I am having trouble on this homework problem, can you please help me:
If the Ksp for Iron (II) sulfide is 6E-18, what is the concentration of Fe2+ in a saturated solution?
Wouldn't you just take the square root of 6E-18? I tried that, but it says incorrect answer. Please explain how to get the right answer.
If the Ksp for Iron (II) sulfide is 6E-18, what is the concentration of Fe2+ in a saturated solution?
Wouldn't you just take the square root of 6E-18? I tried that, but it says incorrect answer. Please explain how to get the right answer.
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Take the square root of 6E-18, as usual to get 2.449489743e-9.
Then, because of the specific heat involved in the reaction, divide this answer by 1.01
The answer should be 2.425237369e-9
Then, because of the specific heat involved in the reaction, divide this answer by 1.01
The answer should be 2.425237369e-9
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if Ksp = 6x10^-18 then:
6x10^-18 = [Fe2+][S2-]
for a saturated solution, Q = Ksp
therefore, [Fe 2+]
6x10^-18 = x^2
x = [Fe 2+] = 2.45x10^-9M
6x10^-18 = [Fe2+][S2-]
for a saturated solution, Q = Ksp
therefore, [Fe 2+]
6x10^-18 = x^2
x = [Fe 2+] = 2.45x10^-9M