Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 30 s
Channel: JoVE

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Water: A Bronsted-Lowry Acid and Base

양쪽성 분자는 산과 염기 모두의 역할을 할 수 있습니다. 물은 양쪽성 분자의 한 예입니다. 암모니아 수용액에서 물은 염기인 암모니아에 양성자를 기증함으로써 산의 역할을 할 수 있습니다.

대조적으로 물은 산에서 양성자를 받아들임으로써 염산 수용액에서 염기 역할을 합니다. 물은 양쪽성이기 때문에 자동 이온화될 수 있습니다. 이 과정에서 한 분자의 물은 그 양성자를 받아들여 염기 역할을 하는 물의 다른 분자에 양성자를 기증함으로써 산의 역할을 합니다.

이 과정에 하이드로늄 이온과 수산화 이온을 생성하게 됩니다. 물의 자동 이온화를 위한 평형 상수인 Kᴡ를 물의 이온곱 상수라고도 하며, Kᴡ로 표현할 수 있으며 값은10의 마이너스 14승입니다. 평형식은 하이드로늄 이온의 농도와 수산화 이온의 농도로 작성되며 두 반응물이 액체이기 때문에 분모가 없습니다.

섭씨 25도의 순수한 물에서 하이드로늄 이온과 수산화 이온의 농도는 같습니다. 즉 10의 마이너스 7승입니다. Kᴡ를 사용하여 용액 내 하이드로늄 이온과 수산화 이온의 농도를 계산하고 용액이 산성인지 또는 염기인지를 결정할 수 있습니다.

만약 용액이 산성이라면 하이드로늄 이온의 농도는 수산화 이온보다 높을 것입니다. 반대로 용액이 염기라면 수산화 이온의 농도는 하이드로늄 이온보다 더 높을 것입니다. 용액 내 하이드로늄 이온 농도가 5 곱하기 10의 마이너스 7승 몰농도이면 Kᴡ를 이용하여 수산화 이온 농도를 결정할 수 있습니다.

Kᴡ와 하이드로늄 이온의 값을 알기 때문에 수산화 이온의 농도는 2 곱하기 10의 마이너스 8승 몰농도로 계산될 수 있습니다. 하이드로늄 이온 농도가 5 곱하기 10의 마이너스 7승 몰농도로 수산화 이온 농도 2 곱하기 10의 마이너스 8승 몰농도보다 높기 때문에 용액은 산성입니다.

물: 브뢴스테드-로우리 산과 염기

브뢴스테드-로우리 산과 물 사이의 반응을 산 이온화라고 합니다. 예를 들어, 불화수소가 물에 용해되어 이온화되면 양성자가 불화수소 분자에서 물 분자로 이동하여 하이드로늄 이온과 불화물 이온이 생성됩니다.

 <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />

종의 염기 이온화는 물 분자로부터 양성자를 받아들일 때 발생합니다. 아래 예에서 피리딘 분자 C_5NH_5는 물에 용해되면 염기 이온화를 거쳐 수산화물 이온과 피리디늄 이온을 생성합니다.

 <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />

앞의 이온화 반응은 물이 염기(불화수소와의 반응에서처럼)와 산(암모니아와의 반응에서처럼)으로 기능할 수 있음을 시사합니다. 양성자를 기증하거나 수용할 수 있는 종을 양쪽성(amphiprotic)이라고 부르며, 더 일반적으로는 양쪽성(amphoteric)이라고 하며, 이 용어는 브뢴스테드-로우리 정의 이외의 정의에 따라 산과 염기에 사용될 수 있습니다. 아래 방정식은 두 가지 양친성 종, 중탄산염 이온 및 물에 대해 가능한 두 가지 산-염기 반응을 보여줍니다.

 <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />

첫 번째 방정식은 산인 중탄산염과 염기인 물의 반응을 나타내고, 두 번째 방정식은 염기인 중탄산염과 산인 물의 반응을 나타냅니다. 중탄산염을 물에 첨가하면 두 평형이 동시에 이루어지며 결과 용액의 조성은 적절한 평형 계산을 통해 결정될 수 있습니다. 액체 상태에서 양쪽성 물질의 분자는 아래 방정식에서 물에 대해 설명된 것처럼 서로 반응할 수 있습니다.

 <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />

유사한 분자가 반응하여 이온을 생성하는 과정을 자동 이온화라고 합니다. 액체 물은 아주 약간의 자동 이온화를 겪습니다. 25°C에서는 물 분자 10억 개 중 약 2개가 이온화됩니다. 물의 자동 이온화 과정의 정도는 평형 상수, 즉 물의 이온-곱 상수 K_W 값에 반영됩니다.

 <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />

순수한 물의 약간의 이온화는 평형 상수의 작은 값에 반영됩니다. 25°C에서 K_W의 값은 1.0 × 10^−14입니다.

 <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />

이 과정은 흡열이므로 온도에 따라 이온화 정도와 하이드로늄 이온 및 수산화물 이온의 농도가 증가합니다. 예를 들어, 100°C에서 K_W 값은 약 5.6 × 10^−13이며, 이는 25°C에서의 값보다 대략 50배 더 큽니다.

물의 자동 이온화는 동일한 수의 하이드로늄 및 수산화물 이온을 생성합니다. 따라서 25°C의 순수한 물에서는 다음과 같습니다.

 <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />

용액 내 이러한 이온의 농도는 종종 용액의 특성과 다른 용질의 화학적 거동을 결정하는 중요한 요소이며 이러한 농도를 상대적인 용어로 설명하기 위해 특정 용어가 개발되었습니다. 동일한 농도의 하이드로늄과 수산화물 이온을 포함하는 경우 용액은 중성입니다. 수산화물 이온보다 더 높은 농도의 하이드로늄 이온을 포함하면 산성이고; 수산화물 이온보다 낮은 농도의 하이드로늄 이온을 포함하는 경우 염기성입니다.

산성, 염기성 및 중성 용액의 관계 요약

<div class="overflow">
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">분류</td>
			<td style="color: black; border: 1px solid black; text-align: center;">상대 이온 농도</td>
			<td style="color: black; border: 1px solid black; text-align: center;">25 °C에서 pH</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">산 성</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;">중립</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;">기본</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>
</div>

이 문서는 에서 발췌되었습니다 <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>, and <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Section 14.2: pH and pOH</a>.

Brønsted-Lowry 산과 물 사이의 반응을 산 이온화라고 합니다. 예를 들어, 불화수소가 물에 용해되어 이온화되면 ...

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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...

ph scale

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...

relative strengths of conjugate acid-base pairs

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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...

strong acid and base solutions

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...

weak acid solutions

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...

weak base solutions

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...

mixtures of acids

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...

ions as acids and bases

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...

determining the ph of salt solutions

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

acidbase-strengths-and-dissociation-constants

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...

lewis acids and bases

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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As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Water as an Amphiprotic Substance

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