Aqueous solutions examples

To identify the major species in any aqueous solution, first categorize the solutes. A soluble salt, strong acid, or strong base generates the appropriate cations and anions as major species. Eveiy other solute generates its molecular species in solution. In addition, H2O is always a major species in aqueous solutions. Example provides practice in identifying the major species in solution. 

Oxide. Nature. Name of Salts. Salts in Aqueous Solution. Examples. Probable Ions in Solution,... 

The selectivity potentially offered by these reagents has attracted the attention of many workers who have proceeded on the assumption that these reagents will adsorb onto the surface of minerals with a selectivity for the metal ions of the lattice similar to that found in aqueous solution. Examples of this are dimethyglyoxime for nickel,6 cupferron for tin,5 salicylaldoxime for copper and 9-hy-droxyquinoline for lead and zinc minerals.7... 

Salt hydrates. These may be formed when R N+ or R3S+ salts crystallize from aqueous solution examples are Bu4N+PhC02-39.5H20 and (Bu3S)F-20H2O. 

Baird, N. C. Free Radical Reactions in Aqueous Solutions Examples from Advanced Oxidation Processes for Wastewater from the Chemistry in Airborne Water Droplets, J. Chem. Educ. 1997, 74, 817-819. 

Inorganic chemists, and coordination chemists in particular, frequently use stability constants (sometimes called formation constants) as indicators of bonding strengths (Table 10-1). These are the equilibrium constants for formation of coordination complexes, usually measured in aqueous solution. Examples of these reactions and corresponding stability constant expressions include the following ... 

Arrhenius Acid A substance that releases H+ ions in aqueous solutions. Examples include HI, HBr, HC1, and H.SO,. ... 

The concentration of the eonjugate base (or acid) generated from a weak acid (or base) is small, since, by definition, weak acids and bases are only slightly dissociated in aqueous solution. Examples of weak acids are organie acids (e.g., acetic) and of strong acids are mineral acids (e.g., hydrochloric and sulfuric). 

Insoluble nonswelling amphiphiles (H20). Lipids in this group have sufficient polarity to orient themselves at an air-water or air-oil interface, but do not interact with water sufficiently to dissolve in aqueous solutions. Examples of interest are cholesterol, triglyceride, the fat-soluble vitamins, and un-ionized fatty acids. 

The analysis of organic solvents presents some unique polyatomic interferences. Tables 10.24, 10.26, and 10.27 list potential polyatomic interfering species and the affected element. Some analysts add oxygen to the plasma when running organic solvents to minimize carbon (soot) formation on the cones. The additional oxygen can not only create the polyatomic species listed in Table 10.24 but can also react with some elements to form refractory oxides, as happens in aqueous solution. Examples include Ti 0, which interferes with Cu, and REE oxides, such as Nd 0, which interferes with Tb. 

Type of salt Nature of aqueous solution Examples... 

A salt composed of a weak base and a strong acid lowers the pH in aqueous solution. Conversely, a salt composed of a weak acid and a strong base raises the pH in aqueous solution. Examples are lidocaine hydrochloride (acid reaction) and sodium phenobarbital (alkaline reaction), respectively. When the pH of aqueous solutions of these substances is adjusted to pH = 7, lidocaine and phenobarbital, respectively, are partially formed again and precipitate. 

Using values of electrode potentials, decide which electrode reactions actually occur in the electrolysis of an aqueous solution. (EXAMPLE 20.13)... 

In this chapter we will consider only fully dissociated electrolytes. These are known as strong electrolytes in contrast with weak electrolytes which include, for example, acids such as ethanoic acid, CH3COOH, which are largely undissociated in aqueous solution. Example of strong electrolytes include aqueous solutions of HCl or KNO3. 

---