The Solubility Of Cadmium(II) Carbonate Is 2.3 × 10 − 6 M 2.3 \times 10^{-6} M 2.3 × 1 0 − 6 M . What Is The K S P K_{sp} K S P ​ For This Compound?

Introduction

Cadmium(II) carbonate is a compound that is known to be slightly soluble in water. The solubility of a compound is a measure of the amount of the compound that can dissolve in a given amount of solvent, typically water. In this case, we are given the solubility of cadmium(II) carbonate as $2.3 \times 10^{-6} M$. The solubility product constant, or $K_{sp}$, is a measure of the solubility of a compound and is defined as the product of the concentrations of the ions in a saturated solution. In this article, we will discuss the calculation of $K_{sp}$ for cadmium(II) carbonate.

The Solubility of Cadmium(II) Carbonate

Cadmium(II) carbonate is a compound that can be represented by the chemical formula CdCO3. When this compound dissolves in water, it breaks down into its constituent ions, cadmium(II) ions (Cd2+) and carbonate ions (CO32-). The solubility of cadmium(II) carbonate is given as $2.3 \times 10^{-6} M$, which means that for every liter of water, $2.3 \times 10^{-6}$ moles of cadmium(II) carbonate can dissolve.

The Solubility Product Constant ($K_{sp}$)

The solubility product constant, or $K_{sp}$, is a measure of the solubility of a compound and is defined as the product of the concentrations of the ions in a saturated solution. For cadmium(II) carbonate, the $K_{sp}$ expression is given by:

$$K_{sp} = [\text{Cd}^{2+}][\text{CO}_3^{2-}]$$

where $[\text{Cd}^{2+}]$ and $[\text{CO}_3^{2-}]$ are the concentrations of cadmium(II) ions and carbonate ions, respectively.

Calculating $K_{sp}$ for Cadmium(II) Carbonate

To calculate the $K_{sp}$ for cadmium(II) carbonate, we need to know the concentrations of the ions in a saturated solution. Since the solubility of cadmium(II) carbonate is $2.3 \times 10^{-6} M$, we can assume that the concentrations of the ions are equal to the solubility.

Let $x$ be the concentration of cadmium(II) ions and carbonate ions. Then, we can write:

$$K_{sp} = x \cdot x = x^2$$

Since the solubility of cadmium(II) carbonate is $2.3 \times 10^{-6} M$, we can substitute this value for $x$:

$$K_{sp} = (2.3 \times 10^{-6})^2 = 5.29 \times 10^{-12}$$

Therefore, the $K_{sp}$ for cadmium(II) carbonate is $5.29 \times 10^{-12}$.

Conclusion

In this article, we discussed the calculation of the solubility product constant ($K_{sp}$) for cadmium(II) carbonate. We started by defining the solubility of cadmium(II) carbonate and the $K_{sp}$ expression. We then calculated the $K_{sp}$ for cadmium(II) carbonate using the given solubility. The result is a $K_{sp}$ value of $5.29 \times 10^{-12}$, which is a measure of the solubility of cadmium(II) carbonate.

References

• [1] Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
• [2] Brown, T. E., & LeMay, J. T. (2012). Chemistry: The Central Science. Pearson Education.
• [3] Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications. Pearson Education.

Additional Resources

• [1] Khan Academy. (n.d.). Solubility product constant ($K_{sp}$). Retrieved from https://www.khanacademy.org/science/chemistry/solubility-equilibria/v/solubility-product-constant-ksp
• [2] Chemistry LibreTexts. (n.d.). Solubility Product Constant ($K_{sp}$). Retrieved from https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Supplemental_Resources_for_General_Chemistry_(Ball_et_al.)/09%3A_Solubility_Equilibria/9.04%3A_Solubility_Product_Constant_(Ksp)
  

Introduction

In our previous article, we discussed the calculation of the solubility product constant ($K_{sp}$) for cadmium(II) carbonate. We defined the solubility of cadmium(II) carbonate and the $K_{sp}$ expression, and then calculated the $K_{sp}$ value using the given solubility. In this article, we will answer some frequently asked questions (FAQs) related to the solubility of cadmium(II) carbonate and the calculation of $K_{sp}$.

Q: What is the solubility of cadmium(II) carbonate?

A: The solubility of cadmium(II) carbonate is given as $2.3 \times 10^{-6} M$. This means that for every liter of water, $2.3 \times 10^{-6}$ moles of cadmium(II) carbonate can dissolve.

Q: What is the $K_{sp}$ expression for cadmium(II) carbonate?

A: The $K_{sp}$ expression for cadmium(II) carbonate is given by:

$$K_{sp} = [\text{Cd}^{2+}][\text{CO}_3^{2-}]$$

where $[\text{Cd}^{2+}]$ and $[\text{CO}_3^{2-}]$ are the concentrations of cadmium(II) ions and carbonate ions, respectively.

Q: How do I calculate the $K_{sp}$ value for cadmium(II) carbonate?

A: To calculate the $K_{sp}$ value for cadmium(II) carbonate, you need to know the concentrations of the ions in a saturated solution. Since the solubility of cadmium(II) carbonate is $2.3 \times 10^{-6} M$, you can assume that the concentrations of the ions are equal to the solubility. Then, you can use the $K_{sp}$ expression to calculate the $K_{sp}$ value.

Q: What is the $K_{sp}$ value for cadmium(II) carbonate?

A: The $K_{sp}$ value for cadmium(II) carbonate is $5.29 \times 10^{-12}$.

Q: Why is the $K_{sp}$ value for cadmium(II) carbonate so small?

A: The $K_{sp}$ value for cadmium(II) carbonate is small because the solubility of cadmium(II) carbonate is very low. This means that only a small amount of cadmium(II) carbonate can dissolve in water, resulting in a small $K_{sp}$ value.

Q: What is the significance of the $K_{sp}$ value for cadmium(II) carbonate?

A: The $K_{sp}$ value for cadmium(II) carbonate is significant because it provides information about the solubility of the compound. A small $K_{sp}$ value indicates that the compound is very insoluble, while a large $K_{sp}$ value indicates that the compound is very soluble.

Q: How does the $K_{sp}$ value for cadmium(II) carbonate compare to other compounds?

A: The $K_{sp}$ value for cadmium(II) carbonate is relatively small compared to other compounds. For example, the $K_{sp}$ value for calcium carbonate is $4.8 \times 10^{-9}$, which is much larger than the $K_{sp}$ value for cadmium(II) carbonate.

Q: Can I use the $K_{sp}$ value for cadmium(II) carbonate to predict the solubility of other compounds?

A: No, you cannot use the $K_{sp}$ value for cadmium(II) carbonate to predict the solubility of other compounds. The $K_{sp}$ value is specific to each compound and cannot be used to predict the solubility of other compounds.

Conclusion

In this article, we answered some frequently asked questions (FAQs) related to the solubility of cadmium(II) carbonate and the calculation of $K_{sp}$. We discussed the solubility of cadmium(II) carbonate, the $K_{sp}$ expression, and the calculation of the $K_{sp}$ value. We also compared the $K_{sp}$ value for cadmium(II) carbonate to other compounds and discussed the significance of the $K_{sp}$ value.

References

• [1] Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
• [2] Brown, T. E., & LeMay, J. T. (2012). Chemistry: The Central Science. Pearson Education.
• [3] Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications. Pearson Education.

Additional Resources

• [1] Khan Academy. (n.d.). Solubility product constant ($K_{sp}$). Retrieved from https://www.khanacademy.org/science/chemistry/solubility-equilibria/v/solubility-product-constant-ksp
• [2] Chemistry LibreTexts. (n.d.). Solubility Product Constant ($K_{sp}$). Retrieved from https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Supplemental_Resources_for_General_Chemistry_(Ball_et_al.)/09%3A_Solubility_Equilibria/9.04%3A_Solubility_Product_Constant_(Ksp)