Salts, solubility table

The composition of the subsurface gas phase may change as a result of gas dissolution into the liquid phase. The solubility of gases in water depends on the type of gas, temperature, salt concentration, and the partial pressure of the gases in the atmosphere. The most soluble gases are those that become ionized in water (CO, NHj, H S), while and are much less soluble (Table 1.2). 

If activity coefficients arc iunorcd la-Mimcd lo bo unity a gro s approximation responsible lor the noii-quantitative connection between chances in Gibbs energy ol solution and actual salt solubilities), it is possible to draw up a table of values of the change in (iibbs energy for the solution of a compound in water that might be expected for various solubilities. Table. Tin contains the calculations of A , (/ for various solubilities of I I ionic compounds. The calculations arc based on the approximate relationship ... 

As a rule, lanthanide bromides, and more especially the iodides, are more reactive because of their often higher solubility (Table 5), and also show enhanced thermodynamic lability (Scheme III). Moreover, reactivities different from those of the chloride analogues should be expected because of, for example, the softer Lewis basicity of the iodide anion and different solubility properties of the eliminated alkali salts. Table 5 gives an arbitrary sample of solubilities for lanthanide halides in various standard-laboratory donating solvents [97f]. 

Solubility tables arc naturally utilized for regulating selective dissolutions but in using them the effects of other soluble compounds on the solubility of the compound in question must be determined as its effect may be quite marked. For instance in Fig. 4, (vurve 1 shows the solubility of sodium sulphate in pure water while Curve 2 shows its solubility in a solution of salt. ... 

KOi-Bu is often used in academia as a moderately strong base.The use of KOf-Bu on scale may be hampered by its relatively low solubility in organic solvents. The salts of i-AmOH have much greater solubility (Table 3.6) and should be considered for use on scale in place of KOi-Bu. NaOi-Am and KOt-Am are readily available. 

The solubilities of ionic salts have wide range. For instance, in contrast to silver perchlorate (AgC104), which has a solubility of 55.7 g per 100 g of water, only 0.00018 g of silver chloride (AgCl) can dissolve in 100 g of water. If the maximum amount of solute dissolved in 100 g of water is less than 0.1 g, this solute is said to be insoluble. The solute that has a solubility range from 0.1 g to 1 g is called slightly soluble. If the amount of solute is more than 1 g, then it is soluble. Silver perchlorate is a soluble compound but silver chloride is an insoluble compound in water. It is not necessary to memorize the solubilities of substances. Solubility tables (e.g.,Table 2) help you determine whether a substance is soluble, insoluble, or slightly soluble in water. 

The solubility table shows us that Ag+ and Cr042- ions form an insoluble salt, Ag2Cr04, but that NaN03 is soluble. The equation, therefore, is... 

This is an acid-base neutralization reaction the products are H2O and the salt that contains the cation of the base, Ca, and the anion of the acid, L Cal2 is a soluble salt (solubility guideline 4). HI is a strong acid (see Table 4-5), Ca(OH)2 is a strong base (see Table 4-7), and Cal2 is a soluble ionic salt, so all are written in ionic form. 

HCN has the chemical synonyms of formonitrile, pmssic acid, and hydrocyanic acid. Some physicochemical properties are compared with those of the sodium, potassium, and calcium salts in Table 14.1. Relevant to the toxicity and hazards of HCN are its hquid state at NTP, poor ionization, low molecular weight (MW), low boiling point, high vapor pressure, low vapor density (0.947 at 31°C), and hence ready diffusibility. The salts are sohds that are readily soluble in water, ionize, and in spite of low vapor pressure they hydrolyze in moist conditions with the hberation of HCN, this being markedly increased under acidic conditions. 

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