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

Sulu bir çözeltideki hidronyum iyonlarının konsantrasyonu genellikle negatif üslerle yazılır ve 1×10⁻¹⁴ M kadar küçük olabilir. PH ölçeği, 1909'da kimyager Soren Sorenson tarafından, farklı çözeltilerin asitliğini hızlı bir şekilde karşılaştırmanın daha uygun bir yolu olarak geliştirilmiştir. Bir çözeltinin pH değeri, hidronyum iyon konsantrasyonunun negatif logaritmasıdır.Örneğin, 1×10⁻⁵ M hidronyum konsantrasyonuna sahip bir çözeltinin pH değeri 5'tir. Bir çözeltinin hidronyum iyon konsantrasyonu ne kadar yüksekse, pH değeri o kadar düşük olur. PH, logaritmik bir ölçekte ifade edildiğinden, tek birimlik bir değişiklik, hidronyum iyon konsantrasyonunun 10 kat artmasına veya azalmasına karşılık gelir.PH değeri 3 olan bir çözelti, pH'ı 4 olan bir çözeltiden on kat, pH'ı 5 olan bir çözeltiden yüz kat daha fazla hidronyum iyonuna sahip olacaktır. Asidik bir çözelti, hidroksit iyonlarından daha yüksek konsantrasyonda hidronyum iyonuna ve 7'den düşük bir pH değerine sahipken, bazik bir çözelti, hidroksit iyonlarından daha düşük bir hidronyum iyon konsantrasyonuna ve 7'den büyük bir pH değerine sahiptir. Eşit konsantrasyonda hidronyum ve hidroksit iyonlarına sahip nötr bir çözeltinin pH değeri 7'dir.Hidroksit iyonlarının konsantrasyonu ayrıca pOH olarak da ifade edilebilir. pOH, hidroksit iyon konsantrasyonunun negatif logaritmasıdır. Hidroksit iyon konsantrasyonu ne kadar yüksekse, pOH değeri o kadar düşüktür.Sulu bir çözeltinin pH veya pOH değeri 0-14 arasında değişir. Bunun nedeni, suyun kendiliğinden iyonlaşması için denge sabiti Kw'nin 1×10⁻¹⁴'e eşit olmasıdır. Denklemin her iki tarafının negatif logaritmasının alınması, pKw'nin pH ve pOH toplamına eşit olduğu bir denklemle sonuçlanır.1×10⁻¹⁴ negatif logu 14 olduğundan, sulu bir çözeltinin pH ve pOH toplamı her zaman 14 olacaktır. Bu, pOH değeri bilindiğinde pH değerini belirlemek için kullanılabilir ve bunun tersi de geçerlidir. Örneğin, pOH değeri 10 olan bir çözeltinin pH değeri 4'tür.

<ol>
	<li>van Lübeck, Henk. "Neden pH ve pOH'yi tek bir gerçek asitlik derecesi olan AG ile değiştirmiyorsunuz? " Kimya Eğitimi Dergisi 76, no. 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 skalası

Hidronyum ve hidroksit iyonları hem saf suda hem de tüm sulu çözeltilerde bulunur ve konsantrasyonları, suyun iyon ürünü (Kw). Bir çözeltideki bu iyonların konsantrasyonları, genellikle çözeltinin özelliklerinin ve diğer çözünenlerin kimyasal davranışlarının kritik belirleyicileridir. İki farklı çözelti hidronyum veya hidroksit iyon konsantrasyonlarında bir milyon, milyar ve hatta trilyon kat farklılık gösterebilir. Pek çok büyüklük sırasına yayılabilen miktarları ifade etmenin yaygın bir yolu, logaritmik ölçek kullanmaktır. Bu nedenle, bir çözeltinin pH'ı, burada gösterildiği gibi tanımlanır; burada [H 3O+], çözeltideki hidronyum iyonunun molar konsantrasyonudur:
 
  <img alt=""Eq1"" src=""/files/ftp_upload/11397/11397_Equation_1.png"" style=""height: 50px;"" />
 
 Hidronyum iyon molaritesini izole etmek için bu denklemi yeniden düzenlemek, eşdeğer ifadeyi verir:
 
  <img alt=""Eq2"" src=""/files/ftp_upload/11397/11397_Equation_2.png"" style=""height: 50px;"" />
 
 Benzer şekilde, hidroksit iyonu molaritesi bir p-fonksiyonu veya pOH olarak ifade edilebilir:
 
  <img alt=""Eq3"" src=""/files/ftp_upload/11397/11397_Equation_3.png"" style=""height: 50px;"" />
 
 ya da
 
  <img alt=""Eq4"" src=""/files/ftp_upload/11397/11397_Equation4.png"" style=""height: 50px;"" />
 
 Son olarak, p-fonksiyonları olarak ifade edilen bu iki iyon konsantrasyonu arasındaki ilişki, KW ifadesinden kolayca türetilebilir:
 
  <img alt=""Eq5"" src=""/files/ftp_upload/11397/11397_Equation_5.png"" style=""height: 135px;"" />
 
 25 °C’de KW’nun değeri 1,0 × 10−14’tür, ve bu yüzden:
 
  <img alt=""Eq6"" src=""/files/ftp_upload/11397/11397_Equation_6.png"" style=""height: 50px;"" />
 
 Saf sudaki (veya herhangi bir nötr çözeltideki) hidronyum iyonu molaritesi 25 °C'de 1,0 × 10−7 M'dir. Bu nedenle, bu sıcaklıkta nötr bir çözeltinin pH'ı ve pOH'sı şu şekildedir:
 
  <img alt=""Eq7"" src=""/files/ftp_upload/11397/11397_Equation_7.png"" style=""height: 95px;"" />
 
 Ve bu nedenle, bu sıcaklıkta, asidik çözeltiler, hidronyum iyon molariteleri 1,0 × 10−7 M'den büyük ve hidroksit iyon molariteleri 1,0 × 10−7 M'den az olanlardır (pH değerleri 7,00'den düşük ve pOH değerleri 7,00'den büyüktür). Bazik çözeltiler, hidronyum iyon molariteleri 1,0 × 10−7 M'den az ve hidroksit iyon molariteleri 1,0 × 10−7 M'den büyük olanlardır (7,00'den büyük pH değerlerine ve 7,00'den düşük pOH değerlerine karşılık gelir).
 
 KW otoiyonizasyon sabiti, sıcaklığa bağlı olduğundan, pH değerleri ile asidik/nötr/bazik sıfatlar arasındaki bu korelasyonlar, 25 °C dışındaki sıcaklıklarda farklı olacaktır. Örneğin, saf suyun 80°C'deki hidronyum molaritesi 4,9 × 10−7 M'dur, aşağıdaki pH ve pOH değerlerine karşılık gelir:
 
  <img alt=""Eq8"" src=""/files/ftp_upload/11397/11397_Equation_8.png"" style=""height: 95px;"" />
 
 Bu sıcaklıkta, nötr çözeltiler pH = pOH = 6,31, asidik çözeltiler 6,31'den düşük pH ve 6,31'den büyük pOH sergilerken, bazik çözeltiler 6,31'den daha yüksek pH ve 6,31'den daha düşük pOH sergiler. Bu ayrım, 36 – 40 °C civarında bir sıcaklıkta sıcak kanlı organizmalarda enzim reaksiyonları gibi diğer sıcaklıklarda meydana gelen belirli süreçleri incelerken önemli olabilir. Aksi belirtilmedikçe, pH değerlerine yapılan atıfların 25 °C'deki referanslar olduğu varsayılır.
 
 Bu metin bu kaynaktan uyarlanmıştır:<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 Skalası

Hidronyum ve hidroksit iyonları hem saf suda hem de tüm sulu çözeltilerde bulunur ve konsantrasyonları ...

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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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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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acid/base strengths and dissociation constants

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lewis acids and bases

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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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