Have 0.02M of KIO3, what is the molaity of IO3?
Since there is 1 mole IO3 per 1 mole KIO3, wouldn't it be 0.02M?
To calculate the molarity of IO3-, we need to know the molar mass of KIO3. The molar mass of KIO3 is calculated as follows:
Molar mass of K: 39.1 g/mol
Molar mass of I: 126.9 g/mol
Molar mass of O: 16.0 g/mol
Total molar mass of KIO3: 39.1 + 126.9 + (3 * 16.0) = 214.0 g/mol
Now, we can calculate the number of moles of KIO3:
0.02 mol/L * 214.0 g/mol = 4.28 g/L
Since we want to determine the molarity of IO3-, we need to divide by the formula weight of IO3-, which is 127.0 g/mol:
4.28 g/L / 127.0 g/mol = 0.034 M
Therefore, the molarity of IO3- in a 0.02 M solution of KIO3 is 0.034 M.
To find the molarity of IO3 in a solution, we need to understand the relationship between molarity, moles, and volume of the solute.
Molarity (M) is defined as the number of moles of solute divided by the volume of the solution in liters.
Given that you have 0.02M of KIO3, this means that you have 0.02 moles of KIO3 dissolved in 1 liter of solution.
KIO3 is a compound made up of one potassium atom (K) and one IO3 ion. Therefore, the molarity of IO3 in the solution is also 0.02M.
In summary, the molarity of IO3 in the solution is 0.02M.