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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Physical Science

Matter and its Interactions

PS.PSc.2.5

Determining the pH of Salt Solutions

Roztwory soli mogą być kwaśne, zasadowe lub obojętne. Poszczególne jony można zbadać, aby określić, czy pH jego roztworu będzie poniżej, powyżej lub równe siedmiu.
Sole zawierające kationy i aniony o neutralnym pH tworzą obojętne roztwory. Sole te składają się z przeciwjonów mocnego kwasu i mocnej zasady. Czysty wodny roztwór azotanu potasu będzie miał pH 7, ponieważ ani potas, ani azotan nie mają właściwości kwaśnych ani zasadowych.
Sole, które zawierają kation, który jest przeciwjonem słabej zasady i anion, który jest przeciwjonem mocnego kwasu, będą miały pH mniejsze niż 7. W roztworze bromku amonu jony bromkowe mają pH neutralne, podczas gdy jony amonowe są kwaśne i oddają protony cząsteczkom wody.
Sole zawierające kation, który jest przeciwjonem mocnej zasady i anion, który jest przeciwjonem słabego kwasu, będą miały pH większe niż 7. W roztworze octanu sodu jony sodu mają pH neutralne, podczas gdy jony octanowe są zasadowe i przyjmują protony z cząsteczek wody.
Niektóre sole zawierają kation i anion, które są przeciwjonami odpowiednio słabego kwasu i słabej zasady. Roztwór będzie kwaśny, jeśli Ka kationu jest większe niż Kb anionu; zasadowy, jeżeli Kb anionu jest większy niż Ka kationu; lub neutralny, jeśli Ka i Kb są równe.
W roztworze azotynu amonu Ka dla amonu jest wyższe niż Kb dla jonów azotynowych, dlatego roztwór będzie kwaśny.
Dokładne pH roztworu soli zawierającego jon kwasowy lub zasadowy można określić za pomocą stałej dysocjacji sprzężonego kwasu lub zasady tego jonu.
pH 0,35 M cyjanku sodu można oznaczyć, obliczając Kb cyjanku z Ka jego sprzężonego kwasu - kwasu cyjanowodorowego - i ustawiając tabelę ICE w celu określenia stężenia równowagowego. 
Ponieważ kationy sodu nie reagują z wodą, nie wpływają na pH i można je pominąć. Natomiast jony cyjankowe przyjmują protony z cząsteczek wody i generują jony wodorotlenkowe.
Kb dla jonów cyjankowych można wyznaczyć za pomocą równania: Ka × Kb = KW. Ponieważ Ka dla kwasu cyjanowodorowego wynosi 4,90 × 10−10, Kb dla jonów cyjankowych wynosi 2,04 × 10−5.
Kb jest równe stężeniu kwasu cyjanowodorowego pomnożonemu stężeniu jonów wodorotlenkowych podzielonemu przez stężenie jonów cyjanku.
Tabelę ICE można skonstruować w celu wyrażenia stężeń początkowych i równowagowych. Podstawiając stężenia równowagowe do wyrażenia, Kb równa się x razy x podzielone przez 0,35, co można później zweryfikować za pomocą reguły 5%.
Po rozwiązaniu równania x równa się 2,7 × 10−3 molowemu. Ponieważ x wynosi tylko 0,77% z 0,35 M, prawidłowe jest przybliżenie 0,35 minus x równe 0,35.
pH roztworu można obliczyć, przyjmując ujemny log 2,7 × 10−3 M, co równa się 2,57.
pH roztworu określa się za pomocą równania pH plus pOH jest równe 14, dlatego pH tego roztworu cyjanku sodu wynosi 11,43.

oznaczanie ph roztworów soli

Odczyn roztworu soli zależy od jej składników – anionów i kationów. Sole zawierające aniony o neutralnym pH i kationy wytwarzające jony hydroniowe tworzą roztwór o pH mniejszym niż 7. Na przykład w roztworze azotanu amonu (NH4NO3) jony NO3- nie reagują z wodą, podczas gdy jony NH4+ wytwarzają jony hydroniowe, w wyniku czego powstał kwaśny roztwór. Natomiast sole zawierające kationy o neutralnym pH i aniony wytwarzające jony wodorotlenkowe tworzą roztwór o pH większym niż 7. Na przykład w roztworze fluorku sodu (NaF) Na+ ma neutralne pH, ale F- wytwarza jony wodorotlenkowe i tworzy roztwór zasadowy. Przeciwjony mocnego kwasu lub zasady mają neutralne pH, a sole utworzone przez takie przeciwjony tworzą obojętny roztwór o pH równym 7. Na przykład w KBr kation K+ jest obojętny i nie wpływa na pH. Jon bromkowy jest sprzężoną zasadą mocnego kwasu, a zatem ma znikomą siłę zasady (brak zauważalnej jonizacji zasady). Rozwiązanie jest neutralne.

Niektóre sole zawierają zarówno kation kwasowy, jak i anion zasadowy. Ogólną kwasowość lub zasadowość roztworu określa się na podstawie względnej siły kationu i anionu, którą można porównać za pomocą Ka i Kb. Na przykład w NH4F jon NH4+ ma charakter kwasowy, a jon F− jest zasadowy (sprzężona zasada słabego kwasu HF). Porównując dwie stałe jonizacji: Ka NH4+ wynosi 5,6 × 10−10, a Kb F− wynosi 1,6 × 10−11, więc roztwór jest kwaśny, ponieważ Ka > Kb.

Obliczanie pH kwaśnego roztworu soli

Anilina to amina stosowana do produkcji barwników. Wydziela się go w postaci chlorku aniliny, [C6H5NH3+]Cl, soli otrzymywanej w reakcji słabej zasady aniliny i kwasu chlorowodorowego. Jakie jest pH 0,233 M roztworu chlorku aniliny?

<img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />

Ka dla jonu anilinowego pochodzi od Kb dla jego koniugatu zasady, aniliny:

<img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />

Na podstawie dostarczonych informacji przygotowywana jest tabela ICE dla tego systemu:

<div class="overflow">
<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+ (wodny) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (wodny)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">C6H5NH2 (wodny)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Stężenie początkowe (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;">Zmień (M)</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>
			<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;">Stężenie równowagowe (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.233 − 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>
</div>

Podstawienie tych warunków stężenia równowagowego do wyrażenia Ka daje

<img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />

Zakładając, że x << 0,233, równanie zostaje uproszczone i rozwiązane dla x:

<img alt="Eq4" src="/files/ftp_upload/11404/11404_Equation_4.png" style="height: 90px;" />

<img alt="Eq5" src="/files/ftp_upload/11404/11404_Equation_5.png" style="height: 50px;" />

Tabela ICE definiuje x jako molarność jonu hydroniowego, dlatego pH oblicza się jako

<img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />

Hydroliza [Al(H2O)6]3+

Oblicz pH 0,10 M roztworu chlorku glinu, który rozpuszcza się całkowicie i daje w roztworze uwodniony jon glinu [Al(H2O)6]3+.

Równanie reakcji i Ka to:

<img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />

Tabela ICE z podanymi informacjami to

<div class="overflow">
<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+ (wodny) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">H3O+ (wodny) </td>
			<td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)5(OH)2+ (wodny)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Stężenie początkowe (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;">Zmień (M)</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>
			<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;">Stężenie równowagowe (M)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.10 − 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>
</div>

Podstawiając wyrażenia dotyczące stężeń równowagowych do równania na stałą jonizacji otrzymuje się:

<img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />

Zakładając x << 0,10 i rozwiązując uproszczone równanie otrzymujemy:

<img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />

W tabeli ICE zdefiniowano x jako równe stężeniu jonów hydroniowych, dlatego obliczono pH na 2,92, a roztwór jest kwaśny.

<img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />

Oznaczanie pH roztworów soli

pH roztworu soli określa się za pomocą jego anionów i kationów składowych. Sole zawierające aniony o neutralnym pH i kationy wytwarzające jony hydroniowe ...

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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 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

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determining the ph of salt 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...

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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.

Salt Hydrolysis and pH in Solutions | JoVE K12

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PS.PSc.1.4

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

PS.PSc.1.5

The Periodic Table

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

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

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 ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

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 ...

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 ...

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 ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

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

PS.PSc.2.1

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 ...

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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