Calculate the Molarity of the solution that contains 43.5 grams of K2SO4 in a total volume of 250ml.
mols K2SO4 = grams/molar mass
Then M = mols/L solution.
To calculate the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
First, you need to find the number of moles of K2SO4 (solute). To do this, you can use the equation:
moles = mass / molar mass
The molar mass of K2SO4 is calculated as follows:
(2 * atomic mass of K) + atomic mass of S + (4 * atomic mass of O)
The atomic masses are:
K (potassium) = 39.10 g/mol
S (sulfur) = 32.06 g/mol
O (oxygen) = 16.00 g/mol
Molar mass of K2SO4 = (2 * 39.10) + 32.06 + (4 * 16.00) g/mol = 174.26 g/mol
Now, substitute the given values into the equation:
moles = 43.5 g / 174.26 g/mol
Calculate the number of moles:
moles = 0.2493 mol (rounded to four decimal places)
Next, convert the volume from milliliters (ml) to liters (L):
volume = 250 ml = 0.25 L
Finally, calculate the molarity (M) using the equation:
Molarity = moles / volume
Molarity = 0.2493 mol / 0.25 L
Calculate the molarity:
Molarity = 0.9972 M (rounded to four decimal places)
Therefore, the molarity of the solution containing 43.5 grams of K2SO4 in a total volume of 250 ml is approximately 0.9972 M.