Which Salts Will Be More Soluble In An Acidic Solution Than In Pure Water?A. CuI B. A G 2 S O 4 Ag_2SO_4 A G 2 ​ S O 4 ​ C. K C L O 4 KClO_4 K Cl O 4 ​ D. C A C O 3 CaCO_3 C A C O 3 ​ E. Z N ( O H ) 2 Zn(OH)_2 Z N ( O H ) 2 ​

Which Salts Will Be More Soluble in an Acidic Solution Than in Pure Water?

Introduction

When it comes to the solubility of salts in different solutions, there are several factors to consider. The solubility of a salt in a solution can be influenced by the pH of the solution, the type of salt, and the presence of other ions. In this article, we will explore which salts are more soluble in an acidic solution than in pure water.

Understanding Solubility

Solubility is a measure of the amount of a substance that can dissolve in a given amount of solvent. In the case of salts, solubility is often influenced by the pH of the solution. Acids and bases can affect the solubility of salts by altering the concentration of hydrogen ions (H+) or hydroxide ions (OH-).

The Effect of pH on Solubility

The pH of a solution can have a significant impact on the solubility of salts. In general, salts that are more soluble in acidic solutions tend to be those that have a high concentration of hydrogen ions (H+). This is because the hydrogen ions can react with the anion of the salt to form a more soluble compound.

Option A: CuI

Copper(I) iodide (CuI) is a salt that is composed of copper ions (Cu+) and iodide ions (I-). In pure water, CuI is relatively insoluble. However, in an acidic solution, the solubility of CuI can increase due to the presence of hydrogen ions (H+). The reaction between CuI and H+ can form a more soluble compound, such as copper(II) iodide (CuI2).

Option B: $Ag_2SO_4$

Silver sulfate ($Ag_2SO_4$) is a salt that is composed of silver ions (Ag+) and sulfate ions (SO42-). In pure water, $Ag_2SO_4$ is relatively insoluble. However, in an acidic solution, the solubility of $Ag_2SO_4$ can increase due to the presence of hydrogen ions (H+). The reaction between $Ag_2SO_4$ and H+ can form a more soluble compound, such as silver hydrogen sulfate (AgHSO4).

Option C: $KClO_4$

Potassium perchlorate ($KClO_4$) is a salt that is composed of potassium ions (K+) and perchlorate ions (ClO4-). In pure water, $KClO_4$ is relatively soluble. However, in an acidic solution, the solubility of $KClO_4$ can decrease due to the presence of hydrogen ions (H+). The reaction between $KClO_4$ and H+ can form a less soluble compound, such as potassium hydrogen perchlorate (KHCIO4).

Option D: $CaCO_3$

Calcium carbonate ($CaCO_3$) is a salt that is composed of calcium ions (Ca2+) and carbonate ions (CO32-). In pure water, $CaCO_3$ is relatively insoluble. However, in an acidic solution, the solubility of $CaCO_3$ can increase due to the presence of hydrogen ions (H+). The reaction between $CaCO_3$ and H+ can form a more soluble compound, such as calcium hydrogen carbonate (CaHCO3).

Option E: $Zn(OH)_2$

Zinc hydroxide ($Zn(OH)_2$) is a salt that is composed of zinc ions (Zn2+) and hydroxide ions (OH-). In pure water, $Zn(OH)_2$ is relatively insoluble. However, in an acidic solution, the solubility of $Zn(OH)_2$ can decrease due to the presence of hydrogen ions (H+). The reaction between $Zn(OH)_2$ and H+ can form a less soluble compound, such as zinc chloride (ZnCl2).

Conclusion

In conclusion, the solubility of salts in acidic solutions can be influenced by the pH of the solution, the type of salt, and the presence of other ions. Based on the analysis of the options provided, the salts that are more soluble in an acidic solution than in pure water are:

• CuI
• $Ag_2SO_4$
• $CaCO_3$

These salts tend to have a high concentration of hydrogen ions (H+) in acidic solutions, which can react with the anion of the salt to form a more soluble compound. On the other hand, the salts that are less soluble in acidic solutions are:

• $KClO_4$
• $Zn(OH)_2$

These salts tend to have a lower concentration of hydrogen ions (H+) in acidic solutions, which can react with the anion of the salt to form a less soluble compound.

References

• Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
• Brown, T. L., LeMay, J. T., Bursten, B. E., & Murphy, C. J. (2012). Chemistry: The Central Science (12th ed.). Pearson Education.
• Cengel, Y. A., & Boles, M. A. (2015). Thermodynamics: An interactive introduction. McGraw-Hill Education.

Note: The references provided are a selection of general chemistry textbooks that may be useful for further reading on the topic of solubility and pH.
Q&A: Solubility and pH

Introduction

In our previous article, we explored which salts are more soluble in an acidic solution than in pure water. In this article, we will answer some frequently asked questions about solubility and pH.

Q: What is the relationship between pH and solubility?

A: The pH of a solution can have a significant impact on the solubility of salts. In general, salts that are more soluble in acidic solutions tend to be those that have a high concentration of hydrogen ions (H+). This is because the hydrogen ions can react with the anion of the salt to form a more soluble compound.

Q: How does the pH of a solution affect the solubility of a salt?

A: The pH of a solution can affect the solubility of a salt in several ways. In acidic solutions, the presence of hydrogen ions (H+) can increase the solubility of some salts. In basic solutions, the presence of hydroxide ions (OH-) can decrease the solubility of some salts.

Q: What is the effect of pH on the solubility of CuI?

A: CuI is a salt that is composed of copper ions (Cu+) and iodide ions (I-). In pure water, CuI is relatively insoluble. However, in an acidic solution, the solubility of CuI can increase due to the presence of hydrogen ions (H+). The reaction between CuI and H+ can form a more soluble compound, such as copper(II) iodide (CuI2).

Q: What is the effect of pH on the solubility of $Ag_2SO_4$?

A: $Ag_2SO_4$ is a salt that is composed of silver ions (Ag+) and sulfate ions (SO42-). In pure water, $Ag_2SO_4$ is relatively insoluble. However, in an acidic solution, the solubility of $Ag_2SO_4$ can increase due to the presence of hydrogen ions (H+). The reaction between $Ag_2SO_4$ and H+ can form a more soluble compound, such as silver hydrogen sulfate (AgHSO4).

Q: What is the effect of pH on the solubility of $KClO_4$?

A: $KClO_4$ is a salt that is composed of potassium ions (K+) and perchlorate ions (ClO4-). In pure water, $KClO_4$ is relatively soluble. However, in an acidic solution, the solubility of $KClO_4$ can decrease due to the presence of hydrogen ions (H+). The reaction between $KClO_4$ and H+ can form a less soluble compound, such as potassium hydrogen perchlorate (KHCIO4).

Q: What is the effect of pH on the solubility of $CaCO_3$?

A: $CaCO_3$ is a salt that is composed of calcium ions (Ca2+) and carbonate ions (CO32-). In pure water, $CaCO_3$ is relatively insoluble. However, in an acidic solution, the solubility of $CaCO_3$ can increase due to the presence of hydrogen ions (H+). The reaction between $CaCO_3$ and H+ can form a more soluble compound, such as calcium hydrogen carbonate (CaHCO3).

Q: What is the effect of pH on the solubility of $Zn(OH)_2$?

A: $Zn(OH)_2$ is a salt that is composed of zinc ions (Zn2+) and hydroxide ions (OH-). In pure water, $Zn(OH)_2$ is relatively insoluble. However, in an acidic solution, the solubility of $Zn(OH)_2$ can decrease due to the presence of hydrogen ions (H+). The reaction between $Zn(OH)_2$ and H+ can form a less soluble compound, such as zinc chloride (ZnCl2).

Q: How can I determine the solubility of a salt in a solution?

A: To determine the solubility of a salt in a solution, you can use a variety of methods, including:

• Measuring the concentration of the salt in the solution using techniques such as titration or spectroscopy.
• Observing the physical properties of the solution, such as its clarity or color.
• Conducting experiments to determine the solubility of the salt in different solutions.

Q: What are some common applications of solubility and pH?

A: Solubility and pH have a wide range of applications in various fields, including:

• Water treatment: Solubility and pH are important factors in the treatment of water for drinking, industrial, and agricultural purposes.
• Pharmaceutical industry: Solubility and pH are critical factors in the development of new medications and the formulation of existing ones.
• Food industry: Solubility and pH are important factors in the processing and preservation of food products.

Conclusion

In conclusion, the relationship between pH and solubility is complex and can be influenced by a variety of factors. By understanding the effects of pH on the solubility of different salts, you can better design and optimize solutions for a wide range of applications.

References

• Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
• Brown, T. L., LeMay, J. T., Bursten, B. E., & Murphy, C. J. (2012). Chemistry: The Central Science (12th ed.). Pearson Education.
• Cengel, Y. A., & Boles, M. A. (2015). Thermodynamics: An interactive introduction. McGraw-Hill Education.

Note: The references provided are a selection of general chemistry textbooks that may be useful for further reading on the topic of solubility and pH.