Redox Equations: Writing Net Ionic Reactions Name: __________

The following Unbalanced Acid Media REDOX equations need to be re-written ionically Unbalanced. Rewrite the following Unbalanced chemical equations ionically in total ionic form (without balancing), then cancel spectators for the net ionic equation. Do not forget to place charges on the ions and no charge on the molecules/formula units. This is Step#1 in REDOX balancing so the equations can not be balanced first as shown in the book (and as on the test item M-8G.)

      Rewrite as ions electrolytes such as

(a)     Soluble salts,

(b)   Strong acids, Some strong acids are hydrochloric acid, nitric acid, sulfuric acid, perchloric acid, hydrobromic acid and hydroiodic acid.

(c)    Strong bases.  Strong bases include KOH and NaOH and any soluble hydroxide. Soluble salts are those ionic hydroxide compounds with (aq) (water solution: therefore soluble).

Reference: Corwin: Section 14.11
                           McMurry: Section 4.3

Write net unbalanced ionic reactions for all 20 of the following as a post lab report due the day of REDOX lab:

1.   Zn (s)   +     HNO3 (aq)   à   Zn(NO3)2 (aq)  +   NH4NO3 (aq)    +    H2O (l)

 

 

 

2.  KMnO4(aq) + K2C2O4(aq) + HCl(aq) à MnCl2(aq) + CO2(g) + KCl(aq) +  H2O(l)

 

 

 

3.   K2Cr2O7 (aq)   +   HCl (aq)     à   CrCl3 (aq)  +  Cl2 (g) +  KCl (aq) +    H2O (l)

 

 

 

4.   Cu (s)  +   HNO3 (aq)   à   Cu(NO3)2 (aq)  +   NO2 (g)    +    H2O (l)

 

Page 2 Net Ionic Reactions

5.   Cu (s)  +   HNO3 (aq)   à   Cu(NO3)2 (aq)  +   NO2 (g)    +    H2O (l)

 

 

 

 

6.   KI (aq) +  HNO3 (aq)    à   NO (g)   +   I2 (s)    +  KNO3 (aq) +  H2O (l)   

 

 

 

7.  K2Cr2O7(aq) + C2H5OH(aq) + HCl(aq) à CrCl3(aq) + HC2H3O2(aq)+ KCl(aq) + H2O(l)

 

 

 

 

8.  CH2O (l)     +   H2SO4 (aq)     à    H2S (g)    +   CO2 (g)   +  H2O (l)

 

 

 

 

9.  Zn (s)     +    HNO3(aq)    à      N2 (g)    +     Zn(NO3)2 (aq)     +      H2O

 

 

 

 

Page 3 Net Ionic Reactions

10.   Zn (s)     +    HNO3(aq)    à      N2O (g)    +     Zn(NO3)2 (aq)     +      H2O (l)

 

 

 

 

11.   PbO2 (s)   +      MnO (s)        +      HNO3(aq)    à       HMnO4(aq)     +    Pb(NO3)2 (aq) +       H2O (l)        

 

 

 

 

12.   MnSO4(aq)  +  K2S2O8(aq)  +   H2Oà  H2SO4(aq) +    MnO2(s) +   K2SO4(aq)         

 

 

 

 

 

13.   CdS (aq)  +  I2 (aq) +     H2SO4 (aq) à     CdSO4 (aq) +   HI (aq)  +    S (s)

 

 

 

 

14.   KI (aq)  +   H2SO4 (aq) à   K2SO4 (aq) +  H2S  (aq)  +    I2 (aq)  +   H2O (l) 

 

 

 

Page 3 Net Ionic Reactions

15.   K2MnO4 (aq) +   H2SO4 (aq) à KMnO4 (aq)  +  MnO2  + K2SO4 (aq) +   H2O

 

 

 

 

16.   H2O2   +   KMnO4(aq)   +     HCl (aq)   à   MnCl2(aq)   +   KCl(aq) +  O2   +    H2O

 

 

 

17.  FeS +  KNO3(aq) + H2SO4(aq) à  NO +  Fe(NO3)2(aq) +  K2SO4(aq)+ KNO3(aq)  +  H2O

 

 

 

 

18.    As2S5 +  KNO3(aq)  +  HNO3(aq) à   NO2  +  H3AsO4(aq) +  KHSO4(aq)  +   H2O

 

 

 

19.  KMnO4   +     H2S   +         HCl     à     MnCl2    +     S   +   KCl   +    H2O

 

 

 

 

20.    KMnO4   +      KNO2   +        HNO3  à        MnO2       +     KNO3     +      H2O