How many grams of sodium sulfate do you need to create 750 mL of a 0.250 M solution of sodium sulfate
How many mols do you need? That's M x L = ?
Convert mols to grams. g = mols x molar mass.
n = MV
n = (0.250 M)(0.750 L) = 0.1875 mol
m = n * MM
m = 0.1875 mol * 142.04 g/mol
m = 27 g
To determine the number of grams of sodium sulfate needed to create a 0.250 M solution, you need to consider the molar mass of sodium sulfate and use the formula:
moles = (molarity) x (volume in liters)
First, convert the given volume of the solution from milliliters to liters:
750 mL = 750/1000 = 0.75 L
Next, calculate the number of moles of sodium sulfate:
moles = (0.250 mol/L) x (0.75 L) = 0.1875 moles
The molar mass of sodium sulfate (Na2SO4) is:
Na: 22.99 g/mol (atomic mass from periodic table)
S: 32.07 g/mol (atomic mass from periodic table)
O: 16.00 g/mol (atomic mass from periodic table)
So, the molar mass of Na2SO4 is:
(2 x 22.99 g/mol) + 32.07 g/mol + (4 x 16.00 g/mol) = 142.04 g/mol
Finally, calculate the mass of sodium sulfate required:
mass = moles x molar mass = 0.1875 mol x 142.04 g/mol = 26.62 grams
You would need approximately 26.62 grams of sodium sulfate to create 750 mL of a 0.250 M solution.