Place 25 mL of 0.1 M cobalt (II) chloride solution in a 125 mL erlenmeyer flask.
ID: 1070263 • Letter: P
Question
Place 25 mL of 0.1 M cobalt (II) chloride solution in a 125 mL erlenmeyer flask. Place 25 mL of concentrated HCl in a graduated cylinder. Slowly and carefully add hydrochloric acid to the cobalt (II) chloride solution until the solution turns purple. Put about 15 mL of the purple solution into a 50 mL beaker. Place about 5 mL of silver nitrate solution into a clean test tube or small beaker. Add the silver nitrate solution dropwise to the cobalt solution. Continue adding silver nitrate until a change is seen.
Silver nitrate is a soluble salt and will dissolve into ions. When silver nitrate was added to the equilibrium mixture, silver ion reacted with chloride ion in a precipitation reaction.
1. What ions were present in solution in the equilibrium mixture following the silver nitrate addition? ( Complex ions take the general form: [Ag(NH3)2]+. Include states-of-matter under the given conditions in your answer.)
Explanation / Answer
Initially cobalt chloride treated with HCL it form (CoCl6) complex and follow Ag(CoCl6)Cl2