Will a precipitate be observed if 0.10 mol Ag+ and 0.001 mol SO42- are added to make 1.0 L of solution? (Ksp = 1.4 x 10-5)
Calculate Qsp and compare with Ksp.
(Qsp = the product of the concns.)
no
Oh, Ag+ and SO42- are having a little get-together in a solution! How exciting! Let's see if they will form a precipitate and crash the party.
To determine if a precipitate will form, we need to compare the value of the ion product (Q) to the solubility product constant (Ksp). If Q is greater than Ksp, then our lovely ions will have too much fun and form a precipitate.
The formula for Q is [Ag+][SO42-]. So let's plug in the values: [Ag+] = 0.10 mol and [SO42-] = 0.001 mol.
Q = (0.10)(0.001) = 0.0001
Now let's compare Q to Ksp. If Q is greater than Ksp (1.4 x 10-5), then it's time to break out the precipitation celebration hats!
0.0001 > 1.4 x 10-5
Uh-oh! It seems like Q is greater than Ksp. So, my friend, a precipitate will indeed be observed when 0.10 mol Ag+ and 0.001 mol SO42- are added to make 1.0 L of solution. Time to get ready for some precipitation party games!
To determine if a precipitate will form when silver ions (Ag+) and sulfate ions (SO42-) are combined, we can calculate the ion product (Qsp) and compare it to the solubility product constant (Ksp).
The solubility product constant (Ksp) is a measure of the equilibrium between the dissociated ions in a saturated solution. It tells us the maximum concentration of the ions that can coexist in a solution at equilibrium before a precipitate starts to form.
In this case, the given Ksp for silver sulfate (Ag2SO4) is 1.4 x 10^-5.
The ion product (Qsp) is similar to the equilibrium constant expression, but it is calculated using the actual concentrations of the ions in the solution, not their equilibrium concentrations. If the ion product (Qsp) is greater than the solubility product constant (Ksp), a precipitate will form.
To calculate the ion product (Qsp), we need to determine the concentrations of the silver ions (Ag+) and sulfate ions (SO42-) in the solution.
Given:
- Amount of Ag+ (silver ions) = 0.10 mol
- Amount of SO42- (sulfate ions) = 0.001 mol
- Volume of solution = 1.0 L
Now, we can calculate the concentrations of the ions:
Concentration of Ag+ = 0.10 mol / 1.0 L = 0.10 M
Concentration of SO42- = 0.001 mol / 1.0 L = 0.001 M
Next, we can calculate the ion product (Qsp) by multiplying the concentrations of the ions:
Qsp = [Ag+] * [SO42-]
= 0.10 M * 0.001 M
= 1 x 10^-4
Lastly, we compare the ion product (Qsp) to the solubility product constant (Ksp):
Qsp = 1 x 10^-4
Ksp = 1.4 x 10^-5
Since Qsp (1 x 10^-4) is greater than Ksp (1.4 x 10^-5), a precipitate will form.