A 335 -mL can of soda pop is found to contain 40 g of sucrose (C12H22O11). What is the molarity of the solution with respect to sucrose?
To find the molarity of a solution, we need to know the number of moles of the solute (sucrose, in this case) and the volume of the solution.
First, we need to calculate the number of moles of sucrose using its molar mass. The molar mass of sucrose (C12H22O11) can be calculated by adding up the atomic masses of the carbon, hydrogen, and oxygen atoms in the molecule.
The atomic masses are:
Carbon (C) = 12.01 g/mol,
Hydrogen (H) = 1.01 g/mol,
Oxygen (O) = 16.00 g/mol.
Molar mass of sucrose = (12 x 12.01) + (22 x 1.01) + (11 x 16.00) = 342.34 g/mol.
Now, we can calculate the number of moles of sucrose in the can of soda by dividing the mass of sucrose by its molar mass:
Number of moles of sucrose = mass of sucrose / molar mass of sucrose
= 40 g / 342.34 g/mol
≈ 0.117 mol.
Next, we need to determine the volume of the solution in liters. The given volume of the soda can is 335 mL. To convert mL to liters, we divide by 1000:
Volume of the solution = 335 mL / 1000 mL/L
= 0.335 L.
Now, we can calculate the molarity (M) of the sucrose solution using the formula:
Molarity (M) = moles of solute / volume of solution in liters.
Molarity of the sucrose solution = 0.117 mol / 0.335 L
≈ 0.349 M.
Therefore, the molarity of the solution with respect to sucrose is approximately 0.349 M.