Question

What is the molarity of a solution of 12.9 G fructose C6H12O6
and 31.0g water

Answer 1

2.31 M

Step-by-step explanation:

Mass of fructose = 12.9 g

Molar mass of fructose (C6H12O6) = 180.16 g/mol

Number of moles of fructose = mass / molar mass

Number of moles of fructose = 12.9 g / 180.16 g/mol

Number of moles of fructose = 0.0716 mol

Next, we need to calculate the volume of the solution. Since the mass of water is given, we can assume the density of the solution is the same as that of water (1 g/mL). Therefore, the volume of the solution is:

Mass of water = 31.0 g

Density of water = 1 g/mL

Volume of solution = mass / density

Volume of solution = 31.0 g / 1 g/mL

Volume of solution = 31.0 mL

Now that we have the number of moles of fructose and the volume of the solution, we can calculate the molarity:

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

Molarity = 0.0716 mol / (31.0 mL / 1000 mL/L)

Molarity = 2.31 M

Therefore, the molarity of the solution is 2.31 M.