What is the molarity of a sucrose solution that contains 76.7 g of C12H22O11 (342.34 g/mol) dissolved in 138.2 mL of solution
To find the molarity of a solution, you need to know the number of moles of solute and the volume of the solution in liters.
First, let's calculate the number of moles of sucrose (C12H22O11) in the solution:
Number of moles = mass of sucrose / molar mass of sucrose
The molar mass of sucrose (C12H22O11) is 342.34 g/mol, and the mass of sucrose in the solution is 76.7 g.
Number of moles = 76.7 g / 342.34 g/mol
Next, convert the volume of the solution from milliliters to liters:
Volume of solution = 138.2 mL = 138.2 mL x (1 L/1000 mL)
Now we have all the necessary values to calculate the molarity:
Molarity (M) = Number of moles / Volume of solution
Let's calculate this:
Number of moles = 76.7 g / 342.34 g/mol = 0.224 mol
Volume of solution = 138.2 mL x (1 L/1000 mL) = 0.1382 L
Molarity (M) = 0.224 mol / 0.1382 L = 1.621 M
Therefore, the molarity of the sucrose solution is 1.621 M.