In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation?
Question 8 answers
In the equation Mn goes from +7 to +2 and As goes from +3 to +5. That should give you the information to balance. Here is a site that may help but please re-post if you have a more detailed question about the procedure.
http://www.chemteam.info/Redox/Redox.html
To write the balanced net ionic equation for this reaction, we need to first write the balanced chemical equation.
The unbalanced equation is:
MnO4- + H3AsO3 -> H3AsO4 + Mn2+
To balance the equation, we start by balancing the atoms in the equation. We have 1 manganese (Mn) atom, 4 oxygen (O) atoms, and 3 arsenic (As) atoms on each side.
MnO4- + 2H3AsO3 -> 2H3AsO4 + Mn2+
Next, we balance the charges. On the left side, the MnO4- ion has a charge of -1, while the H3AsO3 molecule is neutral. On the right side, the H3AsO4 molecule is neutral, and the Mn2+ ion has a charge of +2.
2MnO4- + 3H3AsO3 -> 3H3AsO4 + 2Mn2+
Now that we have the balanced chemical equation, we can write the balanced net ionic equation by removing spectator ions, which do not participate in the reaction.
The spectator ions in this reaction are K+ and OH-, which do not change their oxidation state or form new products. They are found on both the reactant and product sides of the equation and do not participate in the redox reaction.
Thus, the net ionic equation is:
2MnO4- + 3H3AsO3 -> 3H3AsO4 + 2Mn2+
In this equation, there are a total of 3 H+ on both the reactant side (3H3AsO3) and the product side (3H3AsO4).
To write the balanced net ionic equation, we first need to write the balanced chemical equation for the reaction:
MnO4- + H3AsO3 + H+ → H3AsO4 + Mn2+ + H2O
Here, MnO4- is the oxidizing agent, and H3AsO3 is the reducing agent. When MnO4- reacts, it gains electrons and is reduced to Mn2+.
To write the net ionic equation, we need to cancel out any ions that appear on both sides of the equation. In this case, the H+ ions appear on both sides:
MnO4- + H3AsO3 + H+ → H3AsO4 + Mn2+ + H2O
The net ionic equation is:
MnO4- + H3AsO3 → H3AsO4 + Mn2+
Next, we need to determine the number of H+ ions in the balanced equation. From the net ionic equation, we can see that there are three H+ ions on the left side (from the H3AsO3 molecule) and four H+ ions on the right side (from the H3AsO4 molecule):
Net Ionic Equation: MnO4- + H3AsO3 → H3AsO4 + Mn2+
Number of H+ ions: 3 H+ (left side) → 4 H+ (right side)
Therefore, there are four H+ ions in the balanced equation.