3.9 Solubility ProductAt A Certain Temperature, The Solubility Product Of $CaSO_4$ Is $6.4 \times 10^{-5}$. The Solubility Of The Salt In \$mol \, L^{-1}$[/tex\] Is:A. $8 \times 10^{-10}$ B. $8
Understanding the Solubility Product of Calcium Sulfate
The solubility product, also known as the solubility product constant (Ksp), is a measure of the equilibrium between a solid ionic compound and its ions in a solution. In this article, we will explore the concept of solubility product and its application to the compound calcium sulfate (CaSO4).
What is the Solubility Product?
The solubility product is a numerical value that represents the equilibrium constant for the dissolution of a solid ionic compound in a solution. It is defined as the product of the concentrations of the ions in the solution, raised to the power of their stoichiometric coefficients in the balanced equation for the dissolution reaction.
For the compound CaSO4, the dissolution reaction is:
CaSO4 (s) ⇌ Ca2+ (aq) + SO42- (aq)
The solubility product (Ksp) for CaSO4 is given by the equation:
Ksp = [Ca2+][SO42-]
where [Ca2+] and [SO42-] are the concentrations of calcium and sulfate ions in the solution, respectively.
Given the Solubility Product of CaSO4
At a certain temperature, the solubility product of CaSO4 is given as 6.4 × 10-5. This value represents the equilibrium constant for the dissolution reaction of CaSO4 in a solution.
Calculating the Solubility of CaSO4
To calculate the solubility of CaSO4, we need to determine the concentrations of calcium and sulfate ions in the solution. Since the dissolution reaction produces one mole of calcium ions and one mole of sulfate ions for every mole of CaSO4 that dissolves, the concentrations of these ions are equal.
Let x be the concentration of Ca2+ ions in the solution. Then, the concentration of SO42- ions is also x.
The solubility product (Ksp) is given by the equation:
Ksp = [Ca2+][SO42-] = x × x = x^2
Substituting the given value of Ksp (6.4 × 10-5), we get:
x^2 = 6.4 × 10-5
Taking the square root of both sides, we get:
x = √(6.4 × 10-5) = 2.53 × 10-3
Therefore, the concentration of Ca2+ ions in the solution is 2.53 × 10-3 M.
Conclusion
The solubility of CaSO4 is 2.53 × 10-3 M. This value represents the concentration of Ca2+ ions in the solution, which is equal to the concentration of SO42- ions.
Answer
The correct answer is:
C. 2.53 × 10-3
Discussion
The solubility product of CaSO4 is a measure of the equilibrium between the solid compound and its ions in a solution. By calculating the solubility product, we can determine the concentrations of the ions in the solution and understand the behavior of the compound in different conditions.
In this article, we have seen how to calculate the solubility of CaSO4 using the given solubility product. This calculation involves determining the concentrations of calcium and sulfate ions in the solution and using the solubility product equation to find the concentration of one of the ions.
The solubility product is an important concept in chemistry, and it has many applications in various fields, including environmental science, geology, and materials science. Understanding the solubility product and its application can help us better comprehend the behavior of compounds in different conditions and make informed decisions in various fields.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
- Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science. Pearson Education.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2016). General chemistry: Principles and modern applications. Pearson Education.
Q&A: Solubility Product of Calcium Sulfate
In our previous article, we discussed the concept of solubility product and its application to the compound calcium sulfate (CaSO4). We also calculated the solubility of CaSO4 using the given solubility product. In this article, we will answer some frequently asked questions related to the solubility product of CaSO4.
Q: What is the solubility product of CaSO4?
A: The solubility product of CaSO4 is 6.4 × 10-5.
Q: How is the solubility product calculated?
A: The solubility product is calculated using the equation:
Ksp = [Ca2+][SO42-]
where [Ca2+] and [SO42-] are the concentrations of calcium and sulfate ions in the solution, respectively.
Q: What is the relationship between the solubility product and the solubility of CaSO4?
A: The solubility product is related to the solubility of CaSO4 by the equation:
Ksp = x^2
where x is the concentration of Ca2+ ions in the solution.
Q: How do you determine the concentration of Ca2+ ions in the solution?
A: To determine the concentration of Ca2+ ions in the solution, you need to calculate the square root of the solubility product.
Q: What is the significance of the solubility product in chemistry?
A: The solubility product is an important concept in chemistry as it helps us understand the behavior of compounds in different conditions. It is used to predict the solubility of compounds, which is essential in various fields such as environmental science, geology, and materials science.
Q: Can the solubility product be used to predict the solubility of other compounds?
A: Yes, the solubility product can be used to predict the solubility of other compounds. However, the solubility product is specific to each compound and must be calculated separately for each compound.
Q: How does the temperature affect the solubility product of CaSO4?
A: The temperature affects the solubility product of CaSO4. As the temperature increases, the solubility product of CaSO4 also increases.
Q: Can the solubility product be used to predict the solubility of CaSO4 in different solvents?
A: Yes, the solubility product can be used to predict the solubility of CaSO4 in different solvents. However, the solubility product is specific to each solvent and must be calculated separately for each solvent.
Q: What is the relationship between the solubility product and the pH of the solution?
A: The solubility product is related to the pH of the solution by the equation:
Ksp = [Ca2+][SO42-]
where [Ca2+] and [SO42-] are the concentrations of calcium and sulfate ions in the solution, respectively.
Conclusion
In this article, we have answered some frequently asked questions related to the solubility product of CaSO4. We have discussed the concept of solubility product, its calculation, and its significance in chemistry. We have also answered questions related to the relationship between the solubility product and the solubility of CaSO4, the concentration of Ca2+ ions in the solution, and the effect of temperature and pH on the solubility product.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
- Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science. Pearson Education.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2016). General chemistry: Principles and modern applications. Pearson Education.