Name: water as an amphiprotic substance
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Water: A Bronsted-Lowry Acid and Base

An amphoteric molecule is capable of acting as both an acid and a base. Water is an example of an amphoteric molecule.
In an aqueous solution of ammonia, water can act as an acid by donating a proton to ammonia, a base. In contrast, water acts as a base in an aqueous solution of hydrochloric acid by accepting a proton from the acid.
Because it is amphoteric, water can undergo autoionization. In this process, one molecule of water acts as the acid by donating a proton to another molecule of water that acts as a base by accepting that proton.
This results in the production of a hydronium ion and a hydroxide ion.
The equilibrium constant for the autoionization of water, KW, also known as the ion-product constant for water, has a value of 1 &#215; 10&#8722;14. Its equilibrium expression is written as the concentration of the hydronium ions times the concentration of the hydroxide ions, with no denominator as both reactants are liquids. 
In pure water at 25 &#176;C, the concentrations of hydronium and hydroxide ions are equal&#8212;that is 1 &#215; 10&#8722;7 M. 
KW can be used to calculate the concentration of hydronium and hydroxide ions in a solution and to determine whether a solution is acidic or basic.
If a solution is acidic, the concentration of hydronium ions will be higher than hydroxide ions. In contrast, if a solution is basic, the concentration of hydroxide ions will be higher than the hydronium ions.
If the concentration of hydronium ions in solution is 5 &#215; 10&#8722;7 M, the hydroxide ion concentration can be determined using KW.
As the values of KW and hydronium ions are known, the concentration of hydroxide ions can be calculated to be 2 &#215; 10&#8722;8 M.
As the hydronium ion concentration, 5 &#215; 10&#8722;7 M, is higher than the hydroxide ion concentration, 2 &#215; 10&#8722;8 M, the solution is acidic.

water: a bronsted-lowry acid and base

The reaction between a Br&#248;nsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
 <img alt="Acid-base equilibrium equation for HF and H2O forming H3O+ and F-, chemical reaction diagram." src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" data-altupdatedat="1754904545000" data-alt="Acid-base reaction diagram with HF, H2O, H3O+, and F- structures; equilibrium process." />
Base ionization of a species occurs when it accepts protons from water molecules. In the example below, pyridine molecules, C5NH5, undergo base ionization when dissolved in water, yielding hydroxide and pyridinium ions:
 <img alt="Acid-base reaction diagram with chemical formulas, showing water and pyridine interaction." src="/files/ftp_upload/11396/11396_image%202v2.svg" style="height: 190px;" data-altupdatedat="1754904545000" data-alt="Acid-base reaction; diagram; H2O and C5NH5 interaction; chemical equilibrium formula; proton transfer." />
The preceding ionization reactions suggest that water may function as both a base (as in its reaction with hydrogen fluoride) and an acid (as in its reaction with ammonia). Species capable of either donating or accepting protons are called amphiprotic, or more generally, amphoteric, a term that may be used for acids and bases per definitions other than the Br&#248;nsted-Lowry one. The equations below show the two possible acid-base reactions for two amphiprotic species, bicarbonate ion, and water:
 <img alt="Science lab safety rules illustration; symbols of PPE, hazard labels, and safety equipment guide." src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" data-altupdatedat="1754904545000" data-alt="static equilibrium equations &#931;Fx=0 &#931;Fy=0 &#931;&#964;=0 free body diagram, forces balance analysis" />
The first equation represents the reaction of bicarbonate as an acid with water as a base, whereas the second represents the reaction of bicarbonate as a base with water as an acid. When bicarbonate is added to water, both these equilibria are established simultaneously and the composition of the resulting solution may be determined through appropriate equilibrium calculations. In the liquid state, molecules of an amphiprotic substance can react with one another as illustrated for water in the equations below:
 <img alt="Chemical equilibrium, H2O as acid and base, reversible reaction formula, acid-base equilibrium." src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" data-altupdatedat="1754904545000" data-alt="Acid-base reaction diagram; water equilibrium, H2O &#8596; H3O+ + OH&#8722;, chemical formula illustration." />
The process in which like molecules react to yield ions is called autoionization. Liquid water undergoes autoionization to a very slight extent; at 25 &#176;C, approximately two out of every billion water molecules are ionized. The extent of the water autoionization process is reflected in the value of its equilibrium constant, the ion-product constant for water, KW:
 <img alt="Chemical structure of serotonin; neurotransmitter diagram with molecular formula C10H12N2O." src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Spectroscopy setup diagram for optical excitation and emission analysis using lenses and mirrors." />
The slight ionization of pure water is reflected in the small value of the equilibrium constant; at 25 &#176;C, KW has a value of 1.0 &#215; 10&#8722;14.
 <img alt="Chemical equilibrium diagram; reaction profile with energy changes, kinetic rates, &#916;H&#8225;, &#916;H." src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Chemical structure of glutamic acid diagram displaying molecular arrangement." />
The process is endothermic, and so the extent of ionization and the resulting concentrations of hydronium ion and hydroxide ion increase with temperature. For example, at 100 &#176;C, the value for KW is about 5.6 &#215; 10&#8722;13, roughly 50 times larger than the value at 25 &#176;C.
The autoionization of water yields the same number of hydronium and hydroxide ions. Therefore, in pure water at 25 &#176;C:
 <img alt="Chemical structure of caffeine; molecular formula C8H10N4O2; structural diagram." src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" data-altupdatedat="1754904545000" data-alt="Magnetic equilibrium; &#931;Fm=0; diagram; pole strength x2a; force calculation method." />
The concentrations of these ions in a solution are often critical determinants of the solution&#8217;s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is neutral if it contains equal concentrations of hydronium and hydroxide ions; acidic if it contains a greater concentration of hydronium ions than hydroxide ions; and basic if it contains a lesser concentration of hydronium ions than hydroxide ions.
Summary of Relations for Acidic, Basic, and Neutral Solutions
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Classification</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Relative Ion Concentrations</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH at 25 &#176;C</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">acidic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] &#62; [OH&#8722;]</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH &#60; 7</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">neutral</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] = [OH&#8722;]</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;">basic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[H3O+] &#60; [OH&#8722;]</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH &#62; 7</td>
		</tr>
	</tbody>
</table>
This text is adapted from<a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chemistry 2e, Section 14.1: Br&#248;nsted-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>.

The reaction between a Br&#248;nsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, ...

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Acids and Bases

KEY TERMS AND CONCEPTS

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 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...

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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...

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...

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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...

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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...

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

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Water as an Amphiprotic Substance

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