Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 30 s
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Water: A Bronsted-Lowry Acid and Base

Amfoterik bir molekül, hem asit hem de baz görevi görebilir. Su, amfoterik bir molekül örneğidir. Sulu bir amonyak çözeltisinde su, bir baz olan amonyağa bir proton vererek bir asit görevi görebilir.Bunun aksine su, asitten bir protonu kabul ederek sulu bir hidroklorik asit çözeltisinde bir baz görevi görür. Amfoterik olduğu için su, otoiyonizasyona uğrayabilir. Bu süreçte bir su molekülü, bu protonu kabul ederek baz görevi gören başka bir su molekülüne bir proton vererek asit görevi görür.Bu, bir hidronyum iyonu ve bir hidroksit iyonunun üretilmesiyle sonuçlanır. Su için iyon-ürün sabiti olarak da bilinen suyun otoiyonizasyonu denge sabiti Kᴡ, Kᴡ olarak ifade edilebilir ve 1×10⁻¹⁴ değerine sahiptir. Denge ifadesi, her iki reaktan da sıvı olduğundan payda olmaksızın hidronyum iyonlarının konsantrasyonu çarpı hidroksit iyonlarının konsantrasyonu olarak yazılır.25 Santigrat derecedeki saf suda, hidronyum ve hidroksit iyonlarının konsantrasyonları eşittir yani 1×10⁻⁷ M'dir. Kᴡ, bir çözeltideki hidronyum ve hidroksit iyonlarının konsantrasyonunu hesaplamak ve bir çözeltinin asidik mi yoksa bazik mi olduğunu belirlemek için kullanılabilir. Bir çözelti asidik ise, hidronyum iyonlarının konsantrasyonu hidroksit iyonlarından daha yüksek olacaktır.Aksine, bir çözelti bazik ise, hidroksit iyonlarının konsantrasyonu hidronyum iyonlarından daha yüksek olacaktır. Çözeltideki hidronyum iyonlarının konsantrasyonu 5×10⁻⁷ M ise, hidroksit iyon konsantrasyonu Kᴡ kullanılarak belirlenebilir. Kᴡ ve hidronyum iyonlarının değerleri bilindiğinden, hidroksit iyonlarının konsantrasyonu 2×10⁻⁸ M olarak hesaplanabilir.Hidronyum iyon konsantrasyonu, 5 10⁻⁷ M, hidroksit iyon konsantrasyonundan daha yüksek olduğundan, çözelti asidiktir.

su: bir bronsted-lowry asidi ve bazı

Bir Bronsted-Lowry asidi ile su arasındaki reaksiyona asit iyonizasyonu denir. Örneğin, hidrojen florür suda çözündüğünde ve iyonize olduğunda, protonlar hidrojen florür moleküllerinden su moleküllerine aktarılır ve bu da hidronyum iyonları ve florür iyonları verir:
 
  <img alt=""Image1"" src=""/files/ftp_upload/11396/11396_Image_1.svg"" style=""height: 125px;"" />
 
 Bir türün baz iyonlaşması, su moleküllerinden protonları kabul ettiğinde meydana gelir. Aşağıdaki örnekte, piridin molekülleri, C5NH5, suda çözündüklerinde baz iyonizasyonuna uğrayarak hidroksit ve piridinyum iyonları verir:
 
  <img alt=""Image2"" src=""/files/ftp_upload/11396/11396_image 2v2.svg"" style=""height: 190px;"" />
 
 Önceki iyonlaşma reaksiyonları, suyun hem bir baz (hidrojen florürle reaksiyonunda olduğu gibi) hem de bir asit (amonyakla reaksiyonunda olduğu gibi) olarak işlev görebileceğini göstermektedir. Protonları bağışlayabilen veya kabul edebilen türlere amfiprotik veya daha genel olarak amfoterik denir ve Brønsted-Lowry dışındaki tanımlara göre asitler ve bazlar için kullanılabilen bir terimdir. Aşağıdaki denklemler, iki amfiprotik tür, bikarbonat iyonu ve su için iki olası asit-baz reaksiyonunu göstermektedir:
 
  <img alt=""Equation1"" src=""/files/ftp_upload/11396/11396_Equation_1.png"" style=""height: 95px;"" />
 
 İlk denklem bikarbonatın bir asit olarak su ile bir baz olarak reaksiyonunu temsil ederken, ikincisi bikarbonatın bir asit olarak su ile bir baz olarak reaksiyonunu temsil eder. Suya bikarbonat eklendiğinde, bu iki denge aynı anda kurulur ve elde edilen çözeltinin bileşimi uygun denge hesaplamaları ile belirlenebilir. Sıvı halde, amfiprotik bir maddenin molekülleri, aşağıdaki denklemlerde su için gösterildiği gibi birbirleriyle reaksiyona girebilir:
 
  <img alt=""Image3"" src=""/files/ftp_upload/11396/11396_image_3.svg"" style=""height: 125px;"" />
 
 Benzer moleküllerin iyon vermek üzere reaksiyona girdiği sürece otoiyonizasyon denir. Sıvı su, çok az oranda otoiyonizasyona uğrar; 25 °C'de, her milyar su molekülünden yaklaşık ikisi iyonize olur. Su otoiyonizasyon işleminin kapsamı, denge sabitinde, su için iyon-ürün sabitinde, KW ifade edilir:
 
  <img alt=""Equation2"" src=""/files/ftp_upload/11396/11396_Equation_2.png"" style=""height: 50px;"" />
 
 Saf suyun hafif iyonlaşması, denge sabitinin küçük değerinde ifade edilir; 25 °C'de, KW, 1,0 × 10−14 değerine sahiptir.
 
  <img alt=""Equation3"" src=""/files/ftp_upload/11396/11396_Equation_3.png"" style=""height: 50px;"" />
 
 Süreç endotermiktir ve bu nedenle iyonlaşma derecesi ve sonuçta ortaya çıkan hidronyum iyonu ve hidroksit iyonu konsantrasyonları sıcaklıkla artar. Örneğin, 100 °C'de, KW değeri yaklaşık 5,6 × 10−13'tür, 25 °C'deki değerden kabaca 50 kat daha büyüktür.
 
 Suyun otoiyonizasyonu, aynı sayıda hidronyum ve hidroksit iyonu verir. Bu nedenle 25 °C'de saf suda:
 
  <img alt=""Equation4"" src=""/files/ftp_upload/11396/11396_Equation_4.png"" style=""height: 50px;"" />
 
 Bir solüsyondaki bu iyonların konsantrasyonları, genellikle solüsyonun özelliklerinin ve diğer çözünenlerin kimyasal davranışlarının kritik belirleyicileridir ve bu konsantrasyonları göreceli terimlerle açıklamak için özel kelime dağarcığı geliştirilmiştir. Bir çözelti, eşit konsantrasyonlarda hidronyum ve hidroksit iyonları içeriyorsa nötrdür; hidroksit iyonlarından daha fazla konsantrasyonda hidronyum iyonları içeriyorsa asidiktir; ve hidroksit iyonlarından daha az konsantrasyonda hidronyum iyonları içeriyorsa baziktir.
 
 Asidik, Bazik ve Nötr Çözeltiler için İlişkilerin Özeti
 <table style=""margin-left: auto; margin-right: auto;"">
 <tbody>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Sınıflandırma</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Bağıl İyon Konsantrasyonları</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">25 °C’de pH</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">asidik</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">[H3O+] > [OH−]</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">pH < 7</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">nötr</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">[H3O+] = [OH−]</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">pH = 7</td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">bazik</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">[H3O+] < [OH−]</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">pH>7</td>
 </tr>
 </tbody>
 </table>
 
 Bu metin bu kaynaklardan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases""> Openstax, Chemistry 2e, Section 14.1: Brønsted-Lowry Acids and Bases</a>, ve <a href=""https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"">Section 14.2: pH and pOH</a>.

Su: Bir Bronsted-Lowry Asidi ve Bazı

Bir Brønsted-Lowry asidi ile su arasındaki reaksiyona asit iyonizasyonu denir. Örneğin, hidrojen florür suda çözündüğünde ve iyonlaştığında, ...

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water as an amphiprotic substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions.

Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions.

These reactions show that water can play either role. A substance that can donate or accept protons is called amphiprotic. The broader term amphoteric is also used for substances that can act as acids or bases under different definitions. Bicarbonate ion is another amphiprotic species. It can react with water as an acid or as a base, and both equilibria can be present at the same time in solution.

Liquid water can also react with itself. This process is called autoionization. It happens only to a very small extent. At 25 °C, about two out of every billion water molecules are ionized. The equilibrium constant for this process is the ion-product constant for water, K_w, and its value is 1.0 × 10^-14 at 25 °C.

Autoionization is endothermic, so more ionization occurs as temperature rises. At 100 °C, K_w is about 5.6 × 10^-13, which is roughly 50 times larger than at 25 °C. Pure water always produces equal amounts of hydronium and hydroxide ions through this process. A solution is neutral when these ion concentrations are equal. It is acidic when hydronium ion concentration is greater than hydroxide ion concentration, and basic when hydroxide ion concentration is greater. At 25 °C, acidic solutions have pH below 7, neutral solutions have pH 7, and basic solutions have pH above 7.

Water as an Amphiprotic Substance

bronsted-lowry acids and bases

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...

water: a bronsted-lowry acid and base

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

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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...

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How Ka and Kb Show Acid-Base Strength

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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Strong Acids, Strong Bases, and pH

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

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Weak Acid Equilibrium in Water

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...

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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...

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pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

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Salt Hydrolysis and pH of Solutions

Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

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Salt Hydrolysis and pH in Solutions

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

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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. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

acid strength and molecular structure

How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

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Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how water can act as both an acid and a base, why it is amphiprotic, and how autoionization affects hydronium, hydroxide, and pH.

Water as an Amphiprotic Substance | JoVE K12

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Water as an Amphiprotic Substance

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