11397/11397_Equation_6.png" style="height: 50px;"> Die Hydroniumionenmolarität in reinem Wasser (oder einer neutralen Lösung) beträgt 1,0 × 10^−7 M bei 25 °C. Der pH-Wert und der pOH-Wert einer neutralen Lösung bei dieser Temperatur betragen daher:  <img alt="Eq7" src="/files/ftp_upload/11397/11397_Equation_7.png" style="height: 95px;"> Bei dieser Temperatur handelt es sich also um saure Lösungen mit Hydroniumionen-Molaritäten von mehr als 1,0 × 10^–7 M und Hydroxidionen-Molaritäten von weniger als 1,0 × 10^–7 M (entsprechend pH-Werten unter 7,00 und pOH-Werten über 7,00). . Basische Lösungen sind solche mit Molaritäten von Hydroniumionen unter 1,0 × 10^–7 M und Molaritäten von Hydroxidionen über 1,0 × 10^–7 M (entsprechend pH-Werten über 7,00 und pOH-Werten unter 7,00). Da die Autoionisationskonstante K_W temperaturabhängig ist, werden diese Korrelationen zwischen pH-Werten und den Adjektiven sauer/neutral/basisch bei anderen Temperaturen als 25 °C unterschiedlich sein. Beispielsweise beträgt die Hydroniummolarität von reinem Wasser bei 80 °C 4,9 × 10^−7 M, was pH- und pOH-Werten von:  <img alt="Eq8" src="/files/ftp_upload/11397/11397_Equation_8.png" style="height: 95px;"> Bei dieser Temperatur weisen neutrale Lösungen einen pH-Wert von pOH = 6,31 auf, saure Lösungen weisen einen pH-Wert von weniger als 6,31 und einen pOH von mehr als 6,31 auf, wohingegen basische Lösungen einen pH-Wert von mehr als 6,31 und einen pOH von weniger als 6,31 aufweisen. Diese Unterscheidung kann wichtig sein, wenn bestimmte Prozesse untersucht werden, die bei anderen Temperaturen ablaufen, beispielsweise Enzymreaktionen in Warmblütern bei einer Temperatur um 36 – 40 °C. Sofern nicht anders angegeben, beziehen sich die Angaben auf pH-Werte auf Werte bei 25 °C. Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"> Openstax, Chemistry 2e, Section 14.2: pH and pOH.</a>

pH-Skala

Hydronium- und Hydroxidionen sind sowohl in reinem Wasser als auch in allen wässrigen Lösungen vorhanden, und ihre Konzentrationen sind umgekehrt proportional zu ...

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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 relationship.

At 25 °C, K w is 1.0 × 10−14. In pure water, or any neutral solution at this temperature, the hydronium ion concentration is 1.0 × 10−7 M. That gives pH = 7.00 and pOH = 7.00.

At 25 °C, acidic solutions have hydronium ion concentrations greater than 1.0 × 10−7 M and hydroxide ion concentrations less than 1.0 × 10−7 M. This means acidic solutions have pH values below 7.00 and pOH values above 7.00. Basic solutions show the opposite pattern, with pH above 7.00 and pOH below 7.00.

The link between pH and acidity changes with temperature because K w changes with temperature. For example, pure water at 80 °C has a hydronium ion concentration of 4.9 × 10−7 M, which gives pH and pOH values of 6.31. At this temperature, neutral solutions have pH = pOH = 6.31, acidic solutions have pH below 6.31, and basic solutions have pH above 6.31.

This temperature effect matters in processes that happen away from 25 °C, including enzyme reactions in warm-blooded organisms at about 36–40 °C. Unless another temperature is stated, pH values are usually assumed to refer to 25 °C.

pH and pOH in Water

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ph scale

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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key terms and concepts

Learn how hydronium and hydroxide ion levels define pH and pOH, why neutral water changes with temperature, and how acidic or basic solutions are identified.

pH and pOH in Water | JoVE K12

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pH and pOH in Water

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