What is the molarity of a solution containing 5.035grams of FeCl3 in enough water to make 500 ml of solution?
First, we need to calculate the number of moles of FeCl3:
moles = mass / molar mass
The molar mass of FeCl3 is 162.2 g/mol.
moles = 5.035 g / 162.2 g/mol = 0.031 moles
Next, we need to calculate the volume in liters:
500 ml = 0.5 L
Finally, we can calculate the molarity:
Molarity = moles of solute / liters of solution
Molarity = 0.031 moles / 0.5 L = 0.062 M
Therefore, the molarity of the solution is 0.062 M.
To calculate the molarity of a solution, we need to know the number of moles of the solute and the volume of the solution.
Step 1: Calculate the number of moles of FeCl3.
To do this, we need to know the molar mass of FeCl3. The molar mass of Fe is 55.845 g/mol, and the molar mass of Cl is 35.453 g/mol.
Fe: 1 atom x 55.845 g/mol = 55.845 g/mol
Cl: 3 atoms x 35.453 g/mol = 106.359 g/mol
Total molar mass of FeCl3 = 55.845 g/mol + 106.359 g/mol = 162.204 g/mol
Number of moles of FeCl3 = mass / molar mass
Number of moles of FeCl3 = 5.035 g / 162.204 g/mol ≈ 0.031 moles
Step 2: Calculate the volume of the solution in liters.
The volume of the solution is given as 500 ml. To convert this to liters, we divide by 1000.
Volume of the solution = 500 ml / 1000 ml/L = 0.5 L
Step 3: Calculate the molarity.
Molarity (M) = moles of solute / volume of solution in liters
Molarity (M) = 0.031 moles / 0.5 L
Molarity (M) ≈ 0.062 M
Therefore, the molarity of the solution is approximately 0.062 M.