Name: salt hydrolysis and ph of solutions
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 54 s
Channel: JoVE

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NC K-12 Science Standard Course of Study

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PS.PSc.2.5

Ions as Acids and Bases

Acids, bases, and ionic compounds form anions and cations when they dissolve in water.
Anions that are the conjugate base of strong acids, like chloride formed by the dissociation of hydrochloric acid, are too weak to accept a proton from water. Therefore, chloride ions are pH neutral; that is, they are neither acidic nor basic.
In contrast, anions formed by weak acids, like acetate, the conjugate base of acetic acid, acts as a weak base as it can accept a proton from water.
Cations that are the conjugate acid of strong bases, like sodium ions formed by sodium hydroxide, cannot accept protons and, therefore, are also pH neutral.
In contrast, cations produced by weak bases, like ammonium, the conjugate acid of the ammonia, acts as a weak acid as it can donate protons to water.
When they ionize, salts can produce acidic and basic solutions if they contain a conjugate acid or a conjugate base of a weak acid or base.
Ammonium bromide produces ammonium and bromide ions in water. Bromide ions are pH neutral, whereas ammonium ions act as a weak acid as they can donate protons.
When sodium acetate is dissolved in water, the sodium ions do not react with water; however, the acetate ion can accept a proton&#8212;forming a basic solution.
Salts that contain pH neutral cations and anions form neutral solutions. For example, sodium chloride dissociates into sodium ions and chloride ions when dissolved in water. As both of these ions can neither accept nor donate protons, they form a neutral solution.
Small and highly charged metal ions, like iron(III) and aluminium(III), can also act as weak acids when they become hydrated.
When aluminum(III) is hydrated, it acts as a weak acid and transfers protons from its waters of hydration to the free water molecules, leading to the production of hydronium ions.
The smaller the metal ion and the higher the charges present on it, the greater is its tendency to act as an acid. For example, the Ka for Fe(III) is 6.3 &#215; 10&#8722;3, whereas the Ka for Ni(II) is 2.5 &#215; 10&#8722;11.

ions as acids and bases

Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt&#8217;s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
<img alt="Physics kinematic formulas diagram; equations for motion analysis " src="/files/ftp_upload/11403/11403_Equation_1.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq1" />
The ammonium ion is the conjugate acid of the base ammonia, NH3; its acid ionization (or acid hydrolysis) reaction is represented by
<img alt="DNA replication process diagram with helicase enzyme unwinding double helix strands for duplication." src="/files/ftp_upload/11403/11403_Equation_2.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq2" />
Since ammonia is a weak base, Kb is measurable and Ka &#62; 0 (ammonium ion is a weak acid).
The chloride ion is the conjugate base of hydrochloric acid, and so its base ionization (or base hydrolysis) reaction is represented by
<img alt="Geometry triangle diagram with inscribed circle, tangent radii, angle bisectors, and lines l, t, q." src="/files/ftp_upload/11403/11403_Equation_3.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq3" />
Since HCl is a strong acid, Ka is immeasurably large and Kb &#8776; 0 (chloride ions don&#8217;t undergo appreciable hydrolysis). Thus, dissolving ammonium chloride in water yields a solution of weak acid cations (NH4+) and inert anions (Cl&#8722;), resulting in an acidic solution.
Salts with Basic Ions
As another example, consider dissolving sodium acetate in water:
<img alt="Chromatography system diagram for DNA separation; illustrates flow path and key components." src="/files/ftp_upload/11403/11403_Equation_4.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq4" />
The sodium ion does not undergo appreciable acid or base ionization and has no effect on the solution pH. This may seem obvious from the ion's formula, which indicates no hydrogen or oxygen atoms, but some dissolved metal ions function as weak acids, as addressed later in this section. The acetate ion, CH3CO2&#8722;, is the conjugate base of acetic acid, CH3CO2H, and so its base ionization (or base hydrolysis) reaction is represented by
<img alt="Chemical reaction diagram, Diels-Alder process, cycloaddition mechanism, educational chemistry graphic." src="/files/ftp_upload/11403/11403_Equation_5.png" style="height: 95px;" data-altupdatedat="1761830439000" data-alt="Eq5" />
Because acetic acid is a weak acid, its Ka is measurable and Kb &#62; 0 (acetate ion is a weak base). Dissolving sodium acetate in water yields a solution of inert cations (Na+) and weak base anions (CH3CO2&#8722;), resulting in a basic solution.
Salts with Acidic and Basic Ions
Some salts are composed of both acidic and basic ions, and so the pH of their solutions will depend on the relative strengths of these two species. For such types of salts, a comparison of the Ka and Kb values allows the prediction of the solution&#8217;s acid-base status.
The Ionization of Hydrated Metal Ions
Unlike the group 1 and 2 metal ions of the preceding examples (Na+, Ca2+, etc.), some metal ions function as acids in aqueous solutions. These ions are not just loosely solvated by water molecules when dissolved; instead they are covalently bonded to a fixed number of water molecules to yield a complex ion (see the chapter on coordination chemistry). As an example, the dissolution of aluminum nitrate in water is typically represented as
<img alt="Static equilibrium equations, &#931;Fx=0, MA=0, physics diagram, educational concept." src="/files/ftp_upload/11403/11403_Equation_6.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq6" />
However, the aluminum(III) ion actually reacts with six water molecules to form a stable complex ion, and so the more explicit representation of the dissolution process is
<img alt="Static equilibrium diagram, &#931;Fx=0, beam, forces applied, equilibrium analysis, educational physics." src="/files/ftp_upload/11403/11403_Equation_7.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq7" />
The Al(H2O)63+ ions involve bonds between a central Al atom and the O atoms of the six water molecules. Consequently, the bonded water molecules' O&#8211;H bonds are more polar than in nonbonded water molecules, making the bonded molecules more prone to the donation of a hydrogen ion:
<img alt="Kirchhoff's laws circuit diagram showing resistors, voltage sources, and currents for analysis." src="/files/ftp_upload/11403/11403_Equation_8.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq8" />
The conjugate base produced by this process contains five other bonded water molecules capable of acting as acids, and so the sequential or step-wise transfer of protons is possible as depicted in few equations below:
<img alt="Euler's equations for rotation dynamics, showing torque and angular momentum relations, diagram." src="/files/ftp_upload/11403/11403_Equation_9.png" style="height: 130px;" data-altupdatedat="1761830439000" data-alt="Eq9" />
Aside from the alkali metals (group 1) and some alkaline earth metals (group 2), most other metal ions will undergo acid ionization to some extent when dissolved in water. The acid strength of these complex ions typically increases with increasing charge and decreasing size of the metal ions. The first-step acid ionization equations for a few other acidic metal ions are shown below:
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">First-step Ionization Equations</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pKa</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Fe(H2O)63+ (aq) + H2O (l) &#8652; H3O+ (aq) + Fe(H2O)5(OH)2+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">2.74</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Cu(H2O)62+ (aq) + H2O (l) &#8652; H3O+ (aq) + Cu(H2O)5(OH)+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">~6.3</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"> Zn(H2O)42+ (aq) + H2O (l) &#8652; H3O+ (aq) + Zn(H2O)3(OH)+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;"> 9.6</td>
		</tr>
	</tbody>
</table>
This text is adapted from<a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Chemistry 2e, Section 14.4: Hydrolysis of Salts</a>.

Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization ...

Education

JoVE Core

Chemistry

Acids and Bases

KEY TERMS AND CONCEPTS

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 donate a proton to water. Because ammonia is a weak base, the ammonium ion is a weak acid. The chloride ion is the conjugate base of hydrochloric acid, but HCl is a strong acid, so chloride does not undergo appreciable hydrolysis. The result is an acidic solution.

Sodium acetate shows how a salt can make water basic. Sodium ions do not undergo appreciable acid or base ionization and do not affect pH. The acetate ion is the conjugate base of acetic acid, so it can accept a proton from water. Since acetic acid is a weak acid, acetate is a weak base. Dissolving sodium acetate therefore gives a basic solution.

Some salts contain both acidic and basic ions. For these salts, the pH depends on the relative strengths of the two ions. Comparing Ka and Kb values helps predict whether the solution will be acidic or basic. This is useful when a salt does not have just one ion controlling the pH.

Some metal ions also act as acids in water. Group 1 ions and some group 2 ions, such as Na+ and Ca2+, do not show this behavior. Other metal ions form hydrated complex ions, where the metal is covalently bonded to a fixed number of water molecules. For example, aluminum(III) forms Al(H2O)6 3+, and the bonded water molecules are more likely to donate hydrogen ions.

The acidity of these hydrated metal ions can increase in steps. After one proton is lost, the remaining water ligands can still act as acids. Most metal ions outside the alkali metals and some alkaline earth metals undergo acid ionization to some extent in water. Their acid strength generally increases with higher charge and smaller size. Examples include Fe(H2O)6 3+, Cu(H2O)6 2+, and Zn(H2O)4 2+, which have different pKa values for their first ionization step.

Salt Hydrolysis and pH of Solutions

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 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...

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

relative-strengths-of-conjugate-acid-base-pairs

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...

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 salt hydrolysis affects pH by comparing acidic, basic, and neutral salts, plus hydrated metal ions that can act as weak acids in water.

Salt Hydrolysis and pH of Solutions | JoVE K12

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Salt Hydrolysis and pH of Solutions

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