Determination of the solubility

The amount of substance dissolved depends, not only on the substance, but also on the temperature j and the solubility of a substance, or the number of grams of substance dissolved by a given weight of the solvent, may either increase or decrease with rise of temperature. In all cases, however, whatever be its particular form, the solubility curve of any substance is continuous, so long as the solid phase, or solid substance in contact with the solution, remains unchanged. If, however, a change in the solid phase occurs, the solubility curve will show a break or discontinuous change in direction. [Pg.302]

For the production of the equilibrium between a solid and a liquid, i.e. for the production of a saturated solution, time is necessary and the length of time required not only varies with the state of subdivision of the solid, and the efficiency of the shaking or stirring, but is also dependent on the nature of the substance. In all cases, therefore, care must be taken that sufficient time is allowed for equilibrium to be established more especially when changes in the solid phase may occur. [Pg.302]

Determination of the Solubility.—The production of a saturated solution is most simply carried out in the apparatus shown in Fig. loo. It consists of a tube, a, in which the solid and solvent are placed, and vigorously stirred by means of the glass screw stirrer shown at b. The stem of the latter passes through a glass tube, inserted in the rubber stopper by which the solubility tube is closed. The tube should be chosen of such a size that the stem of the stirrer just passes through, the bearing being well lubricated by means of vaseline. [Pg.302]

When the temperature of experiment is fairly high, it may be necessary to warm the pipette first before withdrawing the solution otherwise solid may separate out in the pipette. [Pg.303]

Instead of an ordinary pipette, one may also use a graduated pipette like that shown in Fig. loi. This has the advantage that it allows of the determination of the density of the solutions at the same time. The volume of the tube, up to different marks on the scale, is first determined by filling with [Pg.303]

Determination of the Solubility of Ferric Phosphate in Phosphating Solutions Using Radioiron , US Department of Commerce, Office of Technical Services, Rep. No. PB 111, 399 (1953)... [Pg.720]

The question as to which rule has the greatest influence on the dissolution, Tb(SS) or Tb(WS), was addressed in another study. Again using the fo (solute) attribute as an indication of the extent of dissolution, the results from variations in these two rule sets are compared. The studies indicated that the T b(SS) and J(SS) rules had the greatest influence. This result suggest that the self-affinity of a solute, reflected by the Pb(SS) value, is a greater determinant of the solubility than the hydropathic state, reflected by the Pb(WS) value [5]. The validity of these findings is open to debate. [Pg.65]

Siemann, U., Densitometric determination of the solubility parameters of biodegradable polyesters, Proc. Int. Symp. Control. Rel. Bioact. Mater., 12, 53, 1985. [Pg.33]

Pore water extraction and determination of the soluble salt content of soils by refractometer... [Pg.187]

Glew, D.N., Roberson, R.E. (1956) The spectrophotometric determination of the solubility of cumene in water by a kinetic method. J. Phys. Chem. 60, 332-337. [Pg.52]

May, W. E., Wasik, S. P., Freeman, D. H. (1978b) Determination of the solubility behavior of some polycyclic aromatic hydrocarbons in water. Anal. Chem. 50, 997-1000. [Pg.55]

Natarajan, G.S., Venkatachalam, K.A. (1972) Solubilities of some olefins in aqueous solutions. J. Chem. Eng. Data 17, 328-329. Nelson, H.D., De Ligny, C.L. (1968) The determination of the solubilities of some n-alkanes in water at different temperatures by means of gas chromatography. Rec. Trav. Chim. Payus-Bae (Recueil) 87, 528-544. [Pg.401]

To construct a triangular diagram consisting of two enantiomers and the solvent at constant temperature requires the determination of the concentration of the saturated solutions as a function of the total composition of the system, and the number and nature of the solid phases in equilibrium with the saturated solution. The determination of the solubility of mixtures of enantiomers is... [Pg.371]

Spencer, J.N. and A.F. Voigt. 1961. Thermodynamics of the solution of mercury metal. I. Tracer determination of the solubility in various liquids. Jour. Phys. Chem. 72 464-470. [Pg.439]

The following formula is generally applied for the determination of the solubility of oxygen in (clean) water in equilibrium with the atmosphere ... [Pg.86]

Gross, P. The determination of the solubility of slightly soluble liquids in water and the solubilities of the dichloroethanes and... [Pg.1663]

Korenman, I.M. and Aref eva, R.P. Determination of the solubility of liquid hydrocarbons in water, Otkrytiya Izobret. Prom. [Pg.1681]

McNally, M.E. and Grob, R.L. Determination of the solubility limits of organic priority pollutants by gas chromatographic headspace analysis, J. Chromatogr. A, 260 23-32, 1983. [Pg.1695]

Robb, l.D. Determination of the solubility of vinyl stearate in water by a monolayer technique. Colloid PoIym.ScI, 209 (2) 162-... [Pg.1715]

The most important applications of Cu ISEs are in the direct determination of Cu " in water [169, 372,410], complexometric titration of various metal ions using Cu " as an indicator [30, 143,269, 385] and complexometric titrations of Cu " [409]. This ISE has also been used in the determination of the equilibrium activity of Cu in various Cu complexes in order to determine the stability constants (see [46, 285, 317, 318,427, 445]), in the determination of the solubility of poorly soluble salts [122] and in the determination of the standard Gibbs transfer energies [58]. It can also be used in concentrated electrolytes [170]. [Pg.149]

Solubility diagrams have nearly always been calculated using solubility and stability constants. Experimental determination of the solubility of iron oxides as a function of pH has been concerned predominately with ferrihydrite. Lengweiler et al. [Pg.205]

Vlek, P.L.G. Blom,Th.J.M. Beek, J. Lindsay, W.L. (1974) Determination of the solubility product of various iron hydroxides and jaro-site by the chelation method. Soil Sci Soc. Am. Proc. 38 429-432... [Pg.640]

Over the last 20-30 years not too much effort has been made concerning the determination of standard potentials. It is mostly due to the funding policy all over the world, which directs the sources to new and fashionable research and practically neglects support for the quest for accurate fundamental data. A notable recent exception is the work described in Ref. 1, in which the standard potential of the cell Zn(Hg)jc (two phase) I ZnS O4 (aq) PbS O4 (s) Pb(Hg)jc (two phase) has been determined. Besides the measurements of electromotive force, determinations of the solubility, solubiKty products, osmotic coefficients, water activities, and mean activity coefficients have been carried out and compared with the previous data. The detailed analysis reveals that the uncertainties in some fundamental data such as the mean activity coefficient of ZnS04, the solubility product of Hg2S04, or even the dissociation constant of HS04 can cause uncertainties in the f " " values as high as 3-4 mV. The author recommends this comprehensive treatise to anybody who wants to go deeply into the correct determination of f " " values. [Pg.19]

Reliable determination of the solubility of silica in water has been complicated by the effects of impurities and of surface layers that may affect attainment of equilibrium. The solubility behavior of silica has been discussed (9,27). Reported values for the solubility of quartz, as Si02, at room temperature are in the range 6—11 ppm. Typical values for massive amorphous silica at room temperature are around 70 ppm for other amorphous silicas, 100—130 ppm. Solubility increases with temperature, approaching a maximum at about 200°C. Solubility appears to be at a minimum at about pH 7 and increases markedly above pH 9 (9). [Pg.471]

In essence there are three ways of determining these constants, namely, conductimetry 195,886), potentiometry 184, 289,887, 866), and the determination of the solubility of sparingly soluble metallic salts in presence of triphosphate (I48, 167, 335). [Pg.34]

Thus the solution always contains Mg in approximately constant abundance, which makes it effectively a perfectly mobile component. The same is true for H+ since pH changes little after precipitation of the sepiolite even though the reaction consumes (OH). The experimental system is then "open" with respect to these two components. A determination of the solubility product constant of a natural iron-calcium-aluminous sepiolite confirms generally the above results (Christ, et al , 1973). [Pg.143]

Chlorine and bromine are fairly soluble in water iodine has a low solubility. Early determinations of the solubility of chlorine in water were made by J. L. Gay Lussac1 in 1839, by J. Pelouze in 1843, and by F. Sohonfeld in 1855. They noticed a maximum in the solubility curve in the vicinity of 10°, and at 100° the solubility is nil. Later determinations have been made by H. W. B. Roozeboom in 1885, and by L. W. Winkler in 1907. At temp, below 9 6°, chlorine forms a crystalline hydrate, C12.8H20 and this corresponds with the maximum in the solubility curve. The solubility curves of the gases chlorine and bromine 2 are indicated in Table III. [Pg.71]

N. Schoor] and A. Regenborn say that owing to the ready formation of hydrogen iodide, accurate determinations of the solubility in aq. alcohol can be made only by making a sat. soln. of iodine in absolute alcohol, diluting the soln., and determining the iodine at once. The solubility follows a fairly regular course ... [Pg.86]

The terminal numbers with potassium, rubidium, and csesium nitrates represent the b.p. of sat. soln. at nearly normal press. for sodium nitrate the corresponding value is 67 6 (119°). Determinations of the solubility of sodium nitrate have been made by G. J. Mulder, Earl of Berkeley, A. Ditte, L. Maumene, A. fitard, etc.30 The solubility curve of sodium nitrate has been carried upwards 781 (180°), 83 5 (220°), 915 (225°), and 100 (313°), the last-named temp, represents the m.p. of the salt. According to L. C. de Coppet, the eutectic or cryohydric temp, of sodium nitrate is —18"5°, and the eutectic mixture is not a definite hydrate, NaN03.7H20, as A. Ditte once supposed. A. fitard represents the solubility S... [Pg.815]

Determinations of the solubility of ammonium nitrate in water for a few temp. [Pg.838]

Determination of the Solubility Products of Sparingly Soluble Salts... [Pg.217]

Big Chemical Encyclopedia

Chemical substances, components, reactions, process design ...