The molarity of Sr2+ in a saturated solution of SrSO4 was determined to be 0.000500 M. Calculate the solubility product constant (Ksp) for SrSO4.
SrSO4(s) = Sr^2+(aq) + SO4^2- (aq)
Molar Mass (g/mol)
SrSO4 183.68
This is what I know:
Ksp = [Sr][SO4]
You also know that 1 mole SrSO4 gives 1 mole Sr^+2 and 1 mole SO4^-2.
The problem gives you the concn of Sr^+2 as 5 x 10^-4, sulfate is the same, substitute into the expression you wrote for Ksp and you have it.
Well, it seems like you have a bit of a chemical puzzle there. Let me put on my clown nose and see if I can help you out with some humor!
Knock, knock!
Who's there?
SrSO4.
SrSO4 who?
SrSO4, you sure you want to know the Ksp? Let's calculate it and see if it can crack a smile on your face!
To find the Ksp, we need to know the concentrations of Sr^2+ and SO4^2- ions which come from the dissociation of SrSO4.
Since the molarity of Sr^2+ is 0.000500 M, we can set [Sr^2+] = 0.000500 M.
Now, remember that 1 molecule of SrSO4 gives 1 Sr^2+ ion and 1 SO4^2- ion. Therefore, the concentration of SO4^2- ions will also be 0.000500 M.
Now let's plug these values into the equation!
Ksp = [Sr^2+][SO4^2-]
= (0.000500 M)(0.000500 M)
= 0.000000250 M
So, the solubility product constant (Ksp) for SrSO4 is 0.000000250 M. In other words, it's as tiny as a clown car in a sea of confetti!
I hope that put a smile on your face and helped solve your chemistry question. If you have any more questions, feel free to ask!
To find the solubility product constant (Ksp) for SrSO4, we need to use the molarity of Sr2+ in a saturated solution, which is 0.000500 M.
Since SrSO4 dissociates into Sr^2+ and SO4^2- ions, the concentration of Sr^2+ in a saturated solution is also 0.000500 M.
Now, to calculate the solubility product constant (Ksp), we can use the formula:
Ksp = [Sr^2+][SO4^2-]
Since the concentrations of both Sr^2+ and SO4^2- are the same, we can substitute the value 0.000500 M into the equation:
Ksp = (0.000500 M)(0.000500 M)
Ksp = 2.50 x 10^-7
Therefore, the solubility product constant (Ksp) for SrSO4 is 2.50 x 10^-7.
To calculate the solubility product constant (Ksp) for SrSO4, we need to use the information provided. The balanced equation for the dissociation of SrSO4 is:
SrSO4(s) ⇌ Sr^2+(aq) + SO4^2-(aq)
We are given that the molarity of Sr^2+ in the saturated solution is 0.000500 M.
To find the molarity of SO4^2- in the saturated solution, we need to use stoichiometry. From the balanced equation, we can see that the ratio of Sr^2+ to SO4^2- is 1:1. Therefore, the molarity of SO4^2- in the saturated solution is also 0.000500 M.
Now, we can substitute these values into the expression for Ksp:
Ksp = [Sr^2+][SO4^2-]
Ksp = (0.000500 M)(0.000500 M)
Ksp = 2.5 x 10^-7 M^2
Therefore, the solubility product constant (Ksp) for SrSO4 is 2.5 x 10^-7 M^2.