Given the molecular mass of fructose = 180.16g/mol, what mass of fructose is required to prepare 1 litre of 0.25M solution ?

To solve this problem, we need to use the formula for molarity which is:

Molarity (M) = moles of solute / volume of solution in liters

We know the molarity (0.25 M) and the volume of the solution (1 L), and we need to find the mass of fructose. But first, we need to find the number of moles of fructose. We can rearrange the formula to find the moles of solute:

moles of solute = Molarity (M) * volume of solution in liters

Substituting the given values:

moles of fructose = 0.25 M * 1 L = 0.25 moles

Now, we know that the molecular mass of fructose is 180.16 g/mol. So, the mass of fructose can be found by multiplying the number of moles by the molecular mass:

mass of fructose = moles of fructose * molecular mass of fructose

Substituting the values:

mass of fructose = 0.25 moles * 180.16 g/mol = 45.04 g

So, 45.04 g of fructose is required to prepare 1 litre of 0.25M solution.