Which of the following will increase the molar solubiity of Ag2CO3? (The Ksp for Ag2CO3 is 8.1 x 10^12.)
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To determine which of the following will increase the molar solubility of Ag2CO3, we need to consider the factors that affect solubility.
The solubility of a compound is influenced by its equilibrium constant, known as the solubility product constant (Ksp). Ksp indicates the extent to which the compound dissociates in a solution.
In this case, the given Ksp value for Ag2CO3 is 8.1 x 10^12.
To increase the molar solubility of Ag2CO3, we need to consider the common-ion effect and the effect of pH.
1. Common-ion effect: The common-ion effect occurs when a compound shares a common ion with another compound in the solution. Adding a common ion to the solution can reduce the solubility of a compound due to the Le Chatelier's principle.
Therefore, to increase the molar solubility of Ag2CO3, we should avoid adding any compound that has a common ion with Ag2CO3, which in this case is Ag+.
2. pH effect: The solubility of many ionic compounds is influenced by the pH of the solution. Carbonate compounds, including Ag2CO3, are sensitive to changes in pH.
Decreasing the pH of the solution can increase the solubility of carbonate compounds. This is because the presence of excess H+ ions can react with CO3^2- ions to form HCO3- ions, which are more soluble. It shifts the equilibrium towards the dissolved form of Ag2CO3.
Considering these factors, the following option is likely to increase the molar solubility of Ag2CO3:
- Decreasing the pH of the solution by adding an acid (e.g., HCl or H2SO4).
It is important to note that the solubility of Ag2CO3 is already extremely high (Ksp = 8.1 x 10^12). So, even without any additional factors, it naturally has a high molar solubility.