what are the rules used to determine the solubility of salt?
Solubility Rules:
1. Salts of group 1 and ammonia are soluble.
2. Acetates and nitrates are soluble.
3. Binary compounds of group 17, except F, are soluble with metals,
except Ag, Hg+, and Pb.
4. All sulfates are soluble, except those of Ba, Sr, Pb, Ca, Ag, and Hg+ .
5. Except for those in rule 1, carbonates, hydroxides, oxides, sulfides,
and phosphates are insoluble.
how do you determine the solubility of the following salts:
1. AgNO3
2. Ag2SO4
3. HgCl2
4. BaSO4
5. CaCl2
6. NH4OH
7. PbCl4
8. Mg(C2H3O2)2
9. HgCl
10. CaF2
11. CuO
12. AgI
13. Al(OH)3
14. Fe2(CO3)3
15. CrPO4
16. K2S
You follow the rules Kelly gave you.
Are these right? I didn't know some of them.
1. AgNO3
Soluble, rule 3
2. Ag2SO4
Insoluble, rule 4
3. HgCl2
Insoluble, rule 2
4. BaSO4
Insoluble, rule 4
5. CaCl2
Soluble, rule 2
6. NH4OH
?
7. PbCl4
Insoluble, rule 2
8. Mg(C2H3O2)2
Soluble, rule 3
9. HgCl
Soluble, rule 2
10. CaF2
?
11. CuO
?
12. AgI
Insoluble, rule 2
13. Al(OH)3
Insoluble,
14. Fe2(CO3)3
Insoluble, rule 5
15. CrPO4
Insoluble, rule 5
16. K2S
?
1. AgNO3
Soluble, rule 3
2. Ag2SO4
Insoluble, rule 4slightly soluble
3. HgCl2 soluble. Hg2Cl2 is insol.
Insoluble, rule 2
4. BaSO4
Insoluble, rule 4
5. CaCl2
Soluble, rule 2
6. NH4OHThis is NH3 + H2O and technically there is no NH4OH
?
7. PbCl4PbCl2 is the common chloride. PbCl4 can form but with some difficulty.
Insoluble, rule 2
8. Mg(C2H3O2)2
Soluble, rule 3
9. HgCl Usually written as Hg2Cl2 and it is insoluble
Soluble, rule 2
10. CaF2
?insoluble
11. CuO
?insoluble
12. AgI
Insoluble, rule 2
13. Al(OH)3
Insoluble,
14. Fe2(CO3)3
Insoluble, rule 5
15. CrPO4
Insoluble, rule 5
16. K2S
? soluble
The solubility of salt, or any substance, can be determined by various factors. The primary factors that affect the solubility of salt include temperature, pressure, and the presence of other substances. The following explanation will help you understand how these factors influence the solubility of salt:
1. Temperature: The solubility of most solid solutes, including salt, generally increases with increasing temperature. This means that more salt can dissolve in a given amount of water at higher temperatures compared to lower temperatures. This rule applies to many salts, but some exceptions exist.
2. Pressure: Unlike gases, the solubility of a solid salt is not significantly affected by changes in pressure.
3. Nature of the solvent: The solubility of salt also depends on the nature of the solvent or the substance in which it is dissolved. Salt, which is composed of positive sodium ions (Na+) and negative chloride ions (Cl-), readily dissolves in polar solvents like water. The polar nature of water allows it to attract and surround the ions, causing the salt to dissociate and dissolve.
4. Presence of other substances: The presence of other substances, such as other salts or solutes, can affect the solubility of salt. For instance, adding a salt that shares a common ion with the dissolved salt can reduce its solubility due to the common ion effect. This effect arises because the shared ion competes for the available solvent molecules, making it more difficult for the salt to dissolve completely.
To determine the specific solubility of a particular salt, it is important to refer to solubility tables or experimental data, which provide information on the maximum amount of salt that can dissolve in a given quantity of solvent at various temperatures. These tables often list solubility values in grams per 100 milliliters (g/100 mL) or other standardized units for easy comparison.