Ionic equivalent stoichiometric

Values of limiting molar ionic conductivities for a few common ions are shown in Table 1. The data tabulated are referred to 25°C temperature. The term limiting molar ionic conductivity is used according to lU-PAC recommendation, rather than the formerly used limiting ionic equivalent conductivity. The molar and equivalent values are interconvertible through stoichiometric coefficient z. 

Many others confirmed later the existence of two different species, stoichiometrically equivalent to H atoms, but different in reactivity. An unequivocal proof, however, that the neutral form is e aq, has been obtained by Czapski and Schwarz (12). They showed that the ionic strength effect on reactions of e aq was indeed as expected with unit negatively charged species. This result was verified by other workers (11). 

Ion exchange is a reversible and stoichiometric process with every ion removed from solution replaced by an equivalent amount of another ionic... 

The precipitation of AgX out of solution drives the equilibrium to the right. Similar to acid-base titrations, potentiometric titrations measure the volume of a solution of one reactant that is required to completely react with a measured amount of another reactant, or until the equivalence point (or stoichiometric point) is reached. At the equivalence point, the silver nitrate has reacted stoichiometrically with all of the ionic halide present in your sample solution. In our case, the numbers of moles of halide and silver ions are equal, equation (2.11). 

The synthesis of the azetidin-2-one nucleus, via the classical annulation of acetyl-chlorides with imines, requires more than stoichiometric amounts of Uiethylamine (about 3 equivalent), which cannot be recovered and reused. In addition, the procedure needs a large amount of organic solvents (VOCs) and, as a consequence, causes a large amount of waste. To overcome these difficulties, the possible ytterbium (III) triflate-catalysed stereoselective synthesis of P-lactams via [2+2] cyclocondensation in ionic liquids has been investigated by Su et al. (Scheme 16.4) [93]. 

The technique is generally unaffected by the state (ionic, imdissociated, sometimes complexed) of the analyte to be titrated. For example, the direct potentiometric determination of pH in a solution of a weak acid reports only the hydrogen ion concentration. Since the major portion of the acid is present in the undissociated form, direct potentiometry can not provide data yielding the total acid concentration. Potentiometric titration involves titrating the acid solution with a standard base, determining the equivalence point volume of standard base solution used, and calculating the total weak acid concentration from the stoichiometric data. 

We have already seen an example earlier with the formation of [PtCl2(NH3)2], driven in this case by low solubility of this neutral species allowing it to crystallize out of the reaction mixture rather than continue reaction to form ionic [Pt(NH3)4]2+. Another way to achieve partial substitution is through, use of a stoichiometric amount of a reagent. For example, reaction (6.9) may occur, where only one of two available coordinated chloride ions are substituted because of the availability of only one molar equivalent of added cyanide anion. 

The volume of the FeS04 solution is given in the problem. Therefore, we need to find the nnmber of moles of FeS04 to solve for the molarity. From the net ionic equation, what is the stoichiometric equivalence between Fe" and MnO How many moles of KMn04 are contained in 16.42 mL of 0.1327 M KMn04 solution ... 

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