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SOME ACIDS AND BASES ARE STRONGER THAN OTHERS

Immediately after hydrogen chloride, which is a gaseous substance, is added to water, it reacts with the water to form hydronium ions and chloride ions. That very litde HCI remains (none shown here) tells us that HCI is a strong acid. [Pg.337]

This same trend is seen with strong and weak bases. Strong bases, for example, tend to accept hydrogen ions more readily than weak bases. In solution, a strong base allows the flow of a large electric current and a weak base allows the flow of a small electric current. [Pg.338]

1 When liquid acetic acid is added to water, only a few acetic acid molecules react with water to form ions. The majority of the acetic acid molecules remain in their nonionized form, which tells us that acetic acid is a weak acid. [Pg.338]

SOME ACIDS AND BASES ARE STRONGER THAN OTHERS [Pg.339]

According to the aqueous solutions illustrated here, which is the stronger [Pg.339]


Some Acids and Bases Are Stronger Than Others... [Pg.329]

In this chapter, we explore acids and bases and the chemical reactions they undergo. We begin with a definition of these two important substances and then explore how some acids and bases are stronger than others. After learning about the pH scale, we close by looking at some environmental and physiological applications of acid-base concepts. [Pg.329]

In this chapter, we shall see why some substances are acids, why some acids are stronger than others, and why acids—like their partners the bases—are so important. We shall see that we can use thermodynamics, particularly equilibrium constants, to discuss the strengths of acids and bases quantitatively, and thereby develop our insight into the behavior of species in solution. [Pg.594]

Now we have established why you need to understand acids and bases, we must move on to consider why some acids are stronger than other acids and some bases stronger than other bases. To do this we must be able to estimate the pK of common classes of organic compounds. [Pg.169]

In view of the difficulties that accompany the use of a nonaqueous solvent, one may certainly ask why such use is necessary. The answer includes several of the important principles of nonaqueous solvent chemistry that will be elaborated on in this chapter. First, solubilities are different. In some cases, classes of compounds are more soluble in some nonaqueous solvents than they are in water. Second, the strongest acid that can be used in an aqueous solution is H30+. As was illustrated in Chapter 9, any acid that is stronger than H30+ will react with water to produce H30+. In some other solvents, it is possible to routinely work with acids that are stronger than H30+. Third, the strongest base that can exist in aqueous solutions is OH-. Any stronger base will react with water to produce OH-. In some nonaqueous solvents, a base stronger than OH - can exist, so it is possible to carry out certain reactions in such a solvent that cannot be carried out in aqueous solutions. These differences permit synthetic procedures to be carried out in nonaqueous solvents that would be impossible when water is the solvent. As a result, chemistry in nonaqueous solvents is an important area of inorganic chemistry, and this chapter is devoted to the presentation of a brief overview of this area. [Pg.331]

Hull and Conant in 1927 showed that weak organic bases (ketones and aldehydes) will form salts with perchloric acid in nonaqueous solvents. This results from the ability of perchlonc aad in nonaqueous systems to protonate these weak bases. These early investigators called such a system a superacid. Some authorities believe that any protic acid that is stronger than sulfunc aad (100%) should be typed as a superaad. Based upon this criterion, fluorosulfuric arid and trifluoro-methanesulfonic acid, among others, are so classified. Acidic oxides (silica and silica-aluminai have been used as solid acid catalysts for many years. Within the last few years, solid acid systems of considerably greater strength have been developed and can he classified as solid superacids. [Pg.13]


See other pages where SOME ACIDS AND BASES ARE STRONGER THAN OTHERS is mentioned: [Pg.228]    [Pg.144]    [Pg.144]    [Pg.548]    [Pg.303]    [Pg.448]    [Pg.464]    [Pg.151]    [Pg.523]    [Pg.247]    [Pg.5401]    [Pg.622]    [Pg.627]    [Pg.188]    [Pg.91]    [Pg.188]    [Pg.34]    [Pg.188]    [Pg.5400]    [Pg.140]    [Pg.11]    [Pg.282]    [Pg.28]    [Pg.377]    [Pg.377]    [Pg.223]    [Pg.65]    [Pg.869]    [Pg.331]    [Pg.953]    [Pg.71]    [Pg.136]    [Pg.194]    [Pg.19]    [Pg.656]    [Pg.676]   


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