how many grams of KIO3 are needed to make 50.0 mL of a 1.2 M KIO3 solution
Remember the definition of molarity.
M # moles/L.
To convert g to moles, moles = grams/molar mass.
To calculate the number of grams of KIO3 needed to make a 1.2 M KIO3 solution, we can use the formula:
Molarity (M) = moles of solute / volume of solution (L)
First, let's convert the given volume from mL to L:
50.0 mL = 50.0 mL / 1000 mL/L = 0.0500 L
Now, rearrange the formula to solve for moles of solute:
moles of solute = Molarity × volume of solution
moles of solute = 1.2 mol/L × 0.0500 L = 0.06 moles
Now, we need to find the molar mass of KIO3. By adding up the atomic masses of potassium (K), iodine (I), and oxygen (O) in KIO3, we get:
Molar mass of KIO3 = 39.10 g/mol + (126.90 g/mol + 3 × 16.00 g/mol) = 214.00 g/mol
Finally, we can calculate the grams of KIO3 needed by multiplying the moles of solute by the molar mass:
grams of KIO3 = moles of solute × molar mass
grams of KIO3 = 0.06 moles × 214.00 g/mol = 12.84 grams
Therefore, approximately 12.84 grams of KIO3 are needed to make 50.0 mL of a 1.2 M KIO3 solution.