A solution was prepared by dissolving 0.163 g of sugar, (C12H22O11 MW = 3423gmol)
in 100.00 mL water. What is the molarity of this solution?
You left out a decimal in the MW. It is 342.3 g/mol. 0.163 g is therefore 0.000475 moles. Divide that by 0.100 L to get the molarity (M)in moles/Liter
To find the molarity of a solution, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, we need to calculate the moles of sugar (C12H22O11) in the solution.
Number of moles = mass of solute / molar mass
Molar mass of sugar (C12H22O11) = 12*12 + 22*1 + 11*16 = 342
Number of moles = 0.163 g / 342 g/mol = 0.000476 moles
Next, we need to convert the volume of the solution from milliliters to liters.
Volume of solution = 100.00 mL = 100.00 mL / 1000 mL/L = 0.100 L
Now, we can calculate the molarity of the solution.
Molarity = 0.000476 moles / 0.100 L = 0.00476 M
Therefore, the molarity of the solution is 0.00476 M.