When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown?
ClO3- + HAsO2 Cl- + H3AsO4
Water appears in the balanced equation as a _______(reactant, product, neither) with a coefficient of____ . (Enter 0 for neither.)
Which element is oxidized? ______
Cl changes from +5 to -1. As changes from +3 to +5.
http://www.chemteam.info/Redox/Redox.html
To balance the given chemical equation:
1) Start by balancing the atoms that appear in the equation apart from oxygen and hydrogen. In this case, it would be chlorine (Cl) and arsenic (As).
ClO3- + HAsO2 Cl- + H3AsO4
ClO3- -> Cl- requires a coefficient of 1
HAsO2 -> H3AsO4 requires a coefficient of 3
2) Next, balance the oxygen by adding water molecules (H2O) to the side that needs extra oxygen. In this case, it is the right side.
ClO3- + HAsO2 Cl- + H3AsO4 + H2O
ClO3- has 3 oxygen atoms, and HAsO2 has 2 oxygen atoms, so we need to add one water molecule (H2O) on the right side to balance the oxygen.
3) Now, balance the hydrogen by adding hydrogen ions (H+) to the side that needs extra hydrogen. In this case, it is the left side.
ClO3- + H+ + HAsO2 Cl- + H3AsO4 + H2O
HAsO2 has 2 hydrogen atoms, so we need to add two hydrogen ions (H+) on the left side to balance the hydrogen.
The balanced equation under acidic conditions is:
ClO3- + H+ + 2HAsO2 Cl- + H3AsO4 + H2O
Now we can answer the questions:
Water appears in the balanced equation as a product with a coefficient of 1.
Therefore, the answer is:
Water appears in the balanced equation as a product with a coefficient of 1.
To determine which element is oxidized, we need to compare the oxidation states of the elements in the reactants and products.
In this case, chlorine (Cl) is being reduced because it goes from an oxidation state of +5 in ClO3- to -1 in Cl-.
Therefore, the element that is oxidized is arsenic (As).
So, the answer is:
Which element is oxidized? Arsenic (As).
To balance the given equation under acidic conditions, follow these steps:
1. Start by balancing the atoms other than hydrogen and oxygen. In this case, we have:
ClO3- + HAsO2 → Cl- + H3AsO4
The chlorine (Cl) and arsenic (As) atoms are already balanced.
2. Balance the oxygen atoms by adding water (H2O) molecules:
ClO3- + HAsO2 → Cl- + H3AsO4 + H2O
Now, let's count the number of oxygen atoms on each side:
Left side: 3 oxygen atoms from ClO3- and 2 oxygen atoms from HAsO2, totaling 5 oxygen atoms.
Right side: 4 oxygen atoms from H3AsO4 and 1 oxygen atom from H2O, totaling 5 oxygen atoms.
3. Balance the hydrogen atoms by adding hydrogen ions (H+):
ClO3- + HAsO2 + H+ → Cl- + H3AsO4 + H2O
Now, let's count the number of hydrogen atoms on each side:
Left side: 1 hydrogen atom from HAsO2 and 1 hydrogen atom from H+.
Right side: 3 hydrogen atoms from H3AsO4 and 2 hydrogen atoms from H2O, totaling 5 hydrogen atoms.
4. Finally, balance the charges by adding electrons (e-):
ClO3- + HAsO2 + H+ + 2e- → Cl- + H3AsO4 + H2O
The equation is now balanced.
Water appears in the balanced equation as a product with a coefficient of 1.
The element that is oxidized is As (arsenic). It goes from a lower oxidation state (+3 in HAsO2) to a higher oxidation state (+5 in H3AsO4).