Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
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Water: A Bronsted-Lowry Acid and Base

Cząsteczka amfoteryczna może działać zarówno jako kwas, jak i zasada. Przykładem cząsteczki amfoterycznej jest woda.
W wodnym roztworze amoniaku woda może działać jak kwas, oddając proton amoniakowi, zasadzie. Natomiast woda działa jak zasada w wodnym roztworze kwasu solnego, przyjmując proton z kwasu.
Ponieważ jest amfoteryczny, woda może ulegać autojonizacji. W tym procesie jedna cząsteczka wody działa jak kwas, oddając proton innej cząsteczce wody, która działa jak zasada, przyjmując ten proton.
Powoduje to wytwarzanie jonu hydroniowego i jonu wodorotlenkowego.
Stała równowagi dla autojonizacji wody, KW, znana również jako stała jonowo-produktowa dla wody, ma wartość 1 × 10−14. Jego wyrażenie równowagi jest zapisywane jako stężenie jonów hydroniowych razy stężenie jonów wodorotlenkowych, bez mianownika, ponieważ oba reagenty są cieczami. 
W czystej wodzie o temperaturze 25 °C stężenia jonów hydroniowych i wodorotlenkowych są równe – czyli 1 × 10−7 M. 
KW można wykorzystać do obliczenia stężenia jonów hydroniowych i wodorotlenkowych w roztworze oraz do określenia, czy roztwór jest kwaśny czy zasadowy.
Jeśli roztwór jest kwaśny, stężenie jonów hydroniowych będzie wyższe niż jonów wodorotlenkowych. W przeciwieństwie do tego, jeśli roztwór jest zasadowy, stężenie jonów wodorotlenkowych będzie wyższe niż jonów hydroniowych.
Jeżeli stężenie jonów hydroniowych w roztworze wynosi 5 × 10−7 M, stężenie jonów wodorotlenkowych można oznaczyć za pomocą K W.
Ponieważ znane są wartości KW i jonów hydroniowych, stężenie jonów wodorotlenkowych można obliczyć na 2 × 10−8 M.
Ponieważ stężenie jonów hydroniowych 5 × 10−7 M jest wyższe niż stężenie jonów wodorotlenkowych, 2 × 10−8 M, roztwór jest kwaśny.

woda: kwas i zasada bronsteda-lowry'ego

Reakcja pomiędzy kwasem Brønsteda-Lowry'ego i wodą nazywana jest jonizacją kwasu. Na przykład, gdy fluorowodór rozpuszcza się w wodzie i jonizuje, protony są przenoszone z cząsteczek fluorowodoru do cząsteczek wody, tworząc jony hydroniowe i jony fluorkowe:

 <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />

Jonizacja zasadowa zachodzi, gdy kwas przyjmuje protony z cząsteczek wody. W poniższym przykładzie cząsteczki pirydyny, C5NH5, po rozpuszczeniu w wodzie ulegają jonizacji zasadowej, dając jony wodorotlenkowe i pirydyniowe:

 <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />

Powyższe reakcje jonizacji sugerują, że woda może działać zarówno jako zasada (jak w reakcji z fluorowodorem), jak i kwas (jak w reakcji z amoniakiem). Gatunki zdolne do oddawania lub przyjmowania protonów nazywane są amfiprotycznymi lub bardziej ogólnie amfoterycznymi, co jest terminem, który może być używany do oznaczania kwasów i zasad zgodnie z definicjami innymi niż definicja Brønsteda-Lowry'ego. Poniższe równania przedstawiają dwie możliwe reakcje kwasowo-zasadowe dla dwóch form amfiprotycznych, jonu wodorowęglanowego i wody:

 <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />

Pierwsze równanie przedstawia reakcję wodorowęglanu jako kwasu z wodą jako zasadą, podczas gdy drugie przedstawia reakcję wodorowęglanu jako zasady z wodą jako kwasem. Po dodaniu wodorowęglanu do wody obie te równowagi ustalają się jednocześnie i skład powstałego roztworu można określić poprzez odpowiednie obliczenia równowagi. W stanie ciekłym cząsteczki substancji amfiprotycznej mogą ze sobą reagować, co ilustrują poniższe równania dla wody:

 <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />

Proces, w którym podobne cząsteczki reagują, wytwarzając jony, nazywa się autojonizacją. Woda w stanie ciekłym w bardzo niewielkim stopniu ulega autojonizacji; w temperaturze 25°C około dwie na miliard cząsteczek wody ulegają jonizacji. Stopień procesu autojonizacji wody odzwierciedla wartość jej stałej równowagi, stałej produktu jonowego dla wody, KW:

 <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />

Nieznaczna jonizacja czystej wody znajduje odzwierciedlenie w małej wartości stałej równowagi; w temperaturze 25 °C KW ma wartość 1,0 × 10-14.

 <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />

Proces jest endotermiczny, zatem stopień jonizacji i wynikające z tego stężenia jonów hydroniowych i jonów wodorotlenkowych rosną wraz z temperaturą. Na przykład w temperaturze 100 °C wartość KW wynosi około 5,6 × 10-13, czyli około 50 razy więcej niż wartość w temperaturze 25 °C.

Autojonizacja wody daje taką samą liczbę jonów hydroniowych i wodorotlenkowych. Dlatego w czystej wodzie o temperaturze 25 °C:

 <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />

Stężenia tych jonów w roztworze są często krytycznymi wyznacznikami właściwości roztworu i zachowania chemicznego innych substancji rozpuszczonych, dlatego opracowano specjalne słownictwo w celu opisania tych stężeń w kategoriach względnych. Roztwór jest obojętny, jeśli zawiera równe stężenia jonów hydroniowych i wodorotlenkowych; kwaśny, jeśli zawiera większe stężenie jonów hydroniowych niż jonów wodorotlenkowych; i zasadowy, jeśli zawiera mniejsze stężenie jonów hydroniowych niż jonów wodorotlenkowych.

Podsumowanie relacji dla roztworów kwaśnych, zasadowych i obojętnych

Klasyfikacja Względne stężenie jonów pH w temperaturze 25 °C

<div class="overflow">
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Klasyfikacja</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Względne stężenie jonów</td>
			<td style="color: black; border: 1px solid black; text-align: center;">pH w temperaturze 25 °C</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">kwaśny</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;">obojętny</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;">zasadowy</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>

Woda: kwas i zasada Bronsteda-Lowry'ego

Reakcja między kwasem Brønsteda-Lowry'ego a wodą nazywa się jonizacją kwasową. Na przykład, gdy fluorowodór rozpuszcza się w wodzie i jonizuje, ...

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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

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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...

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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 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 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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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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