Name: how acids and bases form ions
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.4

Acids, Bases and Neutralization Reactions

L'estomac humain est un organe musculaire contenant des sucs gastriques, y compris l'acide chlorhydrique, qui aident à digérer les aliments. Certains types d'aliments augmentent les niveaux d'acidité de l'estomac, provoquant le reflux acide. Consommer des aliments alcalins, ou une base comme un antiacide, neutralise les acides en excès, soulageant ainsi la sensation de brûlure.Ceci est un exemple de réaction acide-base. Les acides les plus simples sont des substances qui contiennent des atomes d'hydrogène dissociables. Dans les solutions aqueuses, ils libèrent des ions hydrogène chargés positivement, ou des protons, avec les anions correspondants.Les protons réagissent avec les molécules d'eau pour former des ions hydronium. Par exemple, une solution aqueuse d'acide nitrique contient des ions hydronium et des ions nitrate. D'autres communément appelés acides de l'acide chlorhydrique, l'acide sulfurique et l'acide phosphorique.Les acides sont monoprotiques ou polyprotiques en fonction du nombre d'atomes d'hydrogène dissociables par molécule. L'acide chlorhydrique et l'acide nitrique, avec un hydrogène dissociable chacun, sont tous deux des exemples d'acides monoprotiques, tandis que l'acide sulfurique et l'acide phosphorique sont polyprotiques. L'acide sulfurique est diprotique et libère ses deux protons séquentiellement, tandis que l'acide phosphorique est triprotique et se dissocie séquentiellement en trois étapes.Les bases les plus simples sont des composés qui produisent des ions hydroxyde chargés négativement dans des solutions aqueuses. Les bases facilement identifiables contiennent des groupes hydroxyles;par exemple, l'hydroxyde de sodium, l'hydroxyde de potassium et l'hydroxyde de calcium. De telles bases, lorsqu'elles sont ajoutées à l'eau, se dissocient en ions hydroxyde et en cations métalliques correspondants.Les bases non hydroxydes comme l'ammoniac réagissent avec l'eau en acceptant les protons des molécules d'eau pour produire des ions ammonium et des ions hydroxydes. En général, un acide et une base réagissent pour former de l'eau et un sel. Les réactions acide-base sont également appelées réactions de neutralisation lorsque les moles des protons fournis par l'acide et les moles des ions hydroxyde fournis par la base sont égaux.Par exemple, lorsque des quantités égales d'acide nitrique aqueux et d'hydroxyde de potassium aqueux sont mélangées, les quantités d'ions hydronium et d'hydroxyde fournis à la solution sont eux aussi égales. Les ions hydronium et hydroxyde, par conséquent, se neutralisent complètement en se combinant pour former de l'eau, ne laissant aucun ion hydronium ou hydroxyde derrière. En outre, les anions de nitrate et les cations de potassium se couplent pour former un sel nitrate de potassium.Certaines réactions de neutralisation sont des réactions d'évolution des gaz. Par exemple, l'acide chlorhydrique et le sulfite de potassium réagissent pour former du chlorure de potassium, de l'eau et du dioxyde de soufre gazeux à travers le système d'équilibre sulfite-bisulfite.

acides, bases et réactions de neutralisation

Une réaction acido-basique est une réaction dans laquelle un ion hydrogène, H+, est transféré d'une espèce chimique à une autre. De telles réactions revêtent une importance majeure pour de nombreux processus naturels et technologiques, allant des transformations chimiques dans les cellules ou dans les lacs et les océans à la production à l'échelle industrielle d'engrais, de produits pharmaceutiques et d'autres substances essentielles à la société . 
 
 Il existe plusieurs façons de définir un acide. Dans le contexte des solutions aqueuses, un acide est une substance qui se dissout pour produire des ions hydrogène. 
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-01.png" style="height: 40px;" />
 
 C'est la définition d'Arrhenius d'un acide, qui porte le nom du chimiste suédois Svante Arrhenius (1859–1927). Un ion hydrogène, représenté par le symbole H+, est appelé proton. En solution, les protons se combinent chimiquement avec des molécules d'eau, par le biais des doublets libres sur l'oxygène, pour former des ions hydronium, H3O+. 
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-02.png" style="height: 40px;" />
 
 L'équation chimique pour l'ionisation d'un acide est écrite comme 
 
 <img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-03.png" style="height: 40px;" />
 
 Les acides qui réagissent totalement avec l'eau de cette manière sont appelés des acides forts. HCl, HNO3 et HBr en sont quelques exemples. 
 
 La plupart des acides rencontrés dans la vie quotidienne sont des acides faibles. L'acide citrique dans les fruits, l'acide acétique dans le vinaigre et l'acide lactique dans le lait en sont quelques exemples. L'acide acétique, principal ingrédient du vinaigre alimentaire, est un exemple familier d'acide faible. Lorsqu'elles sont dissoutes dans l'eau dans des conditions typiques, seulement 1 % des molécules d'acide acétique sont présentes sous la forme ionisée,  CH3CO2−.  
 
 <img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-04.png" style="height: 40px;" />
 
 L'utilisation d'une double flèche dans l'équation ci-dessus indique l'aspect partiel de la réaction dans ce processus. 
 
 Une base est une substance qui se dissout dans l'eau pour produire des ions hydroxyde, OH&minus ;. Les bases les plus courantes sont les composés ioniques composés de cations de métaux alcalins ou alcalino-terreux (groupes 1 et 2) combinés avec l'ion hydroxyde : par exemple, NaOH et Ca(OH)2. Contrairement aux composés acides dont nous avons parlé précédemment, ces composés ne réagissent pas chimiquement avec l'eau ; au lieu de cela, ils se dissolvent et se dissocient, libérant des ions hydroxyde directement dans la solution. Par exemple, KOH et Ba(OH)2 se dissolvent dans l'eau et se dissocient totalement pour produire des cations (K+ et Ba2+, respectivement) et des ions hydroxyde, OH−. Ces bases, ainsi que d'autres hydroxydes qui se dissocient totalement dans l'eau, sont considérées comme des bases fortes. 
 
 Prenons l'exemple de la dissolution de l'hydroxyde de sodium dans l'eau : 
 
 <img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-05.png" style="height: 40px;" />
 
 Cette équation confirme que l'hydroxyde de sodium est une base. Lorsqu'il est dissous dans l'eau, NaOH se dissocie pour produire des ions H+ et OH−. Cela est également vrai pour tout autre composé ionique contenant des ions hydroxyde. Puisque le processus de dissociation est essentiellement total lorsque les composés ioniques se dissolvent dans l'eau dans des conditions typiques, NaOH et d'autres hydroxydes ioniques sont tous classés comme des bases fortes. 
 
 Contrairement aux hydroxydes ioniques, certains composés produisent des ions hydroxyde lorsqu'ils sont dissous par réaction chimique avec des molécules d'eau. Dans tous les cas, ces composés ne réagissent que partiellement et sont donc classés comme des bases faibles. Ces types de composés sont également abondants dans la nature et sont des produits importants dans diverses technologies. Par exemple, la production mondiale de la base faible ammoniac dépasse généralement 100 tonnes métriques par an parce qu'elle est largement utilisée comme engrais agricole, une matière première pour la synthèse chimique d'autres composés, et un ingrédient actif dans les nettoyants ménagers. Lorsqu'il est dissout dans l'eau, l'ammoniac réagit de façon partielle pour produire des ions d'hydroxyde, comme illustré ci-dessous : 
 
 <img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-06.png" style="height: 40px;" />
 
 Il s'agit, par définition, d'une réaction acido-basique impliquant le transfert d'ions H+ des molécules d'eau aux molécules d'ammoniac. Dans des conditions typiques, seulement environ 1 % de l'ammoniac dissous est présent sous forme d'ions NH4+. 
 
 Une réaction de neutralisation est un type particulier de réaction acido-basique dans lequel les réactifs sont un acide et une base (mais pas de l'eau), et les produits sont souvent un sel et de l'eau :  
 
 <img alt="Eq7" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-07.png" style="height: 40px;" />
 
 Pour illustrer une réaction de neutralisation, réfléchissez à ce qui se passe lorsqu'un antiacide typique, comme le lait de magnésie (une suspension aqueuse de Mg(OH)2 solide), est ingéré pour soulager les symptômes associés à l'excès d'acide gastrique (HCl) : 
 
 <img alt="Eq8" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-08.png" style="height: 40px;" />
 
 Notez qu'en plus de l'eau, cette réaction produit un sel, le chlorure de magnésium. Le H+ (aq) de l'acide (fort ou faible) se combine avec le OH− (aq) de la base (ou produit par la réaction d'une base faible avec l'eau) pour former H2O (l). Par exemple, la réaction entre les solutions aqueuses de HCl (acide fort) et de NaOH (base forte) est écrite comme suit : 
 
 <img alt="Eq9" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-09.png" style="height: 40px;" />
 
 HCl et NaOH subissent tous les deux une ionisation à 100 %. L'équation ionique complète, par conséquent, peut être écrite comme suit : 
 
 <img alt="Eq10" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-10.png" style="height: 40px;" />
 
 Les ions Cl- et Na+ sont appelés des ions spectateurs, qui s'annulent, ce qui donne l'équation ionique nette comme suit :  
 
 <img alt="Eq11" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-11.png" style="height: 40px;" />
 
 Ce texte est adapté de <a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions">OpenStax Chemistry 2e, Section: 4.2 : Classer les réactions chimiques.</a>

Acides, bases et réactions de neutralisation

Une réaction acide-base est une réaction dans laquelle un ion hydrogène, H+, est transféré d’une espèce chimique à une autre. De telles réactions sont d’une importance capitale pour ...

Education

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Chemistry

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Chemical Quantities and Aqueous Reactions

Quantités chimiques et réactions en phase aqueuse

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how acids and bases form ions

Acids and bases form ions in water through acid-base reactions. These reactions move a hydrogen ion, H+, from one chemical species to another. They matter in many natural and technological processes, from chemistry inside cells and in lakes and oceans to the large-scale production of fertilizers, pharmaceuticals, and other useful substances.

In water, an acid is a substance that produces hydrogen ions. This is the Arrhenius definition of an acid. The H+ ion is also called a proton. In solution, these protons combine with water molecules to form hydronium ions, H3O+.

Acids that react completely with water are called strong acids. Common examples include HCl, HNO3, and HBr. Most acids people encounter in daily life are weak acids. Citric acid in fruits, acetic acid in vinegar, and lactic acid in milk are examples. Acetic acid is a familiar weak acid, and under typical conditions only about 1% of its molecules are in the ionized form, CH3CO2−. A double arrow shows that this reaction is only partial.

A base is a substance that dissolves in water to yield hydroxide ions, OH−. The most common bases are ionic compounds made of alkali or alkaline earth metal cations from groups 1 and 2 with hydroxide ions, such as NaOH and Ca(OH)2. These compounds do not react chemically with water. Instead, they dissolve and dissociate, releasing hydroxide ions directly into solution.

KOH and Ba(OH)2 are examples of strong bases because they dissociate completely in water. The same is true for sodium hydroxide. When NaOH dissolves, it gives Na+ and OH− ions. Any ionic compound that contains hydroxide ions behaves this way under typical conditions, so these hydroxides are classified as strong bases.

Some compounds make hydroxide ions by reacting with water molecules instead of simply dissociating. These compounds react only partially, so they are weak bases. Ammonia is a common example. It is produced on a very large scale because it is used as an agricultural fertilizer, a starting material for chemical synthesis, and an ingredient in household cleaners. When ammonia dissolves in water, it reacts partially to form OH− and NH4+ ions. This is an acid-base reaction because H+ ions move from water molecules to ammonia molecules. Under typical conditions, only about 1% of dissolved ammonia is present as NH4+.

A neutralization reaction is a special acid-base reaction in which an acid and a base react, but water is not a reactant. The products are often a salt and water. Milk of magnesia is a common antacid made of solid Mg(OH)2 in water. It helps relieve excess stomach acid, HCl, by neutralizing it. This reaction forms water and the salt magnesium chloride.

In neutralization, H+(aq) from the acid combines with OH−(aq) from the base to make H2O(l). For example, HCl and NaOH are both completely ionized in water. Their complete ionic equation includes Na+ and Cl− ions, but these are spectator ions because they cancel out. The net ionic equation shows the essential change: H+(aq) + OH−(aq) → H2O(l).

How Acids and Bases Form Ions

precipitation reactions

Predicting Precipitation in Aqueous Reactions

Precipitation reactions happen when two aqueous solutions of soluble salts are mixed and an insoluble ionic compound forms. That solid is called a precipitate. The ions in solution exchange partners, so these reactions are also called double displacement, double replacement, exchange, or metathesis reactions. These reactions are useful in chemistry for identifying metal ions in a compound. They also support gravimetric methods, which measure composition by the mass of a substance. Whether a...

reaction stoichiometry

Using Balanced Equations to Predict Amounts

Balanced chemical equations show how much of each substance reacts and forms in a chemical change. The formulas identify the reactants and products, which helps classify the reaction. The coefficients show the relative numbers of each substance, which lets chemists measure the relationships between amounts consumed and produced. These quantitative relationships are called stoichiometry. The word comes from the Greek words stoicheion, meaning element, and metron, meaning measure. Stoichiometry...

acids, bases and neutralization reactions

Acids and bases form ions in water through acid-base reactions. These reactions move a hydrogen ion, H+, from one chemical species to another. They matter in many natural and technological processes, from chemistry inside cells and in lakes and oceans to the large-scale production of fertilizers, pharmaceuticals, and other useful substances. In water, an acid is a substance that produces hydrogen ions. This is the Arrhenius definition of an acid. The H+ ion is also called a proton. In...

limiting reactant

Limiting Reactant in Water Formation

Limiting reactants control how much product forms in a chemical reaction. In a balanced equation, the listed amounts of reactants and products are called stoichiometric amounts. In real reactions, the reactants are not always present in those exact proportions. The limiting reactant is the reactant that gets used up first. Once it is gone, the reaction stops making more product. The other reactant is called the excess reactant. Chemists often use extra amounts of one reactant to make sure the...

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Calculating Percent Yield in Reactions

Percent yield shows how much product a chemical reaction actually makes compared with how much it should make. The expected amount is called the theoretical yield. It comes from the balanced chemical equation and the stoichiometry, or mole ratios, in that equation. The theoretical yield assumes that the limiting reactant is completely converted into the desired product. The product collected after a reaction is the actual yield. In many cases, the actual yield is lower than the theoretical...

general properties of solutions

Solvents, Solutes, and Solution Types

Solutions are common mixtures found in everyday life. Ocean water, air, and gasoline are all examples of solutions. These mixtures contain two or more types of atoms or molecules in varying amounts. A solution is a homogeneous mixture, which means its composition is uniform throughout. This is different from a heterogeneous mixture, which has a non-uniform composition. In a homogeneous mixture, the components are evenly spread out and thoroughly mixed. Every solution has a solvent and a...

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Molarity and Dilution in Solutions

Molarity and dilution are key ideas for describing solution concentration. Concentration means the relative amount of one component in a solution. In many solutions, one component is present in much larger amount. That component is the solvent, which acts as the medium that holds the other parts dissolved or dispersed. Water is a very common solvent, so aqueous solutions are common on Earth. A solute is the component present at a much lower concentration than the solvent. Chemists often...

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Conductivity in Electrolyte Solutions

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Solubility Rules for Ionic Salts

Solubility rules help predict whether ionic salts will dissolve in water. Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a set temperature and pressure. It is often measured in molarity, or moles per liter (mol/L). A compound is soluble if it dissolves in water. When a soluble salt dissolves, its ions separate and spread evenly through the solution. This physical change is called dissociation. Potassium chloride, KCl, is a simple example. Water...

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Aqueous Reactions and Ionic Equations

Aqueous reactions are chemical reactions that take place in water. Water is a good solvent, so it can dissolve many substances. Because of that, many chemical reactions happen in aqueous solution. In high school chemistry, these reactions are often grouped into three common patterns: precipitation, acid-base, and oxidation-reduction. A precipitation reaction happens when ions in two aqueous ionic compounds exchange partners and form an insoluble salt, called a precipitate. In an acid-base...

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Redox Reactions and Oxidation Numbers

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Oxidation states help track electron transfer in redox reactions. An oxidation number, also called an oxidation state, is a hypothetical number that shows the effective charge of an atom or element. Chemists assign it by using a set of rules. In an ionic compound, oxidation numbers are based on how many electrons move between reacting species. For example, when calcium chloride forms, calcium loses two valence electrons and the two chlorine atoms each gain one electron. In CaCl2, calcium has...

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Synthesis and decomposition are two redox reactions that show how substances can be built up or broken down. Synthesis means to make something, while decomposition means to break something apart. These reactions also involve chemical changes and energy changes. Synthesis reactions are also called combination reactions. In a synthesis reaction, two or more substances join to form one more complex substance. They are often written as A + B → AB or A + B → C. One example is the formation of...

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chemical quantities and aqueous reactions

Learn how acids and bases form ions in water, including strong and weak acids, strong and weak bases, ammonia, and neutralization reactions.

How Acids and Bases Form Ions | JoVE K12

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Chemical Reactions

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Matter And Its Interactions

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Neutralization Reactions

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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Elements: Chemical Symbols and Isotopes

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Molecules and Compounds

Atoms and Molecules

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Solution Formation

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Colloids

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Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

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Phase Transitions: Vaporization and Condensation

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Vapor Pressure

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Clausius-Clapeyron Equation

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

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Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

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 ...

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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).



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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. ...

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

Understand types, properties, and structure of matter.

How Acids and Bases Form Ions

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