Is Each Compound Soluble Or Insoluble?(a) NiS (b) $Mg_3(PO_4)_2$ (c) $Li_2CO_3$ (d) $ N H 4 C L NH_4Cl N H 4 ​ Cl [/tex]

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Introduction

Solubility is a fundamental concept in chemistry that deals with the ability of a substance to dissolve in a solvent. It is a crucial property that determines the behavior of compounds in various chemical reactions and processes. In this article, we will discuss the solubility of four compounds: NiS, Mg3(PO4)2, Li2CO3, and NH4Cl. We will examine the rules governing solubility and apply them to determine whether each compound is soluble or insoluble.

Solubility Rules

Before we dive into the specific compounds, let's review the basic solubility rules:

  • Sulfates (SO42-): Most sulfates are soluble, except for those of barium (Ba2+), strontium (Sr2+), and lead (Pb2+).
  • Carbonates (CO32-): Most carbonates are insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+).
  • Phosphates (PO43-): Most phosphates are insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+).
  • Chlorides (Cl-): Most chlorides are soluble, except for those of silver (Ag+), lead (Pb2+), and mercury (Hg2+).
  • Nitrates (NO3-): Most nitrates are soluble.

Solubility of NiS

Nickel sulfide (NiS) is a compound that consists of nickel (Ni2+) and sulfide (S2-) ions. Based on the solubility rules, we know that sulfides are generally insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+). Since nickel (Ni2+) is not one of these exceptions, we can conclude that NiS is insoluble.

Solubility of Mg3(PO4)2

Magnesium phosphate (Mg3(PO4)2) is a compound that consists of magnesium (Mg2+) and phosphate (PO43-) ions. Based on the solubility rules, we know that phosphates are generally insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+). Since magnesium (Mg2+) is not one of these exceptions, we can conclude that Mg3(PO4)2 is insoluble.

Solubility of Li2CO3

Lithium carbonate (Li2CO3) is a compound that consists of lithium (Li+) and carbonate (CO32-) ions. Based on the solubility rules, we know that carbonates are generally insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+). Since lithium (Li+) is one of these exceptions, we can conclude that Li2CO3 is soluble.

Solubility of NH4Cl

Ammonium chloride (NH4Cl) is a compound that consists of ammonium (NH4+) and chloride (Cl-) ions. Based on the solubility rules, we know that chlorides are generally soluble, except for those of silver (Ag+), lead (Pb2+), and mercury (Hg2+). Since ammonium (NH4+) is not one of these exceptions, we can conclude that NH4Cl is soluble.

Conclusion

In conclusion, we have examined the solubility of four compounds: NiS, Mg3(PO4)2, Li2CO3, and NH4Cl. Based on the solubility rules, we have determined that:

  • NiS is insoluble
  • Mg3(PO4)2 is insoluble
  • Li2CO3 is soluble
  • NH4Cl is soluble

Understanding the solubility of compounds is crucial in various chemical reactions and processes. By applying the solubility rules, we can predict the behavior of compounds and make informed decisions in laboratory settings and industrial applications.

References

  • Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
  • Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science (13th ed.). Pearson Education.
  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2016). General chemistry: Principles and modern applications (11th ed.). Pearson Education.

Note: The references provided are a selection of popular chemistry textbooks that cover the topic of solubility. They are not an exhaustive list, and readers are encouraged to consult additional resources for further information.

Introduction

In our previous article, we discussed the solubility of four compounds: NiS, Mg3(PO4)2, Li2CO3, and NH4Cl. We applied the solubility rules to determine whether each compound is soluble or insoluble. In this article, we will address some common questions related to solubility and provide additional information to help readers better understand this concept.

Q: What is solubility?

A: Solubility is the ability of a substance to dissolve in a solvent. It is a measure of how much of a substance can dissolve in a given amount of solvent.

Q: What are the solubility rules?

A: The solubility rules are a set of guidelines that help predict the solubility of compounds. They are based on the behavior of ions in solution and are as follows:

  • Sulfates (SO42-): Most sulfates are soluble, except for those of barium (Ba2+), strontium (Sr2+), and lead (Pb2+).
  • Carbonates (CO32-): Most carbonates are insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+).
  • Phosphates (PO43-): Most phosphates are insoluble, except for those of sodium (Na+), potassium (K+), and ammonium (NH4+).
  • Chlorides (Cl-): Most chlorides are soluble, except for those of silver (Ag+), lead (Pb2+), and mercury (Hg2+).
  • Nitrates (NO3-): Most nitrates are soluble.

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

A: To determine the solubility of a compound, you need to identify the ions present in the compound and apply the solubility rules. If the compound contains ions that are exceptions to the solubility rules, it may be soluble. Otherwise, it is likely to be insoluble.

Q: What are some common mistakes to avoid when determining solubility?

A: Some common mistakes to avoid when determining solubility include:

  • Failing to identify the ions present in the compound
  • Not applying the solubility rules correctly
  • Assuming that a compound is soluble or insoluble based on its appearance or properties
  • Not considering the effects of temperature and pressure on solubility

Q: How does temperature affect solubility?

A: Temperature can affect solubility in several ways. Generally, increasing the temperature of a solution increases the solubility of most substances. However, some substances may have a maximum solubility at a specific temperature, and increasing the temperature beyond this point may actually decrease the solubility.

Q: How does pressure affect solubility?

A: Pressure can also affect solubility, although its effects are generally less pronounced than those of temperature. Increasing the pressure of a solution can increase the solubility of some substances, but it can also decrease the solubility of others.

Q: What are some real-world applications of solubility?

A: Solubility has many real-world applications, including:

  • Pharmaceutical industry: Solubility is critical in the development of new medications, as it affects the bioavailability and efficacy of the drug.
  • Food industry: Solubility is important in the production of food products, such as beverages and desserts, where it affects the texture and consistency of the final product.
  • Environmental science: Solubility is crucial in understanding the behavior of pollutants in the environment, such as the solubility of heavy metals in water.

Conclusion

In conclusion, solubility is a fundamental concept in chemistry that has many practical applications. By understanding the solubility rules and how to apply them, you can predict the behavior of compounds and make informed decisions in laboratory settings and industrial applications. We hope this Q&A article has provided you with a better understanding of solubility and its importance in various fields.

References

  • Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
  • Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science (13th ed.). Pearson Education.
  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2016). General chemistry: Principles and modern applications (11th ed.). Pearson Education.

Note: The references provided are a selection of popular chemistry textbooks that cover the topic of solubility. They are not an exhaustive list, and readers are encouraged to consult additional resources for further information.