Final answer:
The molarity of a barium carbonate solution when 22g of solute is dissolved in 800 mL of solvent is 0.1393 M, calculated by dividing the moles of solute by the volume of the solution in liters.
Step-by-step explanation:
The student is asking about the molarity of a solution when 22g of barium carbonate (BaCO3) is dissolved in 800 mL of solvent. To calculate molarity, one must first calculate the moles of solute (in this case, BaCO3) using its molar mass, and then divide by the volume of the solution in liters.
The molar mass of BaCO3 is 197.34 g/mol. Therefore, the moles of BaCO3 are calculated as follows:
Moles of BaCO3 = mass (g) / molar mass (g/mol) = 22 g / 197.34 g/mol = 0.1114 mol
Next, to find the molarity, we divide the moles of solute by the volume of the solution in liters:
Molarity (M) = moles of solute / volume of solution (L) = 0.1114 mol / 0.8 L = 0.1393 M
Therefore, the molarity of the barium carbonate solution is 0.1393 M.