Which of the following is true of the solubility product constant?
A. It is an equilibrium position.
B. Its value changes in the presence of a common ion.
C. It is an equilibrium constant.
D. It is the product of the initial concentrations of the ions in a solution.
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i dont remember :/
The constant determines the way moles dissolve per litre of a solution.
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So which one is it? @Hoslos
It was C.
It's okay :)
For an endothermic dissolution process, which of the following would you observe on cooling a saturated solution by 10°C?
A. An increase in precipitation
B. A decrease in volume
C. An increase in solubility
D. A decrease in pressure
I am not sure about this one.
What do you say @sweetburger ?
Well if the dissolving process is endothermic that means energy is a reactant. If we are cooling the solution then we are taking energy out which is decreasing the amount of reactants which induces a stress on the system which would in turn cause more reactant to be formed which would result in precipitation.
Well the salts with the largest Ksp value will come first which would be Salt D with a very large Ksp of 38.65. Then second would be A with a Ksp of 9.21x10^-8. So the list so Far Is D,A and then the only answer choice which is arranged like this is D. being D,A,B,C. If you continued to look at the Ksp of the remaining salts you would notice that D,A,B,C holds true.
What is the nature of a solution when it has reached its solubility equilibrium?
A. The solution is saturated.
B. The temperature of the solution always rises.
C. The solution is undergoing precipitation.
D. The Ksp of the solution is greater than its Q.
I agree with @Hoslos
i go with A
In which of the following cases will there be precipitation?
A. Q < Ksp
B. Q = Ksp
C. Q << Ksp
D. Q > Ksp