Find the concentration of Cu+ in equilibrium with CuBr(s) and 0.10 M Br-.
CuBr(s) ===> Cu^+ + Br^-
Ksp = (Cu^+)(Br^-)
(Cu^+)= x
(Br^-) = x+0.10
Substitute and solve for x.
(Ksp of CuBr = 5.0 ✕ 10^−9.)
x = (Br-)- 0.10
how do you get the actual answer for that problem if there is no ksp for it?
Well, it seems like you've brought chemistry to the party! Let's dive into the world of equilibrium and find that concentration of Cu+. Now, I must warn you, it might get a little electrifying.
First, let's write the balanced equation for the dissociation of CuBr(s):
CuBr(s) ↔ Cu+(aq) + Br-(aq)
Now, we know that the initial concentration of Br- is 0.10 M, but we don't know the concentration of Cu+ yet. Let's call it x M.
Since CuBr is a solid, we can assume its concentration remains constant. So, we can say that the concentration of Cu+ and Br- at equilibrium is equal to their respective initial concentrations. Therefore, we have:
[Cu+] = x M
[Br-] = 0.10 M
Now, we can use the equilibrium constant expression, called Ksp, to find x. The Ksp expression for CuBr is:
Ksp = [Cu+][Br-]
Substituting the concentrations, we have:
Ksp = (x)(0.10)
But wait, we need the value of Ksp for CuBr to plug in here. I don't have that information on hand, so I'll have to skip the punchline on this one. I apologize for my limited knowledge, but I hope I was able to help in some way.
To find the concentration of Cu+ in equilibrium with CuBr(s) and 0.10 M Br-, we need to use the concept of solubility and the solubility product constant (Ksp).
1. Write the balanced equation:
CuBr(s) ⇌ Cu+(aq) + Br-(aq)
2. Write the expression for the solubility product constant (Ksp):
Ksp = [Cu+][Br-]
3. We know that the concentration of Br- is 0.10 M, so we can substitute it into the Ksp expression:
Ksp = [Cu+][0.10]
4. Rearrange the equation to solve for [Cu+]:
[Cu+] = Ksp / 0.10
5. Determine the value of Ksp for CuBr. You can look up the value in a reliable source, such as a chemistry textbook or an online database. Suppose the Ksp value for CuBr is 6.3 x 10^-9 mol^2/L^2.
6. Substitute the value of Ksp into the equation:
[Cu+] = (6.3 x 10^-9) / 0.10
7. Calculate the concentration of Cu+:
[Cu+] = 6.3 x 10^-8 M
Therefore, the concentration of Cu+ in equilibrium with CuBr(s) and 0.10 M Br- is 6.3 x 10^-8 M.