Calculate the molarity and normality of a solution made by dissolving 50g of Al(SO4)3 to produce 2.5 liter of solution.
mols Al2(SO4)3 = grams/molar mass = ?
Then M = mols/L solution.
Then N = 6M
To calculate the molarity and normality of a solution, we need to determine the number of moles of the solute (Al(SO4)3) and the volume of the solution (in liters).
Step 1: Find the molar mass of Al(SO4)3.
Aluminum (Al) has a molar mass of 26.98 g/mol.
Sulfur (S) has a molar mass of 32.07 g/mol.
Oxygen (O) has a molar mass of 16.00 g/mol.
The molar mass of Al(SO4)3 = (26.98 g/mol x 1) + (32.07 g/mol x 1) + (16.00 g/mol x 12)
= 342.15 g/mol
Step 2: Calculate the number of moles of Al(SO4)3.
Use the formula: Moles = Mass / Molar mass
Number of moles = 50 g / 342.15 g/mol
≈ 0.146 moles
Step 3: Calculate the molarity.
Molarity (M) is defined as moles of solute divided by liters of solution.
Molarity = Moles / Volume of solution
Molarity = 0.146 moles / 2.5 L
≈ 0.0584 M
The molarity of the solution is approximately 0.0584 M.
Step 4: Calculate the normality.
Normality (N) is a measure of the number of equivalents of a solute per liter of solution.
Since Al(SO4)3 is an acid, we need to find the number of equivalents of Al(SO4)3 for each mole. Al(SO4)3 has three moles of H+ ions per mole.
Number of moles of H+ ions = 0.146 moles x 3
= 0.438 moles
Normality = Moles of H+ ions / Volume of solution
Normality = 0.438 moles / 2.5 L
= 0.175 N
The normality of the solution is approximately 0.175 N.