Write balanced net-ionic equations to describe:
a. The oxidation of Mn2+ to MnO4- by ammonium peroxydisulfate [(NH4)2S2O8]
b. The air-oxidation of HAsO32- to HAsO42-
c. The oxidation of Ce3+ to Ce4+ by sodium bismuthate (NaBiO3)
Write balanced net-ionic equations to describe:
a. The titration of H2O2 with KMnO4
b. The reduction of Fe3+ to Fe2+ by SO2
c. The oxidation of HNO2 by a solution of MnO4-
http://www.chemteam.info/Redox/Redox.html
a. The oxidation of Mn2+ to MnO4- by ammonium peroxydisulfate [(NH4)2S2O8]
Step 1: Write the balanced chemical equation for the reaction.
2 Mn2+ + (NH4)2S2O8 -> MnO4- + (NH4)2SO4
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
2 Mn2+ + S2O82- -> MnO4- + 2 SO42-
b. The air-oxidation of HAsO32- to HAsO42-
Step 1: Write the balanced chemical equation for the reaction.
2 HAsO32- + O2 -> 2 HAsO42-
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
2 HAsO32- + O2 -> 2 HAsO42-
c. The oxidation of Ce3+ to Ce4+ by sodium bismuthate (NaBiO3)
Step 1: Write the balanced chemical equation for the reaction.
2 Ce3+ + NaBiO3 + 6 H+ -> 2 Ce4+ + Na+ + Bi3+ + 3 H2O
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
2 Ce3+ + NaBiO3 + 6 H+ -> 2 Ce4+ + Na+ + Bi3+ + 3 H2O
a. The titration of H2O2 with KMnO4
Step 1: Write the balanced chemical equation for the reaction.
5 H2O2 + 2 KMnO4 + 3 H2SO4 -> 5 O2 + 2 MnSO4 + K2SO4 + 8 H2O
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
5 H2O2 + 2 MnO4- + 6 H+ -> 5 O2 + 4 H2O + 2 Mn2+
b. The reduction of Fe3+ to Fe2+ by SO2
Step 1: Write the balanced chemical equation for the reaction.
Fe3+ + SO2 + H2O -> Fe2+ + SO42- + 2 H+
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
Fe3+ + SO2 + H2O -> Fe2+ + SO42- + 2 H+
c. The oxidation of HNO2 by a solution of MnO4-
Step 1: Write the balanced chemical equation for the reaction.
2 MnO4- + 3 HNO2 + 2 H+ -> 2 MnO2 + 3 NO3- + 2 H2O
Step 2: Write the balanced net ionic equation by separating the soluble ionic compounds into their respective ions and eliminating the spectator ions.
2 MnO4- + 3 HNO2 + 6 H+ -> 2 MnO2 + 3 NO3- + 4 H2O
a. In order to write the balanced net ionic equation for the oxidation of Mn2+ to MnO4- by ammonium peroxydisulfate [(NH4)2S2O8], we need to know the chemical equations and the oxidation states of each element involved. Let's start by writing the balanced chemical equation for the reaction:
(Mn2+) + [(NH4)2S2O8] → MnO4- + (NH4)2SO4
Next, we need to determine the oxidation states of Mn in both the reactants and the products. In the reactant, Mn2+ has an oxidation state of +2, and in the product, MnO4- has an oxidation state of +7.
Now, we can write the balanced net ionic equation by canceling out spectator ions. In this case, the ammonium ion (NH4+) is a spectator ion, which means it appears on both sides of the reaction and does not participate in the oxidation-reduction process. Therefore, the net ionic equation is:
(Mn2+) + [(NH4)2S2O8] → MnO4-
b. To write the balanced net ionic equation for the air-oxidation of HAsO32- to HAsO42-, we need to know the chemical equation and the oxidation states of each element involved. The balanced chemical equation for the reaction is:
HAsO32- + O2 → HAsO42-
In the reactant, HAsO32- has an oxidation state of +3, and in the product, HAsO42- has an oxidation state of +5.
Now, we can write the balanced net ionic equation by canceling out spectator ions. In this case, there are no spectator ions, as all the ions involved participate in the oxidation-reduction process. Therefore, the net ionic equation is the same as the balanced chemical equation:
HAsO32- + O2 → HAsO42-
c. To write the balanced net ionic equation for the oxidation of Ce3+ to Ce4+ by sodium bismuthate (NaBiO3), we need to know the chemical equation and the oxidation states of each element involved. The balanced chemical equation for the reaction is:
Ce3+ + NaBiO3 → Ce4+ + NaBiO4
In the reactant, Ce3+ has an oxidation state of +3, and in the product, Ce4+ has an oxidation state of +4.
Now, we can write the balanced net ionic equation by canceling out spectator ions. In this case, the sodium ion (Na+) and the bismuthate ion (BiO3-) are spectator ions, as they appear on both sides of the reaction and do not participate in the oxidation-reduction process. Therefore, the net ionic equation is:
Ce3+ → Ce4+