Naming Inorganic Acids

The anions described in the preceding sections may be formed by reaction of the corresponding acids with hydroxides  

The salts formed by these reactions consist of cations and anions. The cation in each of these cases is Na , and the anions are Cr, S04, and P04 , respectively. In these examples, the chloride ion, sulfate ion, and phosphate ion are formed from their parent acids. Thus the acids and anions are related, and so are their 

Replace the -ate ending of an anion with -ic acid or replace the -ite ending with -ous acid. 

This rule does not change if the anion has a prefix per- or hypo- if the anion has such a prefix, so does the acid. If not, the acid does not either. 

If the anion ends in -ide, add the prefix hydro- and change the ending to -ic acid. 

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Anhydrides. Anhydrides of inorganic acids are named as oxides for example, N2O5, dinitrogen pentaoxide. 

Esters. Esters of inorganic acids are named as the salts for example, ( 113)2804, dimethyl sulfate. However, if it is desired to specify the constitution of the compound, the nomenclature for coordination compounds should be used. 

Again, the recommended names (phosphonic acid and phosphonates) have found more general acceptance for organic derivatives such as RP03 , and purely inorganic salts are still usually called phosphites. The free acid is readily made by direct hydrolysis of PC l3 in cold CCI4 solution ... 

An inorganic acid has a formula that typically begins with H oxoacids have formulas that begin with H and end in O. We distinguish between binary hydrides, such as HX, which are not named as acids, and their aqueous solutions, HX(aq), which are. 

Most chemicals used in the procedure will appear in the index. Thus, there will generally be entries for all starting materials, reagents, intermediates, important by-products, and final products. Most products shown in the Tables in the discus.sion sections of this volume are included unless the compounds are quite similar in which case a general descriptive name was entered. Chemicals generally nut indexed included coiimion solvents, standard inorganic acids and bases, reactants shown in the Tables, and compounds cited in the discussion section in connection with other methods of preparation. 

Inorganic acids with a peroxide function are given the IUPAC name above, which distinguishes them from the organic peroxyacids. Collectively they are a group of very powerful oxidants, individual compounds being ... 

This chapter discusses pharmacologically and toxicologically relevant esters of inorganic acids, namely ... 

In previous chapters, we discussed the hydrolysis of a number of esters of A-(hydroxymethyl)phcnytoin, namely esters of organic acids (7V-acyloxy-methyl derivatives, Sect. 8.7.3) or inorganic acids (Sect. 9.3.2). Hydrolysis of these potential prodrugs released 3-(hydroxymethyl)phenytoin (11.45), whose breakdown to phenytoin and formaldehyde was also investigated per se [79], The latter reaction followed pseudo-first-order kinetics. At pH 7.4, the f1/2 values were 4.7 and 1.6 s at 25° and 37°, respectively. The tm values decreased tenfold for each increase of pH by one unit, which, together with the absence of any buffer catalysis, indicates catalysis by the HO- anion. 

Basilus Valentinus of Italy was first to isolate the acid and reported it under the name spiritus sabs in the fifteenth century. Glauber prepared this acid by the reaction of sulfuric acid with common salt in 1648. Lavoisier proposed the name muriatic acid in 1789 after muriate, the term referring to a chlorine-containing inorganic substance. Sir Humphrey Davy proved the gas was composed of only hydrogen and chlorine in 1810. Subsequently, the gas was named hydrogen chloride. 

Similar to inorganic acids, the reaction of carboxylic acids and bases produces carboxylic acid salts. Several of these salts are commonly used in foods and beverages as preservatives. The most common are salts from benzoic, propionic, and sorbic acids. The salts of these acids have names ending with ate, and can often be found in the list of ingredients of baked goods and fruit drinks. Several common preservatives are shown in Figure 15.11. 

As their name implies, carboxylic acids are acidic—they dissodate slightly in aqueous solution to give H30+ and a carboxylate anion. Carboxylic acids are much weaker than inorganic acids like HC1 or H2S04, however. The Ka of acetic add, for example, is 1.78 X 10-5 (pKa = 4.75), meaning that only about 1% of acetic acid molecules dissociate in a 1.0 M aqueous solution. Note in the following electrostatic potential map of acetic add that the acidic -OH hydrogen is positively polarized (blue). 

Four forms of As, namely, inorganic As (III), dimethylarsinic acid (DMA), monomethylarsonic acid (MMA), and inorganic As (V), were detected in rice [25], but in another study only As(V) and MMA were found [24], As the concentration of As in the rice grain was low, As speciation was performed only on rice straw to predict the risk associated with feeding contaminated straw to the cattle. Speciation of As in tissues by HPLC-ICP-MS revealed that the predominant species present in straw was arsenate followed by arsenite and dimethylarsinic acid (DMA). As DMA was only present at low concentrations, it was considered unlikely this would greatly alter the toxicity of As present in rice [71]. 

These catalysts were modified by adding non-volatile inorganic acids and their salts, namely orthophosphoric acid, boric acid, barium sulfate, sodium silicate, barium nitrate, and hydrofluoric acid. The additives were added to the finished catalyst by direct impregnation from solution. The presence of the additives did not alter the specific surface or the geometric structure of the final preparations. 

In recent years a considerable amount of fascinating new chemistry has been carried out in several highly acidic systems. This is exemplified by the preparation of stable solutions of aliphatic carbonium ions (Olah et al., 1965), the formation of a variety of new inorganic cations, e.g., the If and Sef+ cations (Gillespie, 1968), and the protonation of some unusual very weak bases such as carbonic acid to give C(OH)J (Olah and White, 1968). There has, however, been rather little fundamental information available on these systems and in particular on one of their most important and fundamental properties, namely their acidity. In this review we discuss the properties of systems which have acidities comparable to, or greater than, that of 100% H2S04. 

The nature of esters or ethereal salts has been fully discussed already in connection with the esters of inorganic acids and alcohols (p. 102). The name salts applies because they are formed by neutralizing an alcohol, acting as a base, with an acid. It must be emphasized, however, that in so terming these compounds salts we do not mean this to apply in a physical chemical sense as describing their properties in solution in accordance with the electrolytic theory of ionic dissociation. We are dealing here with questions of composition and constitution. Ethereal salts differ from metal salts, at least as to the degree of their dissociation into ions when in solution. 

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