When the equation Cl2 ---> Cl- + ClO3- (basic solution) is balanced using the smallest whole-number coefficients, the coefficient of OH- is??

To balance the given equation Cl2 ---> Cl- + ClO3- in a basic solution, follow these steps:

Step 1: Write down the unbalanced equation:
Cl2 ---> Cl- + ClO3-

Step 2: Balance the chlorine atoms:
There are two chlorine atoms on the left side and one chlorine atom on the right side. To balance the chlorine atoms, put a coefficient of 2 in front of Cl- and ClO3-:
Cl2 ---> 2Cl- + ClO3-

Step 3: Balance the oxygen atoms:
There are three oxygen atoms on the right side (two from ClO3- and one from OH-). To balance the oxygen atoms, put a coefficient of 3/2 (or 1.5) in front of OH-:
Cl2 ---> 2Cl- + ClO3- + 3/2OH-

However, since we want to use whole-number coefficients, we can multiply the entire equation by 2 to get rid of the fraction:
2Cl2 ---> 4Cl- + 2ClO3- + 3OH-

Therefore, the coefficient of OH- in the balanced equation is 3.

To balance the given equation Cl2 ---> Cl- + ClO3- in a basic solution, you need to follow the steps outlined below:

Step 1: Balance the chlorine atoms:
There are 2 chloride ions (Cl-) on the product side, so you need to ensure the same number on the reactant side. Multiply the Cl- on the left side by 2:

Cl2 + 2Cl- ---> Cl- + ClO3-

Step 2: Balance the oxygen atoms:
There are three oxygen atoms in the chlorate ion (ClO3-) on the product side. To balance the number of oxygen atoms, you need to add three hydroxide ions (OH-) to the reactant side because they are commonly used to balance oxygen atoms in basic solutions:

Cl2 + 2Cl- ---> Cl- + ClO3- + 3OH-

Now the oxygen atoms are balanced.

Step 3: Check and balance the charges:
The charges also need to be balanced. On the left side, there is a total charge of -2 (2Cl-). On the right side, there is a total charge of -2 ([Cl-] + [ClO3-] + 3[OH-]). Therefore, the charges are already balanced.

The coefficient of OH- is 3 in the balanced equation: Cl2 + 2Cl- ---> Cl- + ClO3- + 3OH-

Where is the answer

http://www.chemteam.info/Redox/Redox.html