Calculate the molar solubility of FeCO3 . How many grams of FeCO3 are present in 15.0 L of a saturated FeCO3 solution?
...........FeCO3 ==> Fe^2+ + CO3^2-
I......................0.......0
C......................x.......x
E.......................x.......x
Ksp = (Fe^2+)(CO3^2-)
Substitute from the ICE chart and for Ksp (look up that value) and solve for x = solubility
To calculate the molar solubility of FeCO3, we need to know its Ksp (solubility product constant), which represents the equilibrium constant for the dissociation of FeCO3 in water. Unfortunately, the Ksp for FeCO3 was not provided in the question.
To calculate the grams of FeCO3 present in 15.0 L of a saturated solution, we need to know the molar solubility of FeCO3 and its molar mass.
Let's assume that the molar solubility of FeCO3 is given. We'll use "x" to represent the molar solubility.
First, write the balanced equation for the dissociation of FeCO3 in water:
FeCO3(s) ⇌ Fe2+(aq) + CO3-2(aq)
The solubility product expression for FeCO3 is:
Ksp = [Fe2+][CO3-2]
Since the dissociation produces equal amounts of Fe2+ and CO3-2 ions, the expression simplifies to:
Ksp = x * x = x^2
Now we can proceed to calculate the grams of FeCO3 present in 15.0 L of saturated solution.
1. Calculate the concentration of FeCO3 in moles/L (Molarity):
Molarity (M) = moles of solute / volume of solution (L)
2. From the molar solubility, we know that x moles of FeCO3 dissolve per liter. Therefore, the molarity of FeCO3 is also x.
3. Convert the molarity from moles/L to grams/L:
Use the molar mass of FeCO3 to convert moles to grams.
Grams/L = Molarity (mol/L) * Molar mass (g/mol)
4. Finally, calculate the grams of FeCO3 present in 15.0 L of solution:
Grams = Grams/L * Volume (L)
Remember to substitute the value of x for the molar solubility to calculate the grams of FeCO3 present in the given solution.