How many grams of magnesium chloride are needed to prepare 100ml of a 0.325 M MgCl2 solution?
mass=molarity*molmassMgCl2*volumeinliters
mols = M x L = ?
Then mols = grams/molar mass. Solve for grams.
To find out how many grams of magnesium chloride are needed to prepare a given solution, you need to use the equation:
Molarity (M) = moles/volume (L)
First, convert the volume into liters:
100 mL = 100/1000 = 0.1 L
Next, you need to rearrange the equation to solve for moles:
moles = Molarity × volume
Substituting the given values:
moles = 0.325 M × 0.1 L
Calculate the moles of MgCl2:
moles = 0.0325 moles
To convert moles to grams, you need to use the molar mass of magnesium chloride. The molar mass of MgCl2 can be calculated as follows:
(24.305 g/mol) + 2 × (35.453 g/mol) = 95.211 g/mol
Now, multiply the moles by the molar mass to find the grams of magnesium chloride needed:
grams = moles × molar mass
grams = 0.0325 moles × 95.211 g/mol
Calculating this gives:
grams = 3.090 g
Therefore, you would need approximately 3.090 grams of magnesium chloride to prepare 100 mL of a 0.325 M MgCl2 solution.