Solubility product table

With respect to C-parathion and Cl-toxaphene, protease-liberated flavoprotein was significantly more active than phosphate buffer in photodegrading these chemicals to ater-soluble products (Tables II and III). The amount of C-water-soluble products formed from parathion was 5-7 times greater in the presence than in the absence of flavoprotein. It should be noted that the presence of FMN in the mixture caused a slight grange in amount of water-soluble products formed (Table II). 

The galactoglucomannan of the holocellulose was degraded by the mannanase. The reaction was slow, but conversion showed a steady increase. After 80 hr of incubation, about 25% of the mannan was transformed into water-soluble products (Table I, Column 10). This figure was calculated on the basis of the mannose, glucose, and galactose present in the acid hydrolysate (cf. Experimental). 

ELECTROLYTES, EME, AND CHEMICAL EQUILIBRIUM TABLE 8.6 Solubility Product Constants Continued)... 

Table 1. Solubility and Solubility Products of Silver(I) Compounds...

Table 4. Soluble product yields from hydrogenation of bituminous coals...

Table 7. Elemental composition of soluble products from WVGS 13407 (daf)...

For the most part, the elemental analysis data for the blends are consistent with a weighted average of the individual components. Also shown is the elemental analysis for some of the soluble products form WVGS 13423 in Table 10 As was observed for the WVGS 13421 products, hydrogenation increased the total hydrogen content and decreased the atomic C/H ratio. 

The data given in Tables 1.9 and 1.10 have been based on the assumption that metal cations are the sole species formed, but at higher pH values oxides, hydrated oxides or hydroxides may be formed, and the relevant half reactions will be of the form shown in equations 2(a) and 2(b) (Table 1.7). In these circumstances the a + will be governed by the solubility product of the solid compound and the pH of the solution. At higher pH values the solid compound may become unstable with respect to metal anions (equations 3(a) and 3(b), Table 1.7), and metals like aluminium, zinc, tin and lead, which form amphoteric oxides, corrode in alkaline solutions. It is evident, therefore, that the equilibrium between a metal and an aqueous solution is far more complex than that illustrated in Tables 1.9 and 1.10. Nevertheless, as will be discussed subsequently, a similar thermodynamic approach is possible. 

Using AG tables in Appendix 1, calculate the solubility product constant, Rsp, for PbCl2 at 25°C. 

Solubility equilibrium constants, such as (20) and (22), are given a special name—the solubility product. It is symbolized K,p. A low value of K,p means the concentrations of ions are low at equilibrium. Hence the solubility must be low. Table 10-11 lists solubility products for some common compounds. 

Calculate the solubility, in moles per liter, of calcium sulfate in water, using the solubility product given in Table 10-11. 

Although the hydroxides of the alkaline earth elements become more soluble in water as we go down the column, the opposite trend is observed in the solubilities of the sulfates and carbonates. For example, Table 21-VII shows the solubility products of the alkaline earth sulfates. 

With the aid of a table of solubility products of metallic sulphides, we can calculate whether certain sulphides will precipitate under any given conditions of acidity and also the concentration of the metallic ions remaining in solution. Precipitation of a metallic sulphide MS will occur when [M2 + ] x [S2 ] exceeds the solubility product, and the concentration of metallic ions remaining in the solution may be calculated from the equation ... 

Values for the solubility products of metallic hydroxides are, however, not very precise, so that it is not always possible to make exact theoretical calculations. The approximate pH values at which various hydroxides begin to precipitate from dilute solution are collected in Table 11.2. 

The values for the solubility products of some sparingly soluble salts are listed in Table 11.4. 

The value of Kip is the same as that listed in Table 11.4. Many of the solubility products listed in tables were determined from emf measurements and calculations like this one. 

Seif-Test 12.10B Use the tables in Appendix 2B to calculate the solubility product of cadmium hydroxide, Cd(OH)2. 

The trivalent [P04] and [As04] ions react similarly. Examples of anions that give insoluble Hg(I) compounds in this way include halides, pseudohalides, halates, carboxylates and sulfate. A trace of HNO3 or HCIO4 is often added to the solution of the Hg(I) nitrate or perchlorate to prevent disproportionation induced by alkali. Table 1 lists common Hg(I) derivatives prepared in this way and includes values of the solubility products of the sparingly soluble Hg(I) compounds where these are measured. A similar reaction is used to prepare HgjCO, from a soluble bicarbonate ... 

Table 6. Free calcium concentrations in equilibrium with common complexing agents. A low free calcium concentration implies effective complexation, whether the complex formed is soluble or insoluble. The data were derived from either stability constants (soluble complexes) or solubility products (insoluble complexes).

Use the table below to answer question 4. Solubility Product Constants at 298K... 

We looked at a number of water soluble cosolvents (Table 28.3). In all cases aldehyde products were observed. 1,4-dioxane compares well with ethanol as a co-solvent. The data so far shows that 1,4-dioxane shows slightly lower olefin conversion after two hours than ethanol, but shghtly better selectivity. 

---