Write a balanced net ionic reaction for the reduction of cupric ion (Cu2+) by hydroxylamine (NH2OH) in acid solution, using the smallest integer coefficients.
Im not too sure of what is reacting here to reduce the Cu2+. Help?
To determine the balanced net ionic reaction for the reduction of cupric ion (Cu2+) by hydroxylamine (NH2OH) in acid solution, we need to identify the reactants and products involved in the reaction.
First, let's identify the reactants:
1. Cupric ion (Cu2+) is the oxidizing agent, meaning it will undergo reduction.
2. Hydroxylamine (NH2OH) is the reducing agent, meaning it will undergo oxidation.
By combining these reactants, the following reaction occurs:
Cu2+(aq) + NH2OH(aq) → Cu+ (aq) + N2(g) + H2O(l)
In this reaction, cupric ion (Cu2+) is reduced to cuprous ion (Cu+), and hydroxylamine (NH2OH) is oxidized to nitrogen gas (N2) and water (H2O).
To balance this net ionic reaction, we need to make sure the number of each type of atom is the same on both sides of the equation. Here is the balanced net ionic reaction using the smallest integer coefficients:
2Cu2+(aq) + 5NH2OH(aq) + 4H+(aq) → 2Cu+ (aq) + N2(g) + 7H2O(l)
In this balanced net ionic reaction, two Cu2+ ions react with five NH2OH molecules and four H+ ions to form two Cu+ ions, one N2 molecule, and seven H2O molecules.