1. Aqueous Ion Lab

2. Data

3. For the boxes that made precipitates:  Number half the X’s (one half is the mirror image of the other Set 1 K + CrO 4 2- Na + CrO 4 2- Ba 2+ Cl - Ba 2+ NO 3 - 1 2 3 4

4. Set 1

5. A. Ions Present  For the numbered boxes, write the ions present.  Ex. 1: Ba 2+, Cl -, K +, CrO 4 2- K + CrO 4 2- Na + CrO 4 2- Ba 2+ Cl - Ba 2+ NO 3 - 1 2 34

6. B. Compounds  The solutions preformed double replacement (the anions switched places)  Write the possible compounds formed with each number  Ex. 1: Ba 2+, Cl -, K +, CrO 4 2-  BaCrO 4 and KCl  Only once actual compound precipitated  Discover which compound actually was formed Check your solubility rules on page 920 to find which compounds are soluble and insoluble Check your solubility rules on page 920 to find which compounds are soluble and insoluble If there is an S between the 2 ions, then no compound was formed If there is an S between the 2 ions, then no compound was formed If there is an I between the 2 ions, then that compound is your precipitate. Circle this compound If there is an I between the 2 ions, then that compound is your precipitate. Circle this compound

7. C. Write the equation for the precipitate  For each precipitate, write the equation of formation  Ex. 1: Ba 2+ + Cl - + K + + CrO 4 2-  BaCrO4 (s) + Cl - + K +  Eliminate any ion that does not react (called spectator ions)  Ex. 1: Ba 2+ + CrO 4 2-  BaCrO4 (s)

8. For the boxes that made precipitates:  Number half the X’s (one half is the mirror image of the other Set II Sr +2 NO 3 - Al +3 SO 4 2- Na + SO 4 2- Ba 2+ Cl - Ba 2+ NO 3 - 1 2 3 4 Sr +2 NO 3 - Al +3 SO 4 2- 56

9. Set 2

10. A. Ions Present  For the numbered boxes, write the ions present.  Ex. 1: Sr 2+, NO 3 -, Al +3, SO 4 2- Sr +2 NO 3 - Al +3 SO 4 2- Na + SO 4 2- Ba 2+ Cl - Ba 2+ NO 3 - 1 2 3 4 Sr +2 NO 3 - Al +3 SO 4 2- 56

11. Set 2  For each numbered box you need to complete the following:  A] Ions Present?  B] Possible compounds?  C] Equation?

12. B. Compounds  The solutions performed double replacement (the anions switched places)  Write the possible compounds formed with each number  Ex. 1: Sr 2+, NO 3 -, Al +3, SO 4 2-  SrSO 4 and Al(NO 3 ) 3  Only one actual compound precipitated  Discover which compound actually was formed Check your solubility rules on page 920 to find which compounds are soluble and insoluble Check your solubility rules on page 920 to find which compounds are soluble and insoluble If there is an S between the 2 ions, then no compound was formed If there is an S between the 2 ions, then no compound was formed If there is an I or P between the 2 ions, then that compound is your precipitate. Circle this compound If there is an I or P between the 2 ions, then that compound is your precipitate. Circle this compound

13. Set 2  For each numbered box you need to complete the following:  A] Ions Present?  B] Possible compounds?  C] Equation?

14. C. Equation  For each precipitate, write the equation of formation  Ex. 1: Sr 2+ + NO 3 - + Al +3 + SO 4 2-  SrSO4 (s) + NO 3 - + Al +3  Eliminate any ion that does not react (called spectator ions)  Ex. 1: Sr 2+ + SO 4 2-  SrSO4 (s)

15. Set 2  For each numbered box you need to complete the following:  A] Ions Present?  B] Possible compounds?  C] Equation?