To calculate the molarity of the solution, we will follow these steps:
1. Determine the molecular weight of MnSO4.
2. Calculate moles of MnSO4 using its mass and molecular weight.
3. Convert the volume of the solution from milliliters to liters.
4. Use the number of moles and the volume in liters to calculate the molarity.
Step 1: Determine the molecular weight of MnSO4.
The molecular weight of MnSO4 (Manganese(II) sulfate) can be found by adding the atomic weights of each element in the compound, taking into account their respective quantities in the formula:
Mn: 1 x 54.938 g/mol (for Manganese)
S: 1 x 32.065 g/mol (for Sulfur)
O: 4 x 15.999 g/mol (for Oxygen)
Molecular weight of MnSO4 = (1 x 54.938) + (1 x 32.065) + (4 x 15.999)
= 54.938 + 32.065 + 63.996
= 150.999 g/mol (approximately 151.00 g/mol)
Step 2: Calculate moles of MnSO4 using its mass and molecular weight.
moles = mass (g) / molecular weight (g/mol)
Using the mass of the solute (MnSO4), which is 7.67 grams, we calculate the moles:
moles = 7.67 g / 151.00 g/mol
≈ 0.0508 moles (rounded to four decimal places)
Step 3: Convert the volume of the solution from milliliters to liters.
Since 1 L = 1000 mL, we convert 547 mL into liters by dividing by 1000:
volume = 547 mL / 1000
= 0.547 L
Step 4: Use the number of moles and the volume in liters to calculate the molarity.
Molarity (M) = moles of solute / liters of solution
So the molarity is:
M = 0.0508 moles / 0.547 L
≈ 0.0929 M (rounded to four decimal places)
The molarity of the solution is approximately 0.0929 M.
