The solubility of PbSO4 is 0.048g/1iter. What is the Ksp of PbSO4? (MM PbSO4 = 303.3)
0.048 g/L PbSO4/ 303.3 g/mol = 1.58E-4 mol/L
Then PbSO4 ---> Pb^2+ + [SO4]^2-
...........solid...........1,58E-4....1.58E-4
Ksp = (Pb^2+)(SO4^2-)
Plug in the solubility shown and turn the crank for value of Ksp. Check my arithmetic.
Oh PbSO4, the shy little compound that doesn't like to dissolve. Well, if the solubility of PbSO4 is 0.048g/1 liter, then we can use that information to calculate its Ksp (the solubility product constant).
But before we delve into that, let's have a quick laugh. Why did the PbSO4 molecule refuse to dissolve completely? Because it didn't want to be a "problem-dissolving" compound!
Now, back to business. To find the Ksp of PbSO4, we need to first convert the solubility from grams per liter to moles per liter. The molar mass of PbSO4 is 303.3 g/mol, so let's do some math.
0.048 g / 303.3 g/mol = 0.0001583 mol/1 liter
Now, the Ksp expression for PbSO4 is Ksp = [Pb2+][SO42-]. However, since PbSO4 is sparingly soluble, we can assume that it completely dissociates into its ions.
So, the concentration of both Pb2+ and SO42- is equal to 0.0001583 mol/1 liter.
Thus, the Ksp of PbSO4 is approximately 0.0001583^2, which is equal to... (*calculating noises*)... drumroll please...
Ksp ≈ 2.50873 × 10^-8
And there you have it! The Ksp of PbSO4 is approximately 2.50873 × 10^-8. I hope this answer brought a smile to your face, like a clown brings smiles to everyone's faces!
To find the Ksp (solubility product constant) of PbSO4, we need to use the information given about its solubility.
The solubility of PbSO4 is provided as 0.048g/1 liter. We can use this information to determine the concentration of Pb2+ and SO42- ions in the saturated solution.
The molar mass of PbSO4 is 303.3 g/mol.
To find the concentration of Pb2+ ions, we can use the equation:
concentration (mol/L) = mass (g) / molar mass (g/mol)
concentration of Pb2+ = 0.048g / 303.3 g/mol
Next, we need to determine the concentration of SO42- ions. Since PbSO4 has a 1:1 stoichiometric ratio of Pb2+ to SO42-, the concentration of SO42- will be the same as the concentration of Pb2+.
Now that we have the concentrations of Pb2+ and SO42- ions, we can write the solubility product expression for PbSO4:
Ksp = [Pb2+][SO42-]
Since the concentration of Pb2+ and SO42- ions are the same, we can substitute the values:
Ksp = (concentration of Pb2+) * (concentration of SO42-)
Ksp = (0.048g / 303.3 g/mol) * (0.048g / 303.3 g/mol)
Evaluating the expression gives the value of Ksp for PbSO4.
To find the Ksp (solubility product constant) of PbSO4, we need to understand the relationship between the solubility and the Ksp.
First, let's write the balanced equation for the dissolution of PbSO4:
PbSO4(s) ⇌ Pb2+(aq) + SO42-(aq)
The solubility of PbSO4 given is 0.048 g/1 liter. Since the molar mass of PbSO4 is 303.3 g/mol, we can convert the solubility to moles per liter:
Solubility (mol/L) = 0.048 g / 303.3 g/mol = 0.0001583 mol/L
Now, let's define the expression for the solubility product constant (Ksp):
Ksp = [Pb2+][SO42-]
Since the stoichiometric coefficient for both Pb2+ and SO42- in the balanced equation is 1, the molar solubility of PbSO4 is equal to the concentration of both Pb2+ and SO42-. Therefore, we can simplify the expression to:
Ksp = s^2, where s is the molar solubility (mol/L) of PbSO4.
Plugging in the value of molar solubility, we have:
Ksp = (0.0001583 mol/L)^2 = 2.5028 × 10^-8
Thus, the Ksp of PbSO4 is approximately 2.5028 × 10^-8.