What is the molarity of a solution prepared by placing 7.2 g of glucose in a volumetric flask and adding water to get 250.0 mL of solution?
it is pretty dilute, if you assume the density of the solution is close to 1.00, then the amount of solvent added was 250 grams. Without other information, you have to assume that.
molarity=molessolute/.250kg
mols glucose = grams/molar mass = ?
M = mols/0.250 L = ?
I get an answer of 0.16 = M
To find the molarity of a solution, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, let's calculate the number of moles of glucose in the solution.
The molar mass of glucose (C6H12O6) is:
(6 * atomic mass of carbon) + (12 * atomic mass of hydrogen) + (6 * atomic mass of oxygen) = 180.16 g/mol
To calculate moles of glucose, we divide the mass of glucose by its molar mass:
moles of glucose = mass of glucose / molar mass of glucose
moles of glucose = 7.2 g / 180.16 g/mol
Next, we need to convert the volume of the solution from milliliters to liters:
volume of solution (L) = 250.0 mL / 1000 mL/L
Now, we have all the information needed to calculate the molarity of the solution:
Molarity (M) = moles of glucose / volume of solution in liters
Molarity = (7.2 g / 180.16 g/mol) / (250.0 mL / 1000 mL/L)
Calculating this expression will give us the molarity of the solution.