Water liquid ammonia

Ionic polysulfides dissolve only in media of high polarity hke water, liquid ammonia, alcohols, nitriles, amines, and similar solvents. In all of these solvents 8 can be reduced electrochemically to polysulfide anions. On the other hand, the electrochemical oxidation of polysulfide anions produces elemental sulfur ... 

Dipolar protic ethanol, methanol, water, liquid ammonia... 

White crystalline solid orthogonal plates or needles unstable density 1.21 g/cmS at 20°C melts at 33°C vaporizes at 58°C very soluble in water, liquid ammonia and lower alcohols sparingly soluble in most other organic solvents decomposes in hot water pKa 5.94 at 25°C. 

Physical properties of the solvent are used to describe polarity scales. These include both bulk properties, such as dielectric constant (relative permittivity), refractive index, latent heat of fusion, and vaporization, and molecular properties, such as dipole moment. A second set of polarity assessments has used measures of the chemical interactions between solvents and convenient reference solutes (see table 3.2). Polarity is a subjective phenomenon. (To a synthetic organic chemist, dichloromethane may be a polar solvent, whereas to an inorganic chemist, who is used to water, liquid ammonia, and concentrated sulfuric acid, dichloromethane has low polarity.)... 

Molecules in polar liquids such as water, liquid ammonia, sulfuric acid, and chloroform are held together by dipole-dipole and hydrogen bonding interactions. For molecules of comparable size, these are stronger than London forces resulting in the familiar trends in boiling points of nonmetal hydrides. For the heavier molecules, such as H2S, H,Se, PH3, and HI, dipole effects are not particularly important (the elec-... 

Ammonia is a colorless, pungent-smelling gas, consisting of polar, trigonal pyramidal NH3 molecules that have a lone pair of electrons on the N atom. Because of hydrogen bonding (Section 10.2), gaseous NH3 is extremely soluble in water and is easily condensed to liquid NH3, which boils at —33°C. Like water, liquid ammonia is an excellent solvent for ionic compounds. It also dissolves alkali metals, as mentioned in Section 6.7. 

Derivatives of alkaline, alkaline earth metals and phenols, naphtols, an-troles, etc. (pK> 10). These compounds are salts in their nature and, as the salts of strong bases and moderately weak acids, can exist in water solutions. They are soluble only in polar solvents (water, liquid ammonia), are prone to form adducts with phenols, water, etc., have high thermal stability and cannot be transferred into the gas phase. 

The salts (NH4)2Mo02S2 and (NH4)2W02S2 are soluble in water, liquid ammonia, dimethylsulfoxide, dimethylformamide, and morpholine but are practically insoluble in ethyl alcohol, ether, and carbon disulfide177. ... 

Ammonia dissolves alkali metals, barium, calcium and strontium and forms an unstable blue solution. This solution contains the metal ion and free electrons that slowly decompose, release hydrogen and form the metal amide. Compared to water, liquid ammonia is less likely to release protons (H+ ions), is more likely to take up protons (to form NH4+ ions) and is a stronger reducing agent219. 

These equations are analogous to those shown earlier for amphoteric behavior of Zn2+ and Al3+ in water, liquid ammonia, and liquid hydrogen fluoride. 

The rules given in Table 4.2 (p. 113) allow us to predict the solubility of a particular ionic compound in water. When sodium chloride dissolves in water, the ions are stabilized in solution by hydration, which involves ion-dipole interaction. In general, we predict that ionic compounds should be much more soluble in polar solvents, such as water, liquid ammonia, and liquid hydrogen fluoride, than in nonpolar solvents, such as benzene and carbon tetrachloride. Since the molecules of nonpolar solvents lack a dipole moment, they cannot effectively solvate the Na and Cl ions. Solvation is the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner. The process is called hydration when the solvent is water.) The predominant intermolecular interaction between ions and nonpolar compounds is ion-induced dipole interaction, which is much weaker than ion-dipole interaction. Consequently, ionic compounds usually have extremely low solubility in nonpolar solvents. 

Like water, liquid ammonia undergoes autoionization ... 

It is apparent from the above definition that a substance cannot act as an acid unless a base is present to accept the protons. Thus, acids will undergo complete or partial ionization in basic solvents such as water, liquid ammonia, or ethanol, depending on the basicity of the solvent and the strength of the acid. But in neutral or inert solvents, ionization is insignificant. However, ionization in the solvent is not a prerequisite for an acid-base reaction, as in the last example in the table, where picric acid reacts with aniline. 

MonocJLnjc prisms from methanol, mp 52.0-52.5". bp240 28s dj 1.104 di5 0.9782 dj 0.958, Heat of combustion (25 ) 9909.9 cal (15 )/g. Moderately sol in alcohol freely sol in carbon disulfide, ether, chloroform, amyl acetate sol in liquid sulfur dioxide practically insol in water, liquid ammonia. 

With the development of the definitions of acids and bases due to Bronsted and Lowry many solvents were found to which these definitions could be applied. It followed, therefore, that solvents were classified as proton containing solvents and proton-free solvents ". The former contain hydrogen in an ionizable form and the cations produced by auto-ionization are considered to be solvated protons. Typical proton-containing solvents are water, liquid ammonia, hydrazine, hydrogen cyanide, sulphuric acid, nitric acid, acetic and formic acids, alcohols and amides. Liquid hydrogen fluoride and the other hydrogen halides may also be included in this group of solvents. 

The zinc ion is also a fairly strong acid, and its insoluble compounds with solvent anions are often amphoteric. For example, in water, liquid ammonia, and glacial acetic acid the following reactions occur ... 

In comparing the relative strengths of acids and bases in a particular solvent such as water, liquid ammonia, or glacial acetic acid, the range of comparison is limited by the strength of the solvent as an acid or base. 

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