Question

Calculate the quantity (in grams) of sucrose (C12H22011) required to make a 1.00 M strength solution with a volume of 500. mL.

Answer 1

Let us first define the term molarity. Molarity is a way of expressing the concentration of a compound in solution and is defined as the number of moles per liter of solution.

We are given the molarity value, 1.00M, and the volume of the solution, 500 mL=0.5L. We can find the number of moles by clearing them from the following equation:

`\begin{gathered} Molarity=(MolesSolute)/(Lsolution) \\ MolesSolute=Molarity* Lsolution \end{gathered}`

We replace the known data:

`\begin{gathered} MolesSolute=1.00M*0.5L \\ MolesSolute=1.00(mol)/(L)*0.500L=0.500molC_(12)H_(22)O_(11) \end{gathered}`

Now, the grams of sucralose are found by multiplying the moles found by the molar mass of sucralose, which is 342.3 g/mol:

`gC_(12)H_(22)O_(11)=0.500molC_(12)H_(22)O_(11)*(342.3gC_(12)H_(22)O_(11))/(1molC_(12)H_(22)O_(11))=171gC_(12)H_(22)O_(11)`

The quantity of sucrose required will be 171 g of sucrose