A community for students.
Here's the question you clicked on:
 0 viewing
vera_ewing
 one year ago
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.
vera_ewing
 one year ago
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.

This Question is Closed

rvc
 one year ago
Best ResponseYou've already chosen the best response.1i dont remember :/ maybe B

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0The constant determines the way moles dissolve per litre of a solution.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0So which one is it? @Hoslos

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0For 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

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I am not sure about this one. What do you say @sweetburger ?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1Well 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.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1Thats just my idea though.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1I think it should be A.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0How about this one?

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1Well 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.

rvc
 one year ago
Best ResponseYou've already chosen the best response.1keep up the good work guys @sweetburger @Hoslos

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1I disagree as CaF2 has a greater Ksp than CaCO3.

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0What 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.

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.1I agree with @Hoslos

vera_ewing
 one year ago
Best ResponseYou've already chosen the best response.0In which of the following cases will there be precipitation? A. Q < Ksp B. Q = Ksp C. Q << Ksp D. Q > Ksp
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.