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Solubility rules, a qualitative approach. A chemist prepares four beakers, each with exactly 1.0 M of a particular salt dissolved in water. In the reactions, assume complete formation of any solid products (ignore equilibrium). Step 1: The sodium sulfide solution is poured into the copper(II) sulfate solution. What (if any) precipitate forms? Step 2: Barium chloride solution is poured into the Step 1 mixture. What (if any) precipitate forms? Step 3: Lead(II) nitrate solution is poured into the Step 2 mixture. What (if any) precipitate forms? What are all the remaining ions in solution?
Solubility rules, a qualitative approach. A chemist prepares four beakers, each with exactly 1.0 M of a particular salt dissolved in water. In the reactions, assume complete formation of any solid products (ignore equilibrium). Step 1: The sodium sulfide solution is poured into the copper(II) sulfate solution. What (if any) precipitate forms? Step 2: Barium chloride solution is poured into the Step 1 mixture. What (if any) precipitate forms? Step 3: Lead(II) nitrate solution is poured into the Step 2 mixture. What (if any) precipitate forms? What are all the remaining ions in solution?
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Jamar FerryLv2
14 Mar 2019
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