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

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

pH Scale

يُكتب تركيز أيونات الهيدرونيوم،في محلول مائي عادة بأرقام أسية سالبة وقد يكون صغيرًا لدرجة 1 10⁻¹⁴ مولار. مقياس الحموضة pH،طوره عالم الكيمياء سورن سورنسون عام 1909،كطريقة أسهل لإجراء مقارنة سريعة بين درجة حموضة المحاليل المختلفة. درجة حموضة محلول ما،هي اللوغاريتم السالب لتركيز أيونات الهيدرونيوم فيه.على سبيل المثال،محلول تركيزه 1 10⁻⁵ مولار تكون درجة حموضته pH 5. كلما زاد تركيز أيونات الهيدرونيوم في المحلول،قلّت درجة حموضته. بما أن درجة الحموضة pH تُمثّل على مقياس لوغاريتمي،فإن تغيير وحدة واحدة يقابله ارتفاع أو انخفاض بمقدار 10 أضعاف في تركيز أيونات الهيدرونيوم.محلول درجة حموضته pH 3 سيحتوي على عشرة أضعاف أيونات هيدرونيوم من محلول درجة حموضته pH 4،ومائة ضعف من محلول درجة حموضته pH 5. تركيز أيونات الهيدرونيوم في محلول حمضي أعلى من تركيز أيونات الهيدروكسيد،ودرجة حموضته أقل من pH 7،بينما يكون تركيز أيونات الهيدرونيوم في محلول قاعدي أقل من تركيز أيونات الهيدروكسيد،وتكون درجة حموضته أعلى من pH 7. المحلول المتعادل الذي يحتوي على تركيزين متساويين من أيونات الهيدرونيوم والهيدروكسيد،تكون درجة حموضته pH 7.يمكن كذلك التعبير عن تركيز أيونات الهيدروكسيد بالرمز pOH. وتساوي اللوغاريتم السالب لتركيز أيونات الهيدروكسيد. كلما ارتفع تركيز أيونات الهيدروكسيد،انخفضت قيمة pOH لتلك الأيونات.قيمة pH أو pOH لمحلول مائي تتراوح بين 0 14. وسبب ذلك أن Kw،ثابت التوازن لتأين الماء التلقائي يساوي 1 10⁻¹⁴. إذا أخذنا اللوغاريتم السالب لطرفي المعادلة،تنتج معادلة يكون فيها pKw مساويًا لكمية pH و pOH.بما أن اللوغاريتم السالب لـ 1 10⁻¹⁴،هو 14،فإن كمية pH و pOH لمحلول مائي ستكون دائمًا 14. يمكن استخدام هذا لتحديد قيمة pH عندما تكون قيمة pOH معروفة والعكس صحيح. على سبيل المثال،محلول فيه قيمة pOH تساوي 10،تكون قيمة pH فيه 4.

<ol>
	<li>فان لوبيك ، هينك. "لماذا لا تستبدل الأس الهيدروجيني ودرجة الأس السموهيدية بدرجة حموضة حقيقية واحدة فقط ، AG؟. "مجلة التربية الكيميائية 76 ، العدد 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>

مقياس درجة الحموضة

توجد أيونات الهيدرونيوم والهيدروكسيد في كل من الماء النقي وفي جميع المحاليل المائية ، وتتناسب تركيزاتهما عكسيًا على النحو الذي يحدده المنتج الأيوني للماء (Kw). غالبًا ما تكون تركيزات هذه الأيونات في محلول محددات حاسمة لخصائص المحلول والسلوك الكيميائي للمذابات الأخرى. يمكن أن يختلف محلولان مختلفان في تركيزات أيونات الهيدرونيوم أو الهيدروكسيد بمليون ، مليار ، أو حتى تريليون مرة. من الوسائل الشائعة للتعبير عن الكميات التي قد تمتد عبر العديد من مراتب الحجم استخدام مقياس لوغاريتمي. لذلك يتم تحديد الرقم الهيدروجيني للحل كما هو موضح هنا ، حيث [H 3 O H3O+] هو التركيز المولي لأيون الهيدرونيوم في المحلول:  <img alt="Eq1" src="/files/ftp_upload/11397/11397_Equation_1.png" style="height: 50px;" /> تؤدي إعادة ترتيب هذه المعادلة لعزل مولارية أيون الهيدرونيوم إلى الحصول على التعبير المكافئ:  <img alt="Eq2" src="/files/ftp_upload/11397/11397_Equation_2.png" style="height: 50px;" /> وبالمثل ، يمكن التعبير عن مولارية أيون الهيدروكسيد كدالة p أو pOH :  <img alt="Eq3" src="/files/ftp_upload/11397/11397_Equation_3.png" style="height: 50px;" />أو <img alt="Eq4" src="/files/ftp_upload/11397/11397_Equation4.png" style="height: 50px;" /> أخيرًا، يمكن اشتقاق العلاقة بين هذين التركيزين الأيونيين المعبر عنه كوظائف p بسهولة من تعبير KW:  <img alt="Eq5" src="/files/ftp_upload/11397/11397_Equation_5.png" style="height: 135px;" /> عند 25 °C، قيمة KW هي 1.0 × 10−14 وهكذا:  <img alt="Eq6" src="/files/ftp_upload/11397/11397_Equation_6.png" style="height: 50px;" /> مولارية أيون الهيدرونيوم في الماء النقي (أو أي محلول محايد) هي 1.0 × 10−7 M عند 25 °C. لذلك فإن الأس الهيدروجيني و الأس الهيدروجيني لمحلول محايد عند درجة الحرارة هذه هما:  <img alt="Eq7" src="/files/ftp_upload/11397/11397_Equation_7.png" style="height: 95px;" /> وهكذا، عند درجة الحرارة هذه، المحاليل الحمضية هي تلك التي تحتوي على مولارية أيونات الهيدرونيوم أكبر من 1.0 × 10−7 M ومولارية أيونات الهيدروكسيد أقل من 1.0 × 10−7 M (المقابلة لقيم الأس الهيدروجيني الأقل من 7.00 وقيم الأس الهيدروجيني أكبر من 7.00). الحلول الأساسية هي تلك التي تحتوي على مولات أيونات الهيدرونيوم أقل من 1.0 × 10−7 M ومولاريات أيونات الهيدروكسيد أكبر من1.0 × 10−7 M (المقابلة لقيم الأس الهيدروجيني الأكبر من 7.00 وقيم الأس الهيدروجيني الأقل من 7.00). نظرًا لأن ثابت التأين التلقائي KW يعتمد على درجة الحرارة، فإن هذه الارتباطات بين قيم الأس الهيدروجيني والصفات الحمضية / المحايدة / الأساسية ستكون مختلفة عند درجات حرارة بخلاف 25 °C على سبيل المثال، مولارية الهيدرونيوم للماء النقي عند 80°C هي 4.9 × 10−7 M، والتي تتوافق مع قيم الأس الهيدروجيني والأس الهيدروجيني لـ:  <img alt="Eq8" src="/files/ftp_upload/11397/11397_Equation_8.png" style="height: 95px;" /> عند درجة الحرارة هذه، تُظهر المحاليل المحايدة pH = pOH = 6.31، وتظهر المحاليل الحمضية pH أقل من 6.31 و pOH أكبر من 6.31، بينما تُظهر المحاليل الأساسية pH أكبر من 6.31 و pOH أقل من 6.31. يمكن أن يكون هذا التمييز مهمًا عند دراسة بعض العمليات التي تحدث في درجات حرارة أخرى ، مثل تفاعلات الإنزيم في الكائنات الحية ذوات الدم الحار عند درجة حرارة حوالي 36 – 40 °C. ما لم يُذكر خلاف ذلك، يُفترض أن الإشارات إلى قيم الأس الهيدروجيني هي تلك الموجودة في 25 °C.تم اقتباس هذا النص من<a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"> Openstax, Chemistry 2e, Section 14.2: pH and pOH.</a>

توجد أيونات الهيدرونيوم والهيدروكسيد في كل من الماء النقي وفي جميع المحاليل المائية ، وتتناسب تركيزاتها عكسيا مع ...

Education

JoVE Core

الكيمياء

واحد

Acids and Bases

الأحماض والقواعد

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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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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...

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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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