Name: strong acids, strong bases, and ph
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 22 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

Strong Acid and Base Solutions

Starke Säuren dissoziieren vollständig in Wasser. So dissoziiert Salpetersäure vollständig in Hydronium-Ionen und Nitrat-Ionen. Da die bei der Autoionisation von Wasser erzeugten Hydroniumionen vernachlässigbar sind, ist die Konzentration der Hydroniumionen im Wasser gleich der Konzentration der starken Säure.
Der pH-Wert dieser Lösungen kann anhand der Anfangskonzentration der starken Säure bestimmt werden.
Zum Beispiel dissoziiert HCl in einer 0,10 molaren HCl-Lösung vollständig in die Hydroniumionen und Chloridionen, und daher beträgt die Hydroniumionenkonzentration der Lösung ebenfalls 0,10 molaren. Wenn man den negativen Logarithmus dieser Konzentration nimmt, ist der pH-Wert der Lösung gleich eins.
Umgekehrt kann der pH-Wert einer Lösung verwendet werden, um die Hydroniumionenkonzentration einer Lösung zu bestimmen. Für eine Lösung mit einem pH-Wert von 3,60 kann beispielsweise die Hydroniumionenkonzentration bestimmt werden, indem die Gleichung 3,60 gleich dem negativen Logarithmus der Hydroniumionenkonzentration gelöst wird.
Um die Konzentration zu lösen, multiplizieren Sie beide Seiten mit minus eins und nehmen Sie dann den Antilog beider Seiten. Die Hydronium-Ionen-Konzentration entspricht 2,5 mal zehn hoch zu minus vier Molaren.
Starke Basen, bei denen es sich um Metallhydroxide der Gruppe 1 handelt, wie Natriumhydroxid und Kaliumhydroxid, dissoziieren vollständig in Lösung. Zum Beispiel dissoziiert 0,20 molares Natriumhydroxid vollständig in Wasser und produziert 0,20 molare Natriumionen und 0,20 molare Hydroxidionen.
Metallhydroxide der zweiten Gruppe, wie Bariumhydroxid und Calciumhydroxid, erzeugen jedoch zwei Mol Hydroxidionen für jedes Mol Base. Zum Beispiel dissoziiert 0,020 molare Calciumhydroxid vollständig in Wasser und produziert 0,020 molare Calciumionen und 0,040 molare Hydroxidionen.
Ionische Metalloxide wie Natriumoxid und Calciumoxid sind ebenfalls starke Basen. Ihr Oxidion reagiert mit Wasser und produziert Hydroxidionen.
Die Konzentration der Hydroxidionen kann zur Berechnung eines pOH und des pH-Werts der Lösung verwendet werden. Zum Beispiel hat eine fünfmal zehn bis minus fünf molare Kaliumhydroxidlösung eine gleiche Menge an Hydroxidionen wie eine starke Base und hat daher ein pOH von 4,30.
Wie der pH-Wert kann auch ein pOH der Lösung zur Bestimmung der Hydroxidionenkonzentration verwendet werden, indem die Gleichung gelöst wird: pOH entspricht dem negativen Logarithmus der Hydroxidionenkonzentration.
Da der pH-Wert plus pOH gleich 14 und der pOH 4,3 beträgt, beträgt der pH-Wert der Lösung 9,7.

starke säure- und basenlösungen

Eine starke Säure ist eine Verbindung, die in einer wässrigen Lösung vollständig dissoziiert und eine Konzentration an Hydroniumionen erzeugt, die der anfänglichen Säurekonzentration entspricht. Beispielsweise dissoziiert 0,20 M Bromwasserstoffsäure vollständig in Wasser und erzeugt 0,20 M Hydroniumionen und 0,20 M Bromidionen. <img alt="Eq1" src="/files/ftp_upload/11399/11399_Equation_1.png" style="height: 50px;"> Andererseits ist eine starke Base eine Verbindung, die in einer wässrigen Lösung vollständig dissoziiert und Hydroxidionen erzeugt. Beispielsweise dissoziieren 0,015 M KOH, ein Metallhydroxid der Gruppe 1, vollständig und erzeugen 0,015 M OH- und 0,015 M K+. <img alt="Eq2" src="/files/ftp_upload/11399/11399_Equation_2.png" style="height: 50px;"> Metallhydroxide der Gruppe 2, wie Bariumhydroxid [Ba(OH)2] und Strontiumhydroxid [Sr(OH)2], sind ebenfalls starke Basen und besitzen zwei Hydroxidionen. Dies führt dazu, dass sie im Vergleich zu NaOH oder KOH bei gleicher Konzentration eine basischere Lösung erzeugen. Beispielsweise ergeben 0,015 M Ba(OH)2 0,015 M Ba+ und 0,030 M Hydroxid. <img alt="Eq3" src="/files/ftp_upload/11399/11399_Equation_3.png" style="height: 50px;"> Da starke Säuren und Basen vollständig dissoziieren, können Molverhältnisse zur Bestimmung ihrer Hydronium- und Hydroxidkonzentrationen verwendet werden, die wiederum zur Berechnung des pH-Werts oder pOH einer Lösung verwendet werden können. Beispielsweise erzeugt eine 0,030 M HCl-Lösung 0,03 M Hydroniumionen. Daher wird der pH-Wert dieser Lösung sein <img alt="Eq4" src="/files/ftp_upload/11399/11399_Equation_4.png" style="height: 135px;"> Der pOH der gleichen Lösung kann mit der Formel bestimmt werden <img alt="Eq5" src="/files/ftp_upload/11399/11399_Equation_5.png" style="height: 50px;"> Da der pH-Wert der Lösung 1,52 beträgt, kann ihr pOH-Wert berechnet werden als: <img alt="Eq6" src="/files/ftp_upload/11399/11399_Equation_6.png" style="height: 50px;"> In ähnlicher Weise kann die Konzentration der von starken Basen erzeugten Hydroxidionen verwendet werden, um den pOH-Wert einer Lösung mithilfe der Gleichung zu bestimmen <img alt="Eq7" src="/files/ftp_upload/11399/11399_Equation_7.png" style="height: 50px;"> Die obige Gleichung kann auch zur Bestimmung der Hydroxidionenkonzentration verwendet werden, wenn der pOH bekannt ist. Wenn der pOH-Wert einer Lösung beispielsweise 3,00 beträgt, <img alt="Eq8" src="/files/ftp_upload/11399/11399_Equation_8.png" style="height: 50px;"> Die Multiplikation beider Seiten mit −1 ergibt <img alt="Eq9" src="/files/ftp_upload/11399/11399_Equation_9.png" style="height: 50px;"> Nehmen Sie nun den Antilog beider Seiten <img alt="Eq10" src="/files/ftp_upload/11399/11399_Equation_10.png" style="height: 90px;"> Somit beträgt die Hydroniumionenkonzentration der Lösung mit pOH 3 1,0 × 10−3 M. Eine ähnliche Methode kann verwendet werden, um die Hydroniumionenkonzentration einer Lösung zu bestimmen, wenn ihr pH-Wert bekannt ist.

Starke Säure- und Basenlösungen

Eine starke Säure ist eine Verbindung, die in einer wässrigen Lösung vollständig dissoziiert und eine Konzentration von Hydroniumionen erzeugt, die der ursprünglichen ...

Education

Lehre

JoVE Core

Chemie

Eins

Acids and Bases

Säuren und Basen

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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 completely. It produces 0.015 M OH- and 0.015 M K+.

Some group 2 metal hydroxides are also strong bases. Barium hydroxide, Ba(OH)2, and strontium hydroxide, Sr(OH)2, each contain two hydroxide ions. That means they create a more basic solution than NaOH or KOH at the same concentration. For example, 0.015 M Ba(OH)2 produces 0.015 M Ba+ and 0.030 M hydroxide.

The ion concentrations from strong acids and strong bases can be used to calculate pH and pOH. A 0.030 M HCl solution produces 0.03 M hydronium ions, so its pH can be found from that concentration. The same pH value can then be used to determine pOH. If the pH is 1.52, the pOH can be calculated from the relationship between them.

The same idea works for strong bases. The hydroxide ion concentration can be used to find pOH with the equation for pOH, and the equation can also be used in reverse when pOH is known. For example, if the pOH of a solution is 3.00, multiplying by -1 and taking the antilog gives a hydronium ion concentration of 1.0 × 10^-3 M. The same method can be used to find hydronium ion concentration when pH is known.

Strong Acids, Strong Bases, and pH

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 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...

ions as acids and bases

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...

determining the ph of salt 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...

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 strong acids and strong bases dissociate completely in water and how their ion concentrations are used to calculate pH and pOH.

Strong Acids, Strong Bases, and pH | JoVE K12

chemistry

JoVE Core Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

Physical Science

PS.PSc.2.5

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Minnesota Academic Standards in Science

1.2.1 9L.4.2.2.1

Texas Essential Knowledge and Skills

High School

CHEM.12

CHEM.12.C

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6.a

9-12.PS.3.6.c

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-11.

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Strong Acids, Strong Bases, and pH

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