Chem 214 Spring 2020 Net Ionic Equation Drill  Instructions: 1

Chem 214 Spring 2020 Net Ionic Equation Drill 
Instructions: 1. Refer to the Net Ionic Equation Review posted under Qualitative Analysis. 2. Refer to the Solubility Rules to predict which product may form the precipitate or whicl product may form a gas (form bubbles) 3. Write the balanced a) Molecular equation b) Ionic equation c) Net ionic equation 4. Indicate the states (s for solid, precipitate forms; I for liquid; aq for aqueous solution; g for gas) 5. Some precipitates may dissolve in excess reagent to form the complex ion.SO4 6. Write NR if there is no reaction 
This Drill is worth 10 bonus points. Make sure to write proper subscript and superscript. 1. AlC13(aq) + AgNO3 (aq) 2. K2CO3(aq) + H2SO4 (aq) 3. MgCl2(aq) + NaOH (aq) 4. CuSO4(aq) + excess NH3(aq) 5. Ba(NO3)2(aq) + ZnSO4(aq) 6. Mg(OH)2(aq) + NaOH(aq) 7. AlC13(aq) + excess NaOH(aq) 8. ZnSO4(aq) + NH3(aq) 9. Ba(NO3)2(aq) + AlC13(aq) 10. MgSO4(aq) + Li2CO3(aq) 
 

Chem 214 Net Ionic Equations - REVIEW Net Ionic Equations For double displacement reactions of the type A-B + CD 4 AD + CB where A and C are cations ; B and D are anions a precipitate may be predicted by referring to the solubility rules (table 4.2, page 122, Chang and Goldsby, 12 ed). Note that reaction with acids may produce a gaseous product (p. 132) Example 1 Molecular Equation: NaC1 (aq) + AgNO3 (aq) - ? products A-B + CD 1 -1 I -1 NaC1 (aq) + AgNO3(aq) - Na NO3 + Ag Cl From Table 4.2, NaC1, NaNO3 and AgNO3 are soluble; AgC1 is insoluble. Ionic Equation - break up the soluble species into corresponding ions Na+ (aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) 4 Na+(aq) + NO3 -(aq) + AgC Cross out species that appear both on the reactant side and product sid (aq) + Cl- (aq) + Ag+ (aq) + NO3--(aq) Nal-(a4) + NO3'(aq) + Ag 
What is left is the net ionic equation! nie Equation : C1-(aq) + Ag+(aq) - AgC1N or Ag+(aq) + Cl-(aq) 4 AgCl(s)