The solubility product constant, Ksp, for nickel (II) carbonate, NiCO3, is 1.3 x 10-7 at 25C.
a. Write the balanced chemical equation for this dissolving process
b. Write the equilibrium expression
c. Find the maximum molar concentration of all ions in solution
Please help!
, Ksp, for nickel (II) carbonate, NiCO3, is 1.3 x 10-7 at 25C.
a. Write the balanced chemical equation for this dissolving process
b. Write the equilibrium expression
c. Find the maximum molar concentration of all ions in solution
...............NiCO3(s) + H2O ==> Ni^2+(aq) + [CO3]^2-(aq)
I...................solid..........(l)............0....................0
C..................solid(-x)....(l).............x....................x
E...................solid..........(l).............x....................x
Ksp = (Ni^2+)[CO3]^2- = 1.3E-7. Substitute from the E line into Ksp expression.
1.3E-7 = (x)(x) = x^2
x = sqrt(1.3E-7) = ? M
So (Ni^2+) = x = [CO3]^2- = approx 3.6E-4 M
NOTE: I don't know exactly how your prof writes these equations or expressions so you may need to adjust what I wrote to match how your class usually does it. For example I don't usually write H2O in the dissolution process. Also, I show -x for the solid change but solid-x still is a solid.
thank you so much!
a. Well, when nickel (II) carbonate decides to dissolve, it becomes nickel (II) ions and carbonate ions. It's like they're saying, "Hey, we're gonna break free and explore the watery wonders out there!" So, the balanced chemical equation for this mighty dissolving process is:
NiCO3 (s) ↔ Ni2+ (aq) + CO32- (aq)
b. Now, let's talk about equilibrium expression. This is where things get a little serious. The equilibrium expression for this captivating dissolving process is:
Ksp = [Ni2+][CO32-]
c. Ah, the maximum molar concentration! It's like finding out who the star of the show is. So, since our equilibrium expression is:
Ksp = [Ni2+][CO32-]
And since we have a solubility product constant of Ksp = 1.3 x 10^-7, we can say that the maximum molar concentration of all ions in solution corresponds to the value of Ksp.
So, the maximum molar concentration of nickel (II) ions and carbonate ions in solution is 1.3 x 10^-7 mol/L.
a. The balanced chemical equation for the dissolving process of nickel (II) carbonate, NiCO3, can be written as:
NiCO3 (s) ⇌ Ni2+ (aq) + CO3^2- (aq)
b. The equilibrium expression for this dissolution process can be written as:
Ksp = [Ni2+] * [CO3^2-]
c. To find the maximum molar concentration of all ions in solution, we can assume that all of the nickel carbonate has dissolved, and calculate the concentration of each ion separately.
Let x represent the molar concentration of NiCO3 that dissolves.
Since the stoichiometry of the balanced equation is 1:1:1, the molar concentration of Ni2+ and CO3^2- ions in the solution will also be equal to x.
Therefore, the maximum molar concentration of both Ni2+ and CO3^2- ions in solution is x.
Hence, the maximum molar concentration of all ions in solution is x.
Of course! I'd be happy to help you with this question.
a. To write the balanced chemical equation for the dissolving process of nickel (II) carbonate (NiCO3), we need to know the solubility behavior of the compound. Since the solubility product constant, Ksp, is given, we can assume that NiCO3 dissociates completely in water to form nickel (II) ions (Ni2+) and carbonate ions (CO32-). Therefore, the balanced chemical equation for this dissolving process is:
NiCO3 (s) -> Ni2+ (aq) + CO32- (aq)
b. The equilibrium expression is written using the concentrations of the ions in the equilibrium state. Since nickel (II) carbonate is a solid, it is not included in the equilibrium expression. The equilibrium expression for this reaction can be written as follows:
Ksp = [Ni2+] * [CO32-]
c. To find the maximum molar concentration of all ions in solution, we need to know the solubility of nickel (II) carbonate. From the given Ksp value, we can see that the product of the molar concentrations of Ni2+ and CO32- is equal to 1.3 x 10-7. Assuming that the solubility of NiCO3 is "x", we can write the following expression:
Ksp = [Ni2+] * [CO32-] = (x)(2x) = 4x^2
Setting this equal to the given Ksp value, we have:
1.3 x 10-7 = 4x^2
Solving this equation for "x", we find the maximum molar concentration of all ions in solution.