Silver carbonate has a K-5.65x10-12 and a solubility of 0.0001122 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×10 M? [AgNO,]= M
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![**Solubility Problem: Silver Carbonate in Silver Nitrate Solution**
Silver carbonate has a solubility product constant \( K_{sp} = 5.65 \times 10^{-12} \) and a solubility of 0.0001122 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to \( 1 \times 10^{-9} \) M?
\[
[\text{AgNO}_3] = \_\_\_\_\_ \text{ M}
\]
**Explanation and Analysis:**
This exercise is designed to help understand the concept of solubility equilibrium and the common ion effect. Silver carbonate dissociates into silver ions and carbonate ions in solution. By adding silver nitrate, which provides additional silver ions, the solubility of silver carbonate will decrease due to the common ion effect. Calculating the necessary concentration of silver nitrate involves applying the solubility product constant and solving for the concentration under the given conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89b126cf-58b3-49ad-9704-387f30e63dfe%2Fea467f5a-1741-433d-a98c-2d06b554ec55%2F4czzbbg_processed.jpeg&w=3840&q=75)
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