The Ksp for nickel(II) hydroxide is 5.47E-16. What is the base dissociation constant for nickel(II) hydroxide?
So I started off doing
Ni(OH)2 (s) <-> Ni2+ (aq) + 2OH- (aq)
I ..........................0 .................0
C ........................+x ................+2x
E ........................x ..................2x
Ksp = [Ni2+][OH-]^2
= (x)(2x)^2
= 4x^3
3sqrt 5.47E-16/4 =x
5.15E-6 = x
Wouldn't Kb just be
Kb = [Ni2+][OH-]^2 ??
And then If I solved it by subbing in x, I'd just get the Ksp value... Is Kb supposed to be the same as the Ksp value?
Frankly I never heard of this; however, it appears Ksp and Kb are the same for this.
My calculator is on the blink so I can't check your answer.
Yes, it's the answer inside my workbook for the same question
Well, it seems like you're in quite a pickle. Let me help you out with a humorous twist!
Ah, the joys of chemistry calculations! It's like juggling equations while riding a unicycle. Now, let's dive into your question.
Kb, the base dissociation constant, relates to how well a base dissociates in water, while Ksp refers to the solubility product constant of a sparingly soluble compound. In this case, we are dealing with a base, nickel(II) hydroxide (Ni(OH)2).
Now, if you're wondering if Kb should be the same as Ksp, well, it's like asking if a clown car should be the same as a unicycle - they're related, but different!
Kb is calculated by considering the concentration of hydroxide ions (OH-) and the concentration of nickel(II) ions (Ni2+) produced when the base dissociates. It's different from Ksp, which only considers the concentrations of the products (Ni2+ and OH-) in a saturated solution.
So, to find Kb, you need to establish an equation that represents the dissociation of nickel(II) hydroxide in water. Then, consider the concentrations of Ni2+ and OH- at equilibrium, and use those values to calculate Kb.
Remember, chemistry can be a bit of a clown show sometimes, but with a little bit of humor, you can solve any problem! Good luck!
No, Kb is not the same as Ksp. Ksp (solubility product constant) refers to the equilibrium constant for the dissolution of a sparingly soluble salt, while Kb (base dissociation constant) refers to the equilibrium constant for the dissociation of a weak base in water.
In the case of nickel(II) hydroxide, if we consider it as a weak base, its dissociation equilibrium would be:
Ni(OH)2 + H2O ↔ Ni(OH)3- + H+
The base dissociation constant (Kb) for nickel(II) hydroxide would then be:
Kb = [Ni(OH)3-][H+]/[Ni(OH)2]
To find Kb, you would need to know the concentrations of the nickel(II) hydroxide species in the equilibrium mixture. Unfortunately, without that information, it is not possible to determine the exact value of Kb.
No, Kb is not the same as Ksp.
Ksp stands for the solubility product constant, which describes the equilibrium between the solid compound and its dissolved ions in a solution. It is a measure of the extent to which a slightly soluble compound dissociates into its ions. In the case of nickel(II) hydroxide (Ni(OH)2), the Ksp is 5.47E-16.
On the other hand, Kb stands for the base dissociation constant, and it describes the equilibrium between a base and its conjugate acid in a solution. It is a measure of the strength of a base. In the case of nickel(II) hydroxide, we are looking for the Kb, which represents the strength of the hydroxide-ion (OH-) as a base.
To find the Kb for nickel(II) hydroxide, you need to set up the equation for the dissociation of the hydroxide ions in water:
OH- (aq) + H2O (l) ↔ O2- (aq) + H3O+ (aq)
I...........0.........................0
C..........+x....................+x......+x
E..........x.....................x......x
The Kb expression for this reaction is:
Kb = [O2-][H3O+]/[OH-]
Since the concentration of water remains essentially constant, we can approximate it as 1, so the equation becomes:
Kb = [O2-][H3O+]/[OH-] = [O2-][H3O+]/x
In the case of nickel(II) hydroxide, the concentration of OH- is 2x, as you correctly determined. However, the concentration of H3O+ (hydronium ion) and O2- (hydroxide ion) in water can be considered negligible compared to OH- concentration. Therefore, we can ignore their presence, and the Kb expression simplifies to:
Kb ≈ [OH-]/x = (2x)/x = 2
Hence, the base dissociation constant for nickel(II) hydroxide, Kb, would be approximately equal to 2.
So, in summary, while the Ksp represents the solubility product constant, Kb represents the base dissociation constant, and they are calculated using different equations and have different meanings.