To what pH should a solution that is 0.072 M each in Ca²+ and Cd²+ ions be adjusted in order to best separate ions by precipitation of one of the hydroxides? See the Solubility Product Constant Table. What are the concentrations of the metal ions after the pH is adjusted to this value? [Ca2+] 40 M [Cd²+1 40 M
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![**Title:** Determining Optimal pH for Ion Separation by Precipitation
**Content:**
**Objective:**
To determine the appropriate pH for separating metal ions \( \text{Ca}^{2+} \) and \( \text{Cd}^{2+} \) by precipitating one of their hydroxides.
**Problem Statement:**
To what pH should a solution be adjusted if it contains 0.072 M of \( \text{Ca}^{2+} \) and \( \text{Cd}^{2+} \) ions to optimally separate these ions through precipitation of one of the hydroxides? Consult the Solubility Product Constant Table for guidance.
**Data Input Section:**
- **pH Adjustment Input:**
- [Input box labeled "pH"]
**Question:**
What are the concentrations of the metal ions after the pH is adjusted to this value?
**Ion Concentration Output Section:**
- **Concentration of Calcium Ions \([ \text{Ca}^{2+} ]\):**
- [Input box labeled "[Ca2+]"] \( \text{M} \)
- **Concentration of Cadmium Ions \([ \text{Cd}^{2+} ]\):**
- [Input box labeled "[Cd2+]"] \( \text{M} \)
**Instructions:**
Utilize the given input fields to calculate and input the necessary pH and resulting ion concentrations after adjustment. Refer to the solubility product constants for each metal hydroxide to determine the optimal conditions for precipitation and separation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8eeaacd3-f9c7-4223-a8e6-a717e551a98a%2Fac104567-2b91-483f-8d93-8a5dbc919613%2Febcllfa_processed.png&w=3840&q=75)
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