At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The resulting equilibrium solution has a pH of 10.36. What is the Kp of the salt at 22 °C? Ksp =
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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![**Problem Statement:**
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)₂, is mixed with pure water. The resulting equilibrium solution has a pH of 10.36. What is the \(K_{sp}\) of the salt at 22 °C?
\[ K_{sp} = \underline{\hspace{10cm}} \]
**Explanation:**
Given:
- Temperature: 22 °C
- Chemical compound: M(OH)₂
- pH of the solution: 10.36
To determine:
- Solubility product constant, \(K_{sp}\), of the salt at 22 °C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd6e2cac-a13e-4af0-8d42-5fb7a66b94d3%2F029f862c-f563-4337-989a-9de9efa9c5e8%2Fp7pl0g_processed.png&w=3840&q=75)
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