Determine the grams of solute required to prepare 507 ml of a 2.75M NaF solution
To determine the grams of solute required, we need to use the formula:
moles of solute = Molarity x Volume (in liters)
First, we need to convert the volume from milliliters to liters:
507 ml = 507/1000 = 0.507 L
Then we can use the formula to calculate the moles of NaF:
moles of NaF = 2.75 M x 0.507 L = 1.39425 moles NaF
Now we can calculate the grams of NaF by multiplying the moles by the molar mass of NaF. The molar mass of NaF is approximately 41 grams/mol.
grams of NaF = 1.39425 moles NaF x 41 g/mol = 57.08725 grams NaF (rounded to the nearest hundredth)
Therefore, approximately 57.09 grams of NaF are required to prepare 507 ml of a 2.75M NaF solution.
To determine the grams of solute required, you will need to use the formula:
moles = concentration × volume
First, convert the given volume from milliliters (ml) to liters (L):
507 ml ÷ 1000 = 0.507 L
Next, use the given concentration of the solution (2.75 M) to calculate the moles of NaF needed:
moles = 2.75 M × 0.507 L
Now, use the molecular weight of NaF to convert moles to grams:
82.99 g/mol (molecular weight of NaF) × moles
By substituting the values into the equation, you can calculate the grams of NaF required to prepare the solution.