Chemistry
Reactions of Acids
Acids can react with metals to produce salt and hydrogen gas. They can also react with bases to form salt and water in a neutralization reaction. Additionally, acids can react with carbonates to produce salt, water, and carbon dioxide gas. These reactions are important in understanding the behavior and properties of acids in chemistry.
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6 Key excerpts on "Reactions of Acids"
eBook - PDF- James M. Beard(Author)
- 2016(Publication Date)
- CRC Press(Publisher)
47 CHAPTER 4 Types of Chemical Compounds and Their Reactions The world of chemistry contains millions of compounds and a huge number of dif-ferent types of chemical reactions. In order to keep track of all of this information it is necessary to categorize the material in some way. In this chapter, we are going to break down the field of chemistry into roughly five areas. The first three areas are based on types of chemical reactions that account for a vast majority of all chemi-cal reactions. We will then look at organic chemistry, which is based on a particular type of chemical compound, and, finally, we will look at certain nuclear processes. ACIDS AND BASES Acids Although there are a large number of chemical reactions that could be discussed, only three general classes of reactions—acid–base, precipitation, and oxidation– reduction—are discussed in this chapter. These three classes of reactions explain the chemical behavior of a large variety of substances. There are three major theories of acids and bases. This chapter focuses only on one of them, the simplest and the oldest. This theory was developed by a Swedish chemist, Svante Arrhenius , in the latter part of the 19th century. Let us first con-sider Arrhenius’ definition of acids. Arrhenius said that acids are substances that, when dissolved in water, produce hydrogen ions (H + ). This definition works fairly well with one minor modification. The 20th-century chemists fairly quickly came to the conclusion that H + ions do not exist as such, but rather H + attaches itself to a water molecule to form the hydronium ion (H 3 O + ). An acid can be defined as a substance that, when dissolved in water, produces hydronium ions (H 3 O + ). The properties asso-ciated with acids should be the properties of the H 3 O + ion. What is the behavior that the H 3 O + ion exhibits?
eBook - PDFInorganic Chemistry
Butterworths Intermediate Chemistry
- C. Chambers, A. K. Holliday(Authors)
- 2016(Publication Date)
- Butterworth-Heinemann(Publisher)
76 These topics, which are more fully treated in texts on physical chemistry, require some consideration here, because the terms 'acid', 'base', 'oxidation' and 'reduction' are used so widely in inorganic chemistry. 4.1 Protonic acids and bases An acid was once defined simply as a substance which produces hydrogen ions, or protons. However, the simple proton, H + , is never found under ordinary conditions, and this definition required amendment. Br0nsted and, independently, Lowry, therefore redefined an acid as a substance able to donate protons to other molecules or ions, and a base as a substance capable of accepting such protons. If we consider hydrogen chloride, HCl, as an example, the HCl molecule is essentially covalent, and hydrogen chloride (gas or liquid) contains no protons. But anhydrous hydrogen chloride in benzene will react with anhydrous ammonia: HCl + NH 3 - N H ^ C r Here, clearly, a proton is donated to the ammonia, which is the base, and hydrogen chloride is the acid. In water, the reaction of hydrogen chloride is essentially HCl + H 2 0 - H 3 0 + + Cl-and clearly here water is a base, but giving a new acid H 3 0 + and a new base, Cl~. The concept of Cl -as a base may at first seem strange but if an ionic chloride is added to concentrated sulphuric acid the following reaction occurs: H2SO4 + Cl- - HCl + HSO4 acid base acid base Product acids and bases such as those formed in this process are termed conjugate acids and conjugate bases. Thus, all acid-base reactions can be written as HA + B -BH + + A acid + base = conjugate + conjugate acid of base of base B acid HA Chapter 4 Acids and bases: oxidation and reduction 77 Protonic acids and bases and this equation is the prototype for acid-base reactions whether or not B is a solvent. To quote an example, HC1 in ethanol reacts as follows: 1 HC1 + C 2 H 5 OH ^ C 2 H 5 OH 2 + + Cr but in ethanol the reaction is by no means complete, hence the equilibrium sign.
eBook - PDF- Ageetha Vanamudan(Author)
- 2023(Publication Date)
- Delve Publishing(Publisher)
CHEMICAL REACTIONS CHAPTER5 CONTENTS 5.1 History of Chemical Reactions ........................................................... 77 5.2 Chemical Reactions of Various Types ................................................. 79 5.3 Several Theories Exist to Explain Acid-Base Reactions ........................ 87 5.4 Photolysis Reactions .......................................................................... 92 Introduction to Molecular Science 76 A chemical reaction occurs when one or more reactants are converted into one or more distinct products. Compounds and chemical elements are examples of substances. By rearranging the atoms of the reactants, chemical reactions produce a wide range of products. Chemical reactions are crucial in contemporary culture, technology, and even life itself. Fuel combustion, iron smelting, glass, and pottery manufacture, beer production, and the creation of wine and cheese are some examples of chemical processes that have been employed for millennia. In addition to the chemical reactions that occur in the earth’s crust, atmosphere, and seas, several complex processes occur in all living systems. It is necessary to distinguish between chemical reactions and physical changes. Physical transitions include ice melting into water and water evaporating to create vapor (Rastogi & Sani, 2011). A substance’s physical properties may change throughout metamorphosis, but its chemical identity does not. Water (H 2 O ) is the same substance regardless of its physical state since each molecule includes two hydrogen atoms and one oxygen atom. When water reacts with sodium metal (Na), it produces molecular hydrogen (H 2 ) and sodium hydroxide (NaOH). This denotes the occurrence of a chemical reaction or change. Understanding the fundamentals of chemical interactions. Figure 5.1: Chemical analysis of chemical reactants. Source: By No machine-readable author provided. Burn~commonswiki as- sumed (based on copyright claims).
eBook - PDFIntroductory Chemistry
An Active Learning Approach
- Mark Cracolice, Edward Peters, Mark Cracolice(Authors)
- 2020(Publication Date)
- Cengage Learning EMEA(Publisher)
1. An acid–base reaction is a transfer of protons; a redox reaction is a transfer of electrons. 2. In both cases, the reactants are given special names to indicate their roles in the transfer process. An acid is a proton source; a base is a proton remover. A reducing agent is an electron source; an oxidizing agent is an electron remover. 3. Just as certain species can either provide or remove protons (e.g., HCO 3 2 and H 2 O) and thereby behave as an acid in one reaction and a base in another, certain species can either remove or provide electrons, acting as an oxidizing agent in one reaction and a reducing agent in another. An example is the Fe 21 ion, which can oxidize Zn atoms to Zn 21 in the reaction Fe 21 saqd 1 Znssd S Zn 21 saqd 1 Fessd Fe 21 can also reduce Cl 2 molecules to Cl 2 ions in another reaction: 2 Fe 21 saqd 1 Cl 2 sgd S 2 Cl 2 saqd 1 2 Fe 31 saqd 4. Just as acids and bases may be classified as stronger or weaker depending on how readily they remove or provide protons, the relative strengths of oxidizing and reducing agents may be compared according to their tendencies to attract or release electrons. 5. Just as most acid–base reactions in solution reach a state of equilibrium, most aqueous redox reactions also reach equilibrium. Just as the favored side of an acid–base equilibrium equation can be predicted from acid–base strength, the favored side of a redox equilibrium equation also can be predicted from oxidizing agent–reducing agent strength. 17.9 The Water Equilibrium Goal 12 Given the hydrogen ion or hydroxide ion concentration of water or a water solution, calculate the other value. In the remaining sections of this chapter, you will be multiplying and dividing expo- nentials, taking the square root of an exponential, and working with logarithms. We will furnish brief comments on these operations as we come to them. For more detailed instructions, see Appendix I, Parts A and C.
eBook - PDFChemistry
Structure and Dynamics
- James N. Spencer, George M. Bodner, Lyman H. Rickard(Authors)
- 2011(Publication Date)
- Wiley(Publisher)
One of the characteristic properties of an acid is its ability to dissolve most metals. Zinc metal, for example, rapidly reacts with hydrochloric acid to form an aqueous solution of ZnCl 2 and hydrogen gas. Another characteristic property of acids is their ability to change the color of veg- etable dyes such as litmus. Litmus is a mixture of blue dyes that turns red in the presence of acid. Litmus has been used to test for acids for more than 300 years. Bases also have characteristic properties. They taste bitter and often feel slippery. They change the color of litmus from red to blue, thereby reversing the change in color that occurs when litmus comes in contact with an acid. Bases become less alkaline when they react with acids, and acids lose their characteristic sour taste and ability to dissolve metals when they are mixed with bases or alkalies. 11.2 The Arrhenius Definition of Acids and Bases In 1887, Svante Arrhenius took a major step toward answering the important ques- tion, “What factors determine whether a compound is an acid or a base?” Arrhe- nius suggested that acids dissociate or ionize when they dissolve in water to give H ions and a corresponding negative ion. According to this model, hydrogen chloride is an acid because it dissociates, or ionizes, when it dissolves in water to give H and Cl ions (Figure 11.1). This aqueous solution is known as hydrochloric acid and is often written as HCl(aq). It is important to recognize, however, that HCl is assumed to dissociate almost completely to form the H and Cl ions when it dissolves in water. Arrhenius argued that bases are compounds that dissociate in water to give OH ions and a positive ion. NaOH is an Arrhenius base because it dissociates in water to give the hydroxide (OH ) and sodium (Na ) ions. An Arrhenius acid therefore can be defined as any substance that ionizes when it dissolves in water to give the hydrogen ion, H .
eBook - PDFStantec's Water Treatment
Principles and Design
- John C. Crittenden, R. Rhodes Trussell, David W. Hand, Kerry J. Howe, George Tchobanoglous(Authors)
- 2022(Publication Date)
- Wiley(Publisher)
5-6 Reactions Used in Water Treatment The major chemical reactions that occur in water are (a) acid-base reactions, (b) precipitation (dissolution reactions), (c) complexation reactions with ligands (metal anion reactions), and (d) redox reactions (oxidation and reduction reactions). Acid-base reactions are very fast (reaching equilibrium in less than a second) because they often involve only a proton transfer. Pre- cipitation reactions often involve the coordination of anions around a cation and are relatively fast in the formation of amorphous solids (10 to 1000 min) and much slower (1 to 10,000 years) in the subsequent formation of crystals. Oxidation−reduction reactions follow many steps through specific single- electron transfers and, therefore, can be either very fast or very slow depend- ing on the reaction mechanism. In general, acid−base, complexation, and precipitation reactions tend to be reversible and redox reactions are often not reversible, because a significant amount of energy is often released for each of the elementary reactions that are involved in the overall reaction. 268 5 Principles of Chemical Reactions Acid−base reactions are common in water treatment, and pH has a significant effect on the chemical species present in water and on the efficiency of many treatment processes. In addition, acid-base reactions proceed faster than many other equilibrium reactions, making these reactions feasible given the time scale available for water treatment. Alkalinity, as discussed in Chap. 2, should be reviewed because of its impor- tance to acid−base chemistry. Many acid−base reactions can be described by the loss of a proton, as shown by the expression HA H A arrowpairrightleft + − + (5-118) where HA = acid species H + = hydrated proton (i.e., H 3 O + ) A − = conjugate base species At equilibrium, the following expression can be used to relate the activities of the species in Eq.
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