Final answer:
To calculate how many grams of Calcium Sulfate are in the solution, multiply the number of moles (which is the product of molarity and volume) by the molar mass of Calcium Sulfate. The mass of Calcium Sulfate in a 0.55 L of 1.17 M solution is 87.6 g.
Step-by-step explanation:
The question asks how many grams of Calcium Sulfate are dissolved in 0.55 L of a 1.17 M solution. To find this, we need to use the molar mass of Calcium Sulfate (CaSO4) and the formula: Mass = Molarity (M) × Volume (L) × Molar Mass (g/mol).
First, we calculate the number of moles of CaSO4 in the 0.55 L solution using the given molarity.
Number of moles = Molarity × Volume = 1.17 M × 0.55 L = 0.6435 moles
Next, we find the molar mass of CaSO4. The atomic masses are approximately: Ca = 40.08 g/mol, S = 32.06 g/mol, and O = 16.00 g/mol (for the four oxygen atoms, it's 4 × 16.00 g/mol).
Molar mass of CaSO4 = 40.08 g/mol + 32.06 g/mol + (4 × 16.00 g/mol) = 136.14 g/mol
Now, we calculate the mass of CaSO4.
Mass = Moles × Molar mass = 0.6435 moles × 136.14 g/mol = 87.6 g