• 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 silver nitrate solution is poured into the
ammonium bromide solution. What (if any) precipitate forms?
• Step 2: Sodium sulfate solution is poured into the aqueous
part of the Step 1 mixture. What (if any) precipitate forms?
• Step 3: Barium chloride solution is poured into the aqueous
part of the Step 2 mixture. What (if any) precipitate forms?
• Step 4: Identify all the ions that remain dissolved in the
solution when all the precipitation reactions are finish
This is from a hw problem I have any help would be appreciated
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- ChenBeier
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This really is made on paper not as a experiment.
1. Silverbromide will precipitate.
2. It also precipitate, can be Calcium, Strontium or Barium as sulfate.
3. Now the Joke comes. Sulfate was poured in step 2 first, if you put Bariumchloride in of coures Bariumsulfate will precipitate again.
4. Count by yourself what is left.
1. Silverbromide will precipitate.
2. It also precipitate, can be Calcium, Strontium or Barium as sulfate.
3. Now the Joke comes. Sulfate was poured in step 2 first, if you put Bariumchloride in of coures Bariumsulfate will precipitate again.
4. Count by yourself what is left.