Net Ionic Equation Lab Attached following are the lab report form and the solubility table. Complete the document Given the reactants, perform either a dou

Net Ionic Equation Lab Attached following are the lab report form and the solubility table. Complete the document Given the reactants, perform either a double or a single displacement reaction and predict the products. Use your solubility table and knowledge of gas forming reactions to determine the state of predicted products. Determine if there was “ No Reaction” from your NIE rules not from your observations. Show the total net ionic equation for all reactions. If all species on both sides of the equation are spectator ions then write “ No Reaction” for the net ionic equation and the “reaction type”. Fill in the table ( an example is indicated below) for the following reactions
a. A + B
Overall Equation
Reaction type :_______________
Total Ionic Equation
Net Ionic Equation
1. Ca3(PO4)2 (aq) + H2SO4 (aq)
2. Ca3(PO4)2 (s) + HCl (aq)
3. Ni(NO3)2 (aq) + Na3PO4 (aq)
4. Cu (s) + AgNO3 (aq)
5. CaCO3 (s) + HCl ( aq)
6. Zn (s) + HCl (aq)
7. NaHCO3( aq) + HCl (aq)
8. Pb ( NO3)2 (aq) + KI (aq)
9. Pb ( NO3)2 (aq) + K2CrO4 (aq)
10. Ca(NO3)2 (aq) + Na3PO4 (aq)
11. Fe(NO3)3 (aq) + NaOH (aq)
12. KNO3 (aq) + NaOH (aq)
13. Na2CO3 (aq) + HCl (aq)
14. Ni(NO3)2 (aq) + NaOH (aq)
15. Ni(NO3)2 (aq) + Na2SO4 (aq)
16. Ba(NO3)2 (aq) + Na2SO4 (aq)
17. Ni(NO3) (aq) + Na2CO3 (aq)
18. HCl (aq) + NaOH (aq)
19. CaCO3 (s) + HCl (aq)
20. AgNO3(aq) + Fe(NO3)3(aq)
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General Chemistry
Net Ionic Equations Report Form
Name
Lab Partner
You will NOT have a separate write-up for this lab. You will be handing in the following pages with the observations and equations as a lab
report. Given the reactants, perform either a double or single replacement reaction and predict the products. Use your solubility table and
knowledge of gas forming reactions to determine the states of the predicted products. Determine if there was “No Reaction” from your NIE
rules not from your observations. Show the total ionic equation for all reactions. If all species, on both sides of the equation are spectator ions
then write “No Reaction” for the net ionic equation and the “reaction type.” Write the equations for those that you predicted reacted even if
you didn’t observe it. For each mixture that does react in some way, write the reaction type, overall equation, total ionic equation and the net
ionic equation. All need to be balanced with the states for each compound, ion, and/or element in the reaction indicated.
1. Ca3(PO4)2(s) + H2SO4(aq)
Reaction Type
Observations
Overall Equation
Total lonic Equation
Net lonic Equation
811
General Chemistry !
Reaction Type
2 Cas(Po) + HC gì.
Observations
Overall Equation
Total lonic Equation
Net lonic Equation
Reaction Type
3. Ni(NO3)2(aq) + Na3PO4(aa)
Observations
Overall Equation
Total lonic Equation
82|Pa
Net lonic Equation
General Chemistry !
4. Cu(s) + AgNO3(aq) (Form copper (II) nitrate)
Reaction Type
Observations
Overall Equation
Total lonic Equation
Net lonic Lyvetion
5. CaCO3(s) + HCl(aq)
Reaction Type
Observations
Overall Equation
Total lonic Equation
Net lonic Equation
83 | Page
Table F
Solubility Guidelines for Aqueous Solutions
Exceptions
Ions That Form
Soluble Compounds
Group 1 ions
(Lit, Nat, etc.)
ammonium (NH4+)
nitrate (NO3)
acetate C,H,O, or
CH2C00)
hydrogen carbonate
(HCO3)
chlorate ClO3)
perchlorate (C10,-)
halides (CH, Br, 1-)
Ions That Form
Insoluble Compounds Exceptions
carbonate (CO2) when combined with Group 1
ions or ammonium (NH4+)
chromate (CrO2-) when combined with Group 1
ions, Ca2+, Mg²+, or
ammonium (NH4+)
phosphate (PO3-) when combined with Group 1
ions or ammonium (NH +)
sulfide (S2-)
when combined with Group 1
ions or ammonium (NH)
hydroxide (OH-) when combined with Group 1
ions, Ca2+ Ba2+, SpP+ or
ammonium (NH4)
2-
when combined with
Agt, Pb2+, and Hg2
when combined with Ag+,
Ca2+, Sr2+, Ba2+, and Pb2+
sulfates (SO2)

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