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

O estômago humano é um órgão muscular que contém sucos gástricos, incluindo ácido clorídrico, que ajudam a digerir os alimentos. Certos tipos de alimentos aumentam os níveis de acidez do nosso estômago, causando o refluxo ácido. Consumir alimentos alcalinos, ou uma base como um antiácido, neutraliza o excesso de ácido, aliviando a sensação de ardor.Este é um exemplo de uma reação de base-ácida. Os ácidos mais simples são substâncias que contêm átomos de hidrogênio dissociáveis. Em soluções aquosas, eles libertam íons de hidrogênio de carga positiva, ou prótons, juntamente com os respetivos ânions.Os prótons reagem com as moléculas de água para formarem íons de hidrônio. Por exemplo, uma solução aquosa de ácido nítrico contém íons de hidrônio e íons de nitrato. Outros ácidos vulgarmente conhecidos são o ácido clorídrico, o ácido sulfúrico e o ácido fosfórico.Os ácidos são monopróticos ou polipróticos em função do número de átomos de hidrogênio dissociáveis por molécula. O ácido clorídrico e o ácido nítrico, com um hidrogênio dissociável cada um, são ambos exemplos de ácidos monopróticos, enquanto o ácido sulfúrico e o ácido fosfórico são polipróticos. O ácido sulfúrico é diprótico e liberta os seus dois prótons sequencialmente, enquanto que o ácido fosfórico é triprótico e dissocia-se sequencialmente em três passos.As bases mais simples são compostos que cedem íons de hidróxidos com carga negativa em soluções aquosas. As bases facilmente identificáveis contêm grupos hidroxilos;por exemplo, o hidróxido de sódio, o hidróxido de potássio e o hidróxido de cálcio. Tais bases, quando adicionadas à água, dissociam-se em íons de hidróxido e nos respectivos cátions metálicos.As bases não hidróxidas como o amoníaco reagem com a água aceitando prótons de moléculas de água para produzirem íons de amónio e íons de hidróxido. Em geral, um ácido e uma base reagem para formar água e um sal. As reações de base-ácido são também denominadas de reações de neutralização quando os moles de prótons fornecidos pelo ácido e os moles de íons de hidróxidos fornecidos pela base são iguais.Por exemplo, quando quantidades iguais de ácido nítrico aquoso e hidróxido de potássio aquoso são misturados, as quantidades de íons de hidrônio e de hidróxido fornecidas à solução também são iguais. Os íons de hidrônio e de hidróxido, portanto, neutralizam-se completamente uns aos outros, combinando-se para formar água, não deixando para trás quaisquer íons de hidrônio ou de hidróxido. Para além disso, os ânions de nitrato e os cátions de potássio formam um par para formarem um sal nitrato de potássio.Certas reações de neutralização são reações de evolução de gás. Por exemplo, o ácido clorídrico e o sulfito de potássio reagem para formarem cloreto de potássio, água, e gás de dióxido de enxofre através do sulfito sistema de equilíbrio de bissulfito.

reações de Ácidos, bases e de neutralização

Uma reação ácido-base é aquela em que um ião de hidrogénio, H+, é transferido de uma espécie química para outra. Tais reações são de importância central para numerosos processos naturais e tecnológicos, desde as transformações químicas que ocorrem dentro de células ou lagos e oceanos até à produção industrial de fertilizantes, produtos farmacêuticos, e outras substâncias essenciais para a sociedade.

Há diversas maneiras de definir um ácido. No contexto das soluções aquosas, um ácido é uma substância que se dissolve para produzir iões de hidrogénio.

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-01.png" style="height: 40px;" />

Esta é a definição de Arrhenius de um ácido, cujo nome vem do químico Sueco Svante Arrhenius (1859–1927). Um ião de hidrogénio, representado pelo símbolo H+, é chamado de protão. Em solução, os protões combinam-se quimicamente com moléculas de água, através dos pares isolados de oxigénio, para formar iões de hidrónio, H3O+.

<img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-02.png" style="height: 40px;" />

A equação química para a ionização de um ácido é escrita como

<img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-03.png" style="height: 40px;" />

Os ácidos que reagem completamente com água desta forma são chamados ácidos fortes. HCl, HNO3 e HBr são alguns exemplos.

A maioria dos ácidos encontrados no dia-a-dia são ácidos fracos. O ácido cítrico em frutos, o ácido acético em vinagre, e o ácido láctico no leite são alguns exemplos. Um exemplo familiar de um ácido fraco é o ácido acético, o ingrediente principal no vinagre alimentar. Quando dissolvidas em água em condições típicas, apenas cerca de 1% das moléculas de ácido acético estão presentes na forma ionizada,  CH3CO2−. 

<img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-04.png" style="height: 40px;" />

A utilização de uma seta dupla na equação acima indica o aspecto de reação parcial deste processo.

Uma base é uma substância que se dissolve em água para produzir iões hidróxido, OH−. As bases mais comuns são compostos iónicos compostos por catiões de metais alcalinos ou alcalinoterrosos (grupos 1 e 2) combinados com o ião hidróxido—por exemplo, NaOH e Ca(OH)2. Ao contrário dos compostos ácidos discutidos anteriormente, estes compostos não reagem quimicamente com água; em vez disso, dissolvem-se e dissociam-se, libertando iões hidróxido directamente na solução. Por exemplo, KOH e Ba(OH)2 dissolvem-se em água e dissociam-se completamente para produzir catiões (K+ e Ba2+, respectivamente) e iões hidróxido, OH−. Estas bases, juntamente com outros hidróxidos que se dissociam completamente em água, são consideradas bases fortes.

Considere a dissolução do hidróxido de sódio em água como um exemplo:

<img alt="Eq5" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-05.png" style="height: 40px;" />

Esta equação confirma que o hidróxido de sódio é uma base. Quando dissolvido em água, o NaOH dissocia-se para produzir iões Na+ e OH−. Isto também é válido para qualquer outro composto iónico que contenha iões hidróxido. Uma vez que o processo de dissociação é essencialmente completo quando os compostos iónicos se dissolvem em água em condições típicas, NaOH e outros hidróxidos iónicos são todos classificados como bases fortes.

Ao contrário dos hidróxidos iónicos, alguns compostos produzem iões hidróxido quando dissolvidos ao reagir quimicamente com moléculas de água. Em todos os casos, estes compostos reagem apenas parcialmente e são então classificados como bases fracas. Estes tipos de compostos são também abundantes na natureza e são comodidades importantes em várias tecnologias. Por exemplo, a produção global da base fraca amoníaco é normalmente superior a 100 toneladas métricas por ano, uma vez que é amplamente utilizada como fertilizante agrícola, uma matéria-prima para a síntese química de outros compostos, e um ingrediente ativo nos produtos de limpeza domésticos. Quando dissolvido em água, o amoníaco reage parcialmente para produzir iões hidróxido, como se mostra aqui:

<img alt="Eq6" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-06.png" style="height: 40px;" />

Isto é, por definição, uma reação ácido-base que envolve a transferência de iões H+ de moléculas de água para moléculas de amoníaco. Em condições típicas, apenas cerca de 1% do amoníaco dissolvido está presente como iões NH4+.

Uma reação de neutralização é um tipo específico de reação ácido-base, em que os reagentes são um ácido e uma base (mas não água), e os produtos são frequentemente sal e água: 

<img alt="Eq7" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-07.png" style="height: 40px;" />

Para ilustrar uma reação de neutralização, considere o que acontece quando um antiácido típico, como o leite de magnésia (uma suspensão aquosa de Mg(OH)2 sólido) é ingerido para aliviar os sintomas associados ao excesso de ácido gástrico (HCl):

<img alt="Eq8" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-08.png" style="height: 40px;" />

Note que, para além de água, esta reação produz um sal, cloreto de magnésio. O H+ (aq) do ácido (forte ou fraco) combina-se com o OH− (aq) da base (ou produzido pela reação entre uma base fraca e água) para formar H2O (l). Por exemplo, a reação entre as soluções aquosas de HCl (ácido forte) e NaOH (base forte) é escrita da seguinte forma:

<img alt="Eq9" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-09.png" style="height: 40px;" />

Tanto HCl como NaOH são submetidos a 100% de ionização. A equação iónica completa, portanto, pode ser escrita como:

<img alt="Eq10" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-10.png" style="height: 40px;" />

Cl- e Na+ são designados iões espectadores, que se cancelam, tornando a equação iónica líquida como: 

<img alt="Eq11" src="https://www.jove.com/files/core/CDNSource/lessons/1029/1029_Equations-11.png" style="height: 40px;" />

Este texto é adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions">OpenStax Chemistry 2e, Section: 4.2: Classifying Chemical Reactions.</a>

Reações de Ácidos, Bases e de Neutralização

Uma reação ácido-base é aquela em que um íon hidrogênio, H+, é transferido de uma espécie química para outra. Tais reações são de importância central para ...

Education

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Chemistry

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Chemical Quantities and Aqueous Reactions

Quantidades Químicas e Reações Aquosas

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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...

reaction yield

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...

solution concentration and dilution

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...

electrolyte and nonelectrolyte solutions

Conductivity in Electrolyte Solutions

Electrolyte solutions conduct electricity because they contain mobile ions. The amount of current depends on how many ions are present in the aqueous solution. A solution with more dissolved ions conducts better, while a solution with few or no ions conducts poorly. Strong electrolytes dissociate completely in water. This complete dissociation is shown with a single forward arrow. Water-soluble ionic compounds such as sodium chloride split into sodium cations and chloride anions in solution.

solubility of ionic compounds

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...

chemical reactions in aqueous solutions

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...

oxidation–reduction reactions

Redox Reactions and Oxidation Numbers

Redox reactions are chemical changes in which electrons move between reactants, and oxidation numbers help track that change. The term oxidation once referred only to reactions with molecular oxygen, but it now covers a wider reaction class called oxidation-reduction, or redox, reactions. Some redox reactions form ionic products. A simple example is the reaction between sodium and chlorine that produces sodium chloride. To follow what happens to each reactant, chemists often write...

oxidation numbers

Assigning Oxidation States in Redox Reactions

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...

acids, bases, and neutralization reactions

synthesis and decomposition reactions

Building and Breaking in Chemical Reactions

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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PS.PSc.2.6

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Pennsylvania State Academic Standards

Chemical Reactions

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3.2.9-12.G

Louisiana Student Standards for Science

Matter And Its Interactions

HS-PS1-2

HS-PS1-7

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

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Matter and Its Interactions

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9-12.PS.3.5.d

9-12.PS.3.6.d

Florida Department of Education

SC.912.P.8

SC.912.P.8.8

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New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-4.

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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

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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

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

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

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

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

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Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

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

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

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 ...

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

Understand types, properties, and structure of matter.

How Acids and Bases Form Ions

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