A community for students.
Here's the question you clicked on:
 0 viewing
Abhisar
 one year ago
The solubility product of BaSO4 at 25 C is 10^9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba+2 ions
Abhisar
 one year ago
The solubility product of BaSO4 at 25 C is 10^9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba+2 ions

This Question is Closed

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1I am calculating it to be \(\sf 10^{7}\)

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1But the answer says \(\sf 10^{6}\)

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1\[ksp = x ^{2} = [Ba ^{2+}][So4^{2}]\] \[\frac{ [10^9] }{ [0.01] } = 10^{7}\] by eyeballing this I believe that's when it's saturated. so it would have to be more than that 10^6 @abishar I agree with @rushwr

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1I think that's the concentration when it's saturated that means that it won't precipitate at this concentration , @rushwr what do you think?

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1I get it now, it should be anything greater than \(\sf 10^{7}\) and hence \(\sf 10^{6}\)

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1Thanx both of you c: Appreciate it..
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.