Kielland table

Step 4. I = j([NH4] + [Cl"]) = 0.06 M, other ions being negligible. Since the hydronium required is stated as an activity, we need only /+ for the NH4 ion. Taking the activity coefficient from the Kielland Table A-1 of Appendix A-1, we obtain... 

Calculate the H of a buffer made with analytical concentrations 0.200 M lactic acid and 0.100 M sodium lactate. Repeat after a 100-fold dilution of the solution and compare the need for the full equation (3-2) in each case. Take a constant ionic strength of 0.10 M in both cases and use / values from the Kielland table in Appendix A-1, assuming lactate ion is about the same size as acetate. The reported pX° for lactic acid is 3.858. It is CH3CH(OH)COOH. 

Only the positive root has physical significance in these problems.) One then calculates a better effective value for this ionic strength with the Kielland table (Appendix A-1) and continues until an unchanging solubility about 0.053 M is obtained. 

Normal serum calcium level in man is 4.5-5.5 x IO m. About 40 % of this is bound to protein (nondialyzable) and is not in rapid equilibrium with the solution. Thus, we use about 3 x 10 m for the available calcium(II). Similarly, there is about 1 x 10 available phosphates, mainly H2PO4 and HPO (see a diagrams). This is higher in children during bone-forming years. First, we might ask whether these levels are near or above saturation for the solids listed above. To find the appropriate phosphate ion concentration, we need only multiply the total available phosphates by the a value for blood serum pH, 7.40. We use the Kielland table (Appendix A-1) values of activity coefficients to adjust the K values to / = 0.1 M. The / values are for Ca ", 0.405 for P04 , 0.095 for HPO , 0.37 for OH , 0.755. This produces new conditional K values for the set(ll-5a)-(ll-5e) ... 

This time, let us take the total dissolved iron as 0.01 M and ionic strength 0.1 M (this comes about because ot the higher charges, the factor, and because some acid will be required in practice to prevent FeOH " and other basic ion formation). Estimated iron(II) and ir6n(III) activity coefficients are 0.405 and 0.18 (Kielland table Appendix A-1). So, the activities of each at their maxima are... 

Table A-1. Kielland Table of Ionic Activity Coefficients Arranged by the Sizes of Ions... 

Table 8.5 Effective ion diameters (A) for various ions and inorganic complexes in aqueous solution (after Kielland, 1937).

Kielland has estimated values of x for numerous ions from a variety of experimental data. His best values for effective diameters are given in Table 10-2. Also presented are activity coefficients calculated from Equation iO-5 using these values for the size parameter. 

Activity coefficients are found in Appendix A-1, Tables A-1 and A-2, and in Kielland and Hamer. ... 

Some of the elements of SEMS that were a factor in this incident are shown in Table 2.5. Those elements that are pertinent to the Alexander L. Kielland event are italicized. 

Table 2.5 Elements of a Safety Management System—Kielland...

From the ionic sizes reported by Kielland, values of a were estimated as equal to the mean value of the effective radii of the hydrated ionic species of the electrolyte. Two different methods were used to calculate the diameters of inorganic ions, hydrated to a different extent from the crystal radius and deformability, accordingly to Bonino s equation for cations, and from the ionic mobilities. The calculated values taking this methodology are presented in Tables 2.1-2.10. 

Tables 2.1-2.4 relative to sodiiun, lithium, potassium, rubidium, and cesium salts, also show that, in general, the values of a obtained by fitting experimental data of activity coefficients are larger than the sum of ionic radii in solutions (or crystal-lattice spacing) and the interatomic distances, d. Also they are close to the values obtained from Kielland sdata and toab initio values calculated by using two models model I and model II, considering the absence and the presence of five water molecules between anion and cation, optimized in the gas phase, respectively), and also to those obtained fi om MM studies, where no water molecules are consid-...

Table 3.1 summarizes a values of 20 acids in aqueous solution, determined from different experimental techniques and/or theoretical approaches, informing us that one estimation of this parameter, at least, was done for every system. Table 3.1 also shows that, in general, the values of a obtained by fitting experimental data of diffusion and activity coefficients are similar but smaller than those obtained from Kielland sdata. This fact could be interpreted on the basis that some effects such as ion-ion and ion-solvent... 

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