Name: salt hydrolysis and ph in solutions
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 4 min 8 s
Channel: JoVE

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Determining the pH of Salt Solutions

Salt solutions can be acidic, basic, or neutral. The individual ions can be examined to determine if the pH of its solution will be below, above, or equal to seven.
Salts that contain pH-neutral cations and anions form neutral solutions. These salts are composed of the counterions of a strong acid and a strong base. A pure aqueous solution of potassium nitrate will have a pH of 7, as neither potassium nor nitrate has acidic or basic properties.
Salts that contain a cation that is the counterion of a weak base and an anion that is the counterion of a strong acid will have a pH less than 7. In a solution of ammonium bromide, the bromide ions are pH neutral, whereas the ammonium ions are acidic and donate protons to the water molecules.
Salts that contain a cation that is the counterion of a strong base and an anion that is the counterion of a weak acid will have a pH greater than 7. In a sodium acetate solution, the sodium ions are pH neutral, whereas the acetate ions are basic and accept protons from the water molecules.
Some salts contain a cation and anion that are counterions of a weak acid and weak base, respectively. The solution will be acidic if the Ka of the cation is larger than the Kb of the anion; basic if the Kb of the anion is larger than the Ka of the cation; or neutral if the Ka and the Kb are equal.
In a solution of ammonium nitrite, the Ka for ammonium is higher than the Kb for nitrite ions; therefore, the solution will be acidic.
The exact pH of a salt solution containing an acidic or basic ion can be determined using the dissociation constant for the conjugate acid or base of that ion.
The pH of 0.35 M sodium cyanide can be determined by calculating the Kb of cyanide from the Ka of its conjugate acid - hydrocyanic acid - and setting up an ICE table to determine the equilibrium concentration. 
As sodium cations do not react with water, they do not affect the pH and can be omitted. In contrast, cyanide ions accept protons from water molecules and generate hydroxide ions.
The Kb for cyanide ions can be determined using the equation: Ka &#215; Kb = KW. As the Ka for hydrocyanic acid is 4.90 &#215; 10&#8722;10, the Kb for cyanide ions is 2.04 &#215; 10&#8722;5.
The Kb is equal to the concentration of hydrocyanic acid times the concentration of hydroxide ions divided by the concentration of cyanide ions.
An ICE table can be constructed to express the initial and equilibrium concentrations. Substituting the equilibrium concentrations into the expression, Kb equals x times x divided by 0.35, which can be verified later by the 5% rule.
Upon solving the equation, x equals 2.7 &#215; 10&#8722;3 molar. As x is only 0.77% of 0.35 M, the approximation 0.35 minus x is equal to 0.35 is valid.
The pOH of the solution can be calculated by taking the negative log of 2.7 &#215; 10&#8722;3 M, which equals 2.57.
The pH of the solution is determined using the equation pH plus pOH is equal to 14; therefore, the pH of this sodium cyanide solution is 11.43.

determining the ph of salt solutions

The pH of a salt solution is determined by its component anions and cations. Salts that contain pH-neutral anions and the hydronium ion-producing cations form a solution with a pH less than 7. For example, in ammonium nitrate (NH4NO3) solution, NO3&#8722; ions do not react with water whereas NH4+ ions produce the hydronium ions resulting in the acidic solution. In contrast, salts that contain pH-neutral cations and the hydroxide ion-producing anions form a solution with a pH greater than 7. For example, in sodium fluoride (NaF) solution, the Na+ is pH-neutral but the F- produces the hydroxide ions and forms the basic solution. The counterions of a strong acid or base are pH-neutral and salts formed by such counterions form a neutral solution with a pH equal to 7. For example, in KBr, The K+ cation is inert and will not affect pH. The bromide ion is the conjugate base of a strong acid, and so it is of negligible base strength (no appreciable base ionization). The solution is neutral.
Some salts contain both an acidic cation and a basic anion. The overall acidity or basicity of a solution is determined by the relative strength of the cation and anion, which can be compared using Ka and Kb. For example, in NH4F, the NH4+ ion is acidic and the F&#8722; ion is basic (conjugate base of the weak acid HF). Comparing the two ionization constants: Ka of NH4+ is 5.6 &#215; 10&#8722;10 and the Kb of F&#8722; is 1.6 &#215; 10&#8722;11, so the solution is acidic, since Ka &#62; Kb.
Calculating the pH of an Acidic Salt Solution
Aniline is an amine that is used to manufacture dyes. It is isolated as anilinium chloride, [C6H5NH3+]Cl, a salt prepared by the reaction of the weak base aniline and hydrochloric acid. What is the pH of a 0.233 M solution of anilinium chloride?
<img alt="Static equilibrium, &#931;Fx=0, &#931;Fy=0 truss diagram; load distribution, forces, support reactions." src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq1" />
The Ka for anilinium ion is derived from the Kb for its conjugate base, aniline:
<img alt="Chemical structure of serotonin molecule, neurotransmitter in nervous system, diagram." src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq2" />
Using the provided information, an ICE table for this system is prepared:
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"></td>
			<td style="color: black; border: 1px solid black; text-align: center;">C6H5NH3+ (aq) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">C6H5NH2 (aq)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Initial Concentration (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.233</td>
			<td style="color: black; border: 1px solid black; text-align: center;">~0</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Change (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#8722;x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Equilibrium Concentration (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.233 &#8722; x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">x</td>
		</tr>
	</tbody>
</table>
Substituting these equilibrium concentration terms into the Ka expression gives
<img alt="Chromatography diagram showing component separation in stationary and mobile phases." src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq3" />
Assuming x &#60;&#60; 0.233, the equation is simplified and solved for x: 
<img alt="Static equilibrium concept; &#931;Fx=0 diagram; force vectors, balance analysis, physics education." src="/files/ftp_upload/11404/11404_Equation_4.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq4" />
<img alt="DNA transcription process diagram showing mRNA synthesis from DNA template." src="/files/ftp_upload/11404/11404_Equation_5.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq5" />
The ICE table defines x as the hydronium ion molarity, and so the pH is computed as
<img alt="Gene editing concept diagram, CRISPR-Cas9 DNA modification process, guide RNA sequence binding." src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq6" />
Hydrolysis of [Al(H2O)6]3+
Calculate the pH of a 0.10 M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion [Al(H2O)6]3+ in solution.
The equation for the reaction and Ka are:
<img alt="Molecular spectroscopy diagram showing energy levels and transitions; absorption and emission arrows." src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq7" />
An ICE table with the provided information is
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"></td>
			<td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)63+ (aq) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)5(OH)2+ (aq)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Initial Concentration (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.10</td>
			<td style="color: black; border: 1px solid black; text-align: center;">~0</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Change (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#8722;x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Equilibrium Concentration (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.10 &#8722; x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">x</td>
			<td style="color: black; border: 1px solid black; text-align: center;">x</td>
		</tr>
	</tbody>
</table>
Substituting the expressions for the equilibrium concentrations into the equation for the ionization constant yields:
<img alt="Ethylene glycol-initiated carbamate formation reaction diagram, chemical synthesis process." src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq8" />
Assuming x &#60;&#60; 0.10 and solving the simplified equation gives:
<img alt="Fourier series formula representation diagram; mathematical expression for periodic functions analysis." src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" data-altupdatedat="1761830439000" data-alt="Eq9" />
The ICE table defined x as equal to the hydronium ion concentration, and so the pH is calculated to be 2.92, and the solution is acidic.
<img alt="Electrophoresis separation diagram; 2D presentation of amino acids; shows amino acid R groups." src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" data-altupdatedat="1761830439000" data-alt="Eq10" />
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>.

The pH of a salt solution is determined by its component anions and cations. Salts that contain pH-neutral anions and the hydronium ion-producing cations ...

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KEY TERMS AND CONCEPTS

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 contain pH-neutral cations and anions that produce hydroxide ions. These salts form basic solutions with pH above 7. Sodium fluoride is an example. In NaF, Na+ is pH-neutral, while F− reacts with water to produce hydroxide ions.

Salts made from the counterions of a strong acid or a strong base are usually neutral. Their solutions have a pH of 7. In KBr, K+ is inert and does not change the pH. Br− is the conjugate base of a strong acid, so it has negligible base strength and does not appreciably ionize in water.

Some salts contain both an acidic cation and a basic anion. In those cases, the overall pH depends on which ion is stronger. The ionization constants Ka and Kb are used to compare them. For NH4F, NH4+ is acidic and F− is basic. Because Ka for NH4+ is 5.6 × 10−10 and Kb for F− is 1.6 × 10−11, the solution is acidic since Ka is greater than Kb.

The pH of an acidic salt solution can be calculated with an ICE table. Anilinium chloride, [C6H5NH3+]Cl, comes from the weak base aniline and hydrochloric acid. For a 0.233 M solution, the Ka value for the anilinium ion is found from the Kb of aniline. The ICE table gives x as the hydronium ion concentration, and the pH is then calculated from that value.

Hydrolysis of the hydrated aluminum ion works the same way. Aluminum chloride dissolves completely to give [Al(H2O)6]3+ in solution. For a 0.10 M solution, the reaction and Ka are set up in an ICE table. After assuming x is much smaller than 0.10 and solving the simplified equation, the hydronium ion concentration gives a pH of 2.92. The solution is acidic.

Salt Hydrolysis and pH in 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...

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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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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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weak base solutions

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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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Salt Hydrolysis and pH of Solutions

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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...

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Learn how salt ions affect pH, from acidic ammonium salts and basic fluoride salts to neutral salts and pH calculations with ICE tables.

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Classifying Matter by State

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Types of Chemical Bonds

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Bonding in Metals

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Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

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Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

IUPAC Nomenclature of Ketones

Like aldehydes, ketones are named using IUPAC rules; in this case, by replacing &#8220;e&#8221; in the name of the longest hydrocarbon chain with ...

IUPAC Nomenclature of Carboxylic Acids

IUPAC names of carboxylic acids are systematically derived following a few rules discussed below.
For acyclic saturated monocarboxylic acids, the longest ...

nomenclature-of-aromatic-compounds-with-a-single-substituent

Nomenclature of Aromatic Compounds with a Single Substituent

Benzene is the simplest aromatic hydrocarbon or arene. The IUPAC names for simple monosubstituted benzene derivatives are derived by adding the ...

nomenclature-of-aromatic-compounds-with-multiple-substituents

Nomenclature of Aromatic Compounds with Multiple Substituents

When more than one substituent is present on the benzene ring, the IUPAC nomenclature depends on the number of substituents present.
For disubstituted ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Salt Hydrolysis and pH in Solutions

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