Using The Solubility Rules Provided, Determine If The Following Compounds Are Soluble Or Insoluble In Water. Write soluble Or insoluble On The Lines Provided Below.a. LiCl B. N A 3 P O 4 Na_3PO_4 N A 3 ​ P O 4 ​ C. A G 2 S Ag_2S A G 2 ​ S D. ( N H 4 ) 2 C O 3 (NH_4)_2CO_3 ( N H 4 ​ ) 2 ​ C O 3 ​

Introduction

In chemistry, solubility refers to the ability of a substance to dissolve in a solvent, typically water. Understanding the solubility rules is crucial in predicting whether a compound will dissolve in water or not. In this article, we will explore the solubility rules and apply them to determine the solubility of four compounds in water.

Solubility Rules

The solubility rules are a set of guidelines that help predict the solubility of compounds in water. These rules are based on the chemical properties of the ions involved and are as follows:

• Group 1A (Alkali Metals) Compounds: All compounds of Group 1A metals (Li, Na, K, Rb, Cs, and Fr) are soluble in water.
• Group 2A (Alkaline Earth Metals) Compounds: Compounds of Group 2A metals (Mg, Ca, Sr, Ba, and Ra) are generally insoluble in water, except for those with nitrate (NO3-) and ammonium (NH4+) ions.
• Halides: Most halides (chlorides, bromides, iodides, and fluorides) are soluble in water, except for those of silver (Ag), lead (Pb), and mercury (Hg).
• Carbonates: Compounds of carbonates (CO32-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.
• Phosphates: Compounds of phosphates (PO43-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.
• Sulfides: Compounds of sulfides (S2-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.

Applying Solubility Rules to Compounds

Now that we have discussed the solubility rules, let's apply them to the four compounds listed:

a. LiCl

• Group 1A (Alkali Metals) Compounds: LiCl is a compound of a Group 1A metal (Li) and a halide (Cl-). According to the solubility rules, all compounds of Group 1A metals are soluble in water.
• Conclusion: LiCl is soluble in water.

b. $Na_3PO_4$

• Group 1A (Alkali Metals) Compounds: $Na_3PO_4$ is a compound of a Group 1A metal (Na) and a phosphate (PO43-). According to the solubility rules, compounds of Group 1A metals with phosphate ions are soluble in water.
• Conclusion: $Na_3PO_4$ is soluble in water.

c. $Ag_2S$

• Halides: $Ag_2S$ is a compound of a halide (S2-) and a silver (Ag) ion. According to the solubility rules, most halides are soluble in water, except for those of silver (Ag), lead (Pb), and mercury (Hg).
• Conclusion: $Ag_2S$ is insoluble in water.

d. $(NH_4)_2CO_3$

• Carbonates: $(NH_4)_2CO_3$ is a compound of a carbonate (CO32-) and an ammonium (NH4+) ion. According to the solubility rules, compounds of carbonates are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.
• Conclusion: $(NH_4)_2CO_3$ is soluble in water.

Conclusion

In conclusion, the solubility rules provide a useful guide for predicting the solubility of compounds in water. By applying these rules to the four compounds listed, we have determined that LiCl and $Na_3PO_4$ are soluble in water, while $Ag_2S$ is insoluble in water. $(NH_4)_2CO_3$ is also soluble in water, as it contains an ammonium ion.

References

• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.
• Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.

Further Reading

• Solubility rules: A comprehensive guide to predicting solubility in water
• Chemistry: A guide to understanding chemical reactions and properties
• Solubility: A key concept in chemistry and its applications
  Solubility Rules Q&A: Frequently Asked Questions and Answers ====================================================================

Introduction

In our previous article, we discussed the solubility rules and applied them to determine the solubility of four compounds in water. In this article, we will answer some frequently asked questions related to solubility rules and provide additional information to help you better understand this concept.

Q&A

Q1: What are the solubility rules?

A1: The solubility rules are a set of guidelines that help predict the solubility of compounds in water. These rules are based on the chemical properties of the ions involved and are as follows:

• Group 1A (Alkali Metals) Compounds: All compounds of Group 1A metals (Li, Na, K, Rb, Cs, and Fr) are soluble in water.
• Group 2A (Alkaline Earth Metals) Compounds: Compounds of Group 2A metals (Mg, Ca, Sr, Ba, and Ra) are generally insoluble in water, except for those with nitrate (NO3-) and ammonium (NH4+) ions.
• Halides: Most halides (chlorides, bromides, iodides, and fluorides) are soluble in water, except for those of silver (Ag), lead (Pb), and mercury (Hg).
• Carbonates: Compounds of carbonates (CO32-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.
• Phosphates: Compounds of phosphates (PO43-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.
• Sulfides: Compounds of sulfides (S2-) are generally insoluble in water, except for those of Group 1A and ammonium (NH4+) ions.

Q2: What is the difference between soluble and insoluble compounds?

A2: Soluble compounds are those that can dissolve in water, while insoluble compounds are those that cannot dissolve in water. Soluble compounds typically have ions that are highly polar or have a high charge density, which allows them to interact with water molecules and dissolve.

Q3: How do I determine the solubility of a compound?

A3: To determine the solubility of a compound, you can use the solubility rules. First, identify the ions involved in the compound and determine their solubility based on the rules. If the compound contains ions that are soluble, it is likely to be soluble in water. If the compound contains ions that are insoluble, it is likely to be insoluble in water.

Q4: What are some common exceptions to the solubility rules?

A4: Some common exceptions to the solubility rules include:

• Silver (Ag) compounds: Most silver compounds are insoluble in water, except for those with chloride (Cl-) and nitrate (NO3-) ions.
• Lead (Pb) compounds: Most lead compounds are insoluble in water, except for those with nitrate (NO3-) and chloride (Cl-) ions.
• Mercury (Hg) compounds: Most mercury compounds are insoluble in water, except for those with chloride (Cl-) and nitrate (NO3-) ions.

Q5: Can I use the solubility rules to predict the solubility of a compound in a solvent other than water?

A5: No, the solubility rules are specific to water and cannot be used to predict the solubility of a compound in a solvent other than water. The solubility of a compound in a solvent other than water will depend on the specific properties of the solvent and the compound.

Conclusion

In conclusion, the solubility rules provide a useful guide for predicting the solubility of compounds in water. By understanding the solubility rules and applying them to specific compounds, you can determine whether a compound is soluble or insoluble in water. Remember to consider any exceptions to the solubility rules and to use the rules only for compounds in water.

References

• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.
• Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.

Further Reading

• Solubility rules: A comprehensive guide to predicting solubility in water
• Chemistry: A guide to understanding chemical reactions and properties
• Solubility: A key concept in chemistry and its applications