Solubility guidelines, for ionic

Solubility guidelines for ionic compounds in water at room temperature... 

Active Figure 9.13 Solubility guidelines for ionic compounds. If a compound contains at least one of the ions in the Solnble Compounds list, apart from the exceptions listed, it is likely to be at least moderately soluble in water. Componnds with at least one ion in the Insoluble Compounds list are poorly soluble in water (again, with the exception of the few compounds in the Exceptions list). Watch this Active Figure at http //now.brookscole.com/cracolice3e. 

The final step in predicting the outcome of such a reaction is to determine which of the products, if any, will precipitate from solution. We do this using the solubility guidelines for ionic compounds (Tables 4.2 and 4.3). The first product (NaOH) contains a Group 1A cation (Na ) and will therefore be soluble. We indicate its phase as aq). The second product (BaS04) contains the sulfate ion (SO ). Sulfate compounds are soluble unless the cation is Ag, Hg, Ca ,... 

Solubility Guidelines for Common Ionic Compounds in Water Generally Soluble Exceptions... 

How do you know which ionic compounds are soluble and which are not In your previous chemistry course, you learned a set of solubility guidelines. Table 9.3 summarizes these guidelines. Remember the higher guideline takes precedence. (For instance, guideline 3 says that carbonates have very low solubility. Sodium carbonate is soluble, however, because guideline 1 says that ionic compounds containing sodium are soluble.) Chemists do not usually work with solubility products for soluble compounds. Thus, you will not find soluble ionic compounds listed in tables. If you see a compound in a A p table, you know that it has a low solubility relative to compounds such as sodium chloride. 

Use the general solubility guidelines to name three reagents that will combine with each ion below to form a precipitate. Assume that the reactions take place in aqueous solution. For each reaction, write the net ionic equation. 

Both silver nitrate and copper(II) nitrate are soluble ionic compounds (for solubility guidelines see page 134 and Table 4-8). 

Exercises 69 and 70 describe precipitation reactions in aqueous solutions. For each, write balanced (i) formula unit, (ii) total ionic, and (hi) net ionic equations. Refer to the solubility guidelines as necessary. 

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