Name: ionic strength in salt and acid solutions
Uploaded: 2024-04-04T10:51:15.000Z
Duration: 1 min 12 s
Channel: JoVE

Wenn sich ein Salz in Wasser auflöst, dissoziieren Kation und Anion. Jedes Ion zieht aufgrund der elektrostatischen Anziehung Ionen der entgegengesetzten Ladung an.
Diese ionische Atmosphäre um die Ionen schirmt die Ladung des Zentralions schwach ab.
Die Wirksamkeit der Abschirmung der ionischen Atmosphäre hängt mit der Ionenstärke zusammen, die durch die Konzentration und die Ladung der Ionen bestimmt wird.
Formal symbolisiert als I, umfasst die Ionenstärke einer Lösung die Gesamtkonzentration aller Ionen in der Lösung und ist proportional zur molaren Konzentration des Salzes.
Da die Ladung des Ions in der Berechnung quadriert wird, ist sein Beitrag zum Ionenstärkewert umso bedeutender, je größer die Ladung eines Ions ist.
Zum Beispiel ist die Ionenstärke einer Kaliumnitratlösung die gleiche wie ihre Konzentration.
Die Ionenstärken von Lösungen von Kaliumsulfat, einem 2:1-Elektrolyten, und Calciumsulfat, einem 2:2-Elektrolyten, betragen jedoch das Drei- bzw. Vierfache ihrer Konzentrationen.

ionenstärke: Überblick

Die Ionenstärke einer Lösung ist ein quantitativer Ausdruck für die Gesamtelektrolytkonzentration einer Lösung. Dieses Konzept wurde erstmals 1921 von zwei amerikanischen physikalischen Chemikern, Gilbert N. Lewis und Merle Randall, eingeführt, als sie den Aktivitätskoeffizienten starker Elektrolyte beschrieben. Bei der Berechnung der Ionenstärke (I oder μ) werden alle Kationen und Anionen berücksichtigt. Allerdings hat die Konzentration (c) eines Ions mit einer größeren Ladungszahl (z) einen größeren Beitrag zur Gesamtionenstärke, da die Ladung des Ions quadratisch ist.

Bei der Berechnung der Ionenstärke für ein Salz, das bei der Dissoziation mehrere Äquivalente desselben Ions erzeugt, müssen wir den Beitrag jedes Ions berücksichtigen. Beispielsweise kann die Ionenstärke von 0,1 mol/L Na2SO4 wie folgt berechnet werden:

Die Konzentration von Na+ beträgt 0,2 mol/L, da ein Molekül Na2SO4 dissoziiert und in Lösung zwei Na+-Ionen ergibt. Die Ionenstärke verdünnter Lösungen lässt sich leicht berechnen. In einer konzentrierteren Lösung wird die Berechnung jedoch komplexer und ungenauer, da die Salze nicht vollständig dissoziieren. Beispielsweise liegen in einer wässrigen Lösung von 0,025 mol/L MgSO4 25 bis 35 % MgSO4 als Ionenpaar MgSO4 (aq) vor.

Das Konzept der Ionenstärke kann weiter auf starke und schwache Säuren ausgedehnt werden. Da starke Säuren in Lösung vollständig dissoziieren, kann ihre Ionenstärke auf die gleiche Weise berechnet werden wie die von dissoziierten Salzen. Bei schwachen Säuren kann die Konzentration ionisierter Spezies aus dem Wert der Ionisationskonstanten berechnet und dann zur Bestimmung der Ionenstärke verwendet werden. Wenn die Säure sehr schwach ist und größtenteils nicht ionisiert bleibt, ist ihr Beitrag zur Gesamtionenstärke der Lösung vernachlässigbar.

Ionenstärke: Überblick

Wenn sich ein Salz in Wasser auflöst, dissoziieren Kation und Anion. Jedes Ion zieht aufgrund der elektrostatischen Anziehung Ionen der entgegengesetzten Ladung an.
Diese ionische ...

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Ionic Strength: Overview

ionic strength in salt and acid solutions

Ionic strength describes the total electrolyte concentration in a solution. It is a quantitative measure of how many ions are present and how strongly they contribute to the solution. The concept was introduced in 1921 by Gilbert N. Lewis and Merle Randall while they were describing the activity coefficient of strong electrolytes.

To calculate ionic strength, written as I or μ, both cations and anions are included. The concentration of each ion matters, but the charge number z matters even more because it is squared in the calculation. That means ions with a higher charge contribute more to the total ionic strength than ions with a lower charge at the same concentration.

When a salt produces more than one of the same ion after dissolving, each ion must be counted. For example, 0.1 mol/L Na2SO4 gives a sodium ion concentration of 0.2 mol/L because each formula unit forms two Na+ ions in solution. This makes the sodium contribution part of the final ionic strength value.

Ionic strength is easier to calculate for dilute solutions. In more concentrated solutions, the calculation becomes less exact because salts do not dissociate completely. For instance, in 0.025 mol/L MgSO4(aq), about 25% to 35% of the salt can remain as the ion pair MgSO4(aq).

The idea also applies to strong and weak acids. Strong acids dissociate completely in solution, so their ionic strength can be calculated in the same way as fully dissociated salts. Weak acids require the concentration of ionized species, which can be found from the ionization constant and then used for ionic strength. If an acid is very weak and stays mostly non-ionized, its contribution to the total ionic strength is negligible.

Ionic Strength in Salt and Acid Solutions

ionic-strength-in-salt-and-acid-solutions

ionic strength: overview

Ionic strength describes the total electrolyte concentration in a solution. It is a quantitative measure of how many ions are present and how strongly they contribute to the solution. The concept was introduced in 1921 by Gilbert N. Lewis and Merle Randall while they were describing the activity coefficient of strong electrolytes. To calculate ionic strength, written as I or μ, both cations and anions are included. The concentration of each ion matters, but the charge number z matters even...

ionic strength: effects on chemical equilibria

ionic-strength-effects-on-chemical-equilibria

Salt Effect on Salt Solubility

Salt effect can change the solubility of a sparingly soluble salt in water. When an inert ionic compound is added, the dissolved salt may become more soluble. A common example is potassium nitrate added to a saturated calcium sulfate solution, which increases the amount of calcium sulfate that dissolves. Le Châtelier’s principle does not explain this shift well. Instead, the change is described by the effective concentration of ions in solution. Each ion is surrounded by an ionic atmosphere,...

thermodynamics: chemical potential and activity

thermodynamics-chemical-potential-and-activity

Chemical Potential in Solution Activity

Chemical potential and activity describe how a species behaves in a solution. Activity is the effective concentration of a species. It accounts for the electrolytes near that species and depends on the ionic strength of the solution. Activity is calculated as molar concentration multiplied by the activity coefficient. This makes it a more precise way to describe a species in solution than concentration alone. The thermodynamic equilibrium constant is also defined more accurately using activity...

thermodynamics: activity coefficient

Activity Coefficient in Ionic Solutions

Activity coefficient in ionic solutions describes how much a species behaves like its measured concentration. Activity is the effective concentration of a solute in solution. It equals the molar concentration multiplied by the activity coefficient, which is a unitless number. The activity coefficient depends on the total ionic strength of the solution. It shows how far a solution is from ideal behavior. When ionic strength is very low, the activity coefficient of an ionic species is close to...

chemical equilibria: redefining equilibrium constant

chemical-equilibria-redefining-equilibrium-constant

Salt Effect in Equilibrium Constant Calculations

Salt effect changes how a sparingly soluble salt dissolves when an inert salt is added. The size of this effect depends on the ionic strength of the solution. Ionic strength reflects how strongly the ions in the solution interact. In solution, the activity of a species is the product of its concentration and its activity coefficient. A redefined equilibrium constant must account for these activity effects when the ionic strength is moderately high. This form is also called the thermodynamic...

factors affecting activity coefficient

How Ionic Strength Changes Activity Coefficient

The activity coefficient of an ion in water depends on ionic strength, ion charge, and ion size. The extended Debye-Hückel equation describes these effects for aqueous solutions at 25°C. These three factors are partly linked, so changes in one can influence the others. When a solution has almost zero ionic strength, the activity coefficient is close to one. That means the solution behaves almost ideally. As ionic strength rises from 0 to 0.1 mol/L, the activity coefficient usually drops.

chemical equilibria: systematic approach to equilibrium calculations

chemical-equilibria-systematic-approach-to-equilibrium-calculations

Equilibrium Calculations with Mass and Charge

Chemical equilibrium calculations become easier when they are organized around mass balance and charge balance. This approach is useful for systems with multiple equilibria, where several reactions must be considered together. It is especially helpful when finding the solubility of a sparingly soluble salt in water with a common ion present. The first step is to identify every chemical reaction in the system. Next, write the equilibrium constant expression for each reaction. These expressions...

acid&#8211;base equilibria: activity-based definition of ph

acidbase-equilibria-activity-based-definition-of-ph

How Ionic Strength Changes pH

pH depends on hydrogen ion activity, not just hydrogen ion concentration. In an ideal solution, pH is the negative logarithm of the hydrogen ion concentration. In a non-ideal solution, a more accurate pH uses hydrogen ion activity, which combines concentration with an activity coefficient. This difference matters most in very low ionic strength solutions, such as pure water. At first, the hydrogen ion activity coefficient is close to one. When an electrolyte that does not donate or accept a...

ladder diagrams: acid&#8211;base equilibria

Using Ladder Diagrams to Predict pH

Ladder diagrams help show how acid-base equilibria change with pH. They are graphical tools that make the chemistry of a system easier to read during analysis. In a ladder diagram, the vertical axis shows pH. Horizontal bars, or steps, place the pKa values in the system.

ladder diagrams: redox equilibria

Redox Potential Shifts in Ladder Diagrams

Ladder diagrams show redox equilibrium using electrochemical potential, E, as the vertical scale. They help students see how changes in concentration affect which species is most stable. The areas of predominance are set with the Nernst equation. A useful example is the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates. At potentials more negative than +0.771 V, Fe2+ predominates. Ladder diagrams also show...

ladder diagrams: complexation equilibria

Reading Metal-Ligand Ladder Diagrams

Ladder diagrams help show equilibria in metal-ligand complexes. In these diagrams, the vertical scale shows pL, or the concentration of free ligand that has not reacted. The horizontal lines mark the log of formation constants and show which species is dominant in each region. For the Cd and ammonia system, the formation constant K1 for Cd(NH3)2+ is 3.55 × 10^2. Its log value is 2.55, so pNH3 = 2.55 is the dividing line between Cd2+ and Cd(NH3)2+ dominance. Above 2.55, Cd2+ is the predominant...

solubility equilibria: overview

How Solubility Reaches Equilibrium

Solubility equilibrium describes what happens when a sparingly soluble salt dissolves in water and then reaches a balance with the solid left over. In a saturated solution, dissolved ions and the undissolved solid are in dynamic equilibrium. The process is reversible, so this topic is also called precipitation equilibrium. This balance matters in real life. Sugar-rich foods can produce organic acids that dissolve hydroxyapatite, the mineral in tooth enamel, which can lead to tooth decay. A...

solubility equilibria: ionic product of water

solubility-equilibria-ionic-product-of-water

Water Ionization and Kw in Equilibrium

Water ionization and the ionic product of water describe how pure water reaches equilibrium. Water is a weak electrolyte, so only a small amount breaks into hydrogen ions and hydroxide ions. At a fixed temperature, the amount of undissociated water stays almost constant. Because of this, the ionic product of water is the product of the hydrogen ion concentration and the hydroxide ion concentration. It is written as K w . The square root of K w gives the concentration of each ion in pure water.

complexation equilibria: overview

Stepwise Metal-Ligand Complexation

Stepwise metal-ligand complexation forms coordination compounds when metal ions and ligands share electrons through dative, or coordinate covalent, bonds. In these reactions, the metal ion binds to one or more ligands until its coordination number is reached. This number tells how many bonds form between the metal ion and the ligands. In aqueous solution, many metal ions are already surrounded by water molecules. These species are called aqua complexes. Complexation reactions are described by...

complexation equilibria: the chelate effect

complexation-equilibria-the-chelate-effect

Chelating Ligands and Metal Complex Stability

Metal complexes form when metal atoms or cations interact with ligands in a complexation reaction. These donor-acceptor adducts are central to understanding how metal ions bind in chemistry. Ligands can bind in different ways. A monodentate ligand uses one donor site. A bidentate ligand uses two donor sites, and a polydentate ligand uses more than two. Ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms and forms a five-membered ring. Polydentate ligands can...

complexation equilibria: factors influencing stability of complexes

complexation-equilibria-factors-influencing-stability-of-complexes

Complex Ions: Metal and Ligand Stability

Complex ions form when a metal cation accepts electron pairs from ligands, which are the electron pair donors. The stability of these metal complexes depends mainly on the metal ion and on the ligands attached to it. The metal ion’s size and charge play a major role in stability. As the size of the metal ion increases, complex stability usually decreases when the valency of the metal ion and the ligands stays the same. As the charge on the metal ion increases, complex stability increases. <br...

redox equilibria: overview

Redox Electron Transfer and Half-Reactions

Redox reactions involve the transfer of electrons from one species to another. In this type of reaction, electrons are not shared between atoms. They move from the species that loses them to the species that gains them. The species that loses electrons is the reducing agent, also called the reductant. It is oxidized during the reaction. The species that gains electrons is the oxidizing agent, or oxidant, and it is reduced. Redox reactions are often written as two half-reactions. One...

titrimetric methods: types and commonly used strategies

titrimetric-methods-types-and-commonly-used-strategies

Direct, Back, and Displacement Titrations

Titrimetric methods use a standard solution to measure the amount of an analyte in chemistry. The main categories are volumetric, gravimetric, and coulometric methods. Each one reaches the endpoint in a different way. In volumetric titrations, the key measurement is the volume of a titrant with a known concentration. The titrant is added until it reacts completely with the analyte. In gravimetric titrations, the standard solution forms an insoluble precipitate with the analyte. That solid is...

classification of titrimetric analysis based on reaction types

classification-of-titrimetric-analysis-based-on-reaction-types

Four Reaction Types in Titrimetric Analysis

Titrimetric analysis measures solution volume and is also called volumetric analysis. A standard solution with a known concentration is placed in the burette and is called the titrant. The solution with an unknown concentration in the flask is the analyte, or titrand. Titrimetric analysis is grouped into four types based on the reaction between the titrant and the analyte. Acid-base titrations involve a neutralization reaction between an acid and a base. This reaction forms water molecules.

key terms and concepts

Learn how ionic strength depends on ion charge, ion concentration, and dissociation in salt and acid solutions, with examples from Na2SO4, MgSO4, and acids.

Ionic Strength in Salt and Acid Solutions | JoVE K12

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Ionic Strength in Salt and Acid Solutions

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