What pH buffer solution is needed to give a Ni2+ concentration of 2.5 x 10-3M in equilibrium with solid nickel hydroxide Ni(OH)2? Ksp = 6.0 x 10-16.

Ksp = (Ni^2+)(OH^-)^2

Substitute Ni from the problem into the Ksp expression and solve for Oh^-, then convert this to pH.

Well, well, well, looks like we have some chemistry fun going on here! Alright, let's see what we can come up with.

To determine the pH buffer solution needed, we need to consider the equilibrium between the nickel ion (Ni2+) and the solid nickel hydroxide (Ni(OH)2). Lucky for us, we've got a Ksp value to work with!

The Ksp expression for this reaction is:

Ni(OH)2(s) ⇌ Ni2+(aq) + 2OH-(aq)

Now, let's start by writing the Ksp expression:

Ksp = [Ni2+][OH-]^2

Given that Ksp = 6.0 x 10^-16, and we know the concentration of Ni2+ needed (2.5 x 10^-3M), we can rearrange the equation to find the concentration of OH- ions:

6.0 x 10^-16 = (2.5 x 10^-3)(OH-)^2

Solving this equation will give us the concentration of OH-. After that, we can use that concentration to find the pH of the solution.

However, since you're looking for a buffer solution, we want to maintain the pH of the solution within a certain range. So, we need to choose a weak acid and its conjugate base to create a buffer.

Let me know if you have a specific acid and its conjugate base in mind, and I'll be more than happy to guide you through the process and maybe throw in a joke or two along the way!

To determine the pH buffer solution needed to give a Ni2+ concentration of 2.5 x 10^-3 M in equilibrium with solid nickel hydroxide (Ni(OH)2), we first need to write the balanced equation for the dissolution of nickel hydroxide:

Ni(OH)2 (s) ⇌ Ni^2+ (aq) + 2OH- (aq)

The solubility product constant (Ksp) for nickel hydroxide is given as 6.0 x 10^-16. This means that at equilibrium, the product of the concentration of Ni^2+ ions and OH- ions must be equal to Ksp. Utilizing this information, we can set up an expression to calculate the concentration of OH- ions at equilibrium:

Ksp = [Ni^2+][OH-]^2

Since the concentration of Ni^2+ ions is given as 2.5 x 10^-3 M, we can substitute this value into the equation:

6.0 x 10^-16 = (2.5 x 10^-3)[OH-]^2

To solve for the concentration of OH- ions, we rearrange the equation and take the square root of both sides:

[OH-] = √(6.0 x 10^-16 / 2.5 x 10^-3)
= √(2.4 x 10^-13)
≈ 4.9 x 10^-7

Now that we know the concentration of OH- ions, we can use this information to calculate the pH. The pH is determined by the concentration of H+ ions, which is related to the concentration of OH- ions by the expression:

pH = -log [H+]

Since water autoionizes to produce equal concentrations of H+ and OH- ions, we can use the concentration of OH- ions as an approximation for H+ ions:

[H+] ≈ [OH-]
[H+] ≈ 4.9 x 10^-7

Taking the negative logarithm of the concentration of H+ ions, we get:

pH = -log (4.9 x 10^-7)
≈ 6.31

Therefore, a pH buffer solution with a pH of approximately 6.31 is needed to give a Ni2+ concentration of 2.5 x 10^-3 M in equilibrium with solid nickel hydroxide (Ni(OH)2).

To determine the pH buffer solution needed to give a certain concentration of Ni2+ in equilibrium with solid nickel hydroxide (Ni(OH)2), we need to use the solubility product constant (Ksp) and the appropriate equilibrium equation.

The equilibrium equation for the dissolution of nickel hydroxide is:

Ni(OH)2(s) ⇌ Ni2+(aq) + 2 OH-(aq)

The expression for the solubility product constant (Ksp) is derived from this equation:

Ksp = [Ni2+][OH-]^2

Given that the Ksp of nickel hydroxide (Ni(OH)2) is 6.0 x 10^-16, and we want to achieve a Ni2+ concentration of 2.5 x 10^-3 M in equilibrium, we can set up an equation using the Ksp expression:

6.0 x 10^-16 = (2.5 x 10^-3)([OH-]^2)

Now, we can solve for [OH-] using algebraic methods:

[OH-]^2 = (6.0 x 10^-16) / (2.5 x 10^-3)
[OH-]^2 = 2.4 x 10^-13

Taking the square root of both sides, we get:

[OH-] = √(2.4 x 10^-13)
[OH-] = 4.9 x 10^-7 M

Now, to determine the required pH buffer solution, we need to calculate the pOH of the solution using the given hydroxide concentration.

pOH = -log[OH-]
pOH = -log(4.9 x 10^-7)
pOH ≈ 6.31

Next, we can use the pOH to determine the pH of the buffer solution using the equation:

pH = 14 - pOH
pH ≈ 14 - 6.31
pH ≈ 7.69

Therefore, a pH buffer solution with a pH of approximately 7.69 is needed to achieve a Ni2+ concentration of 2.5 x 10^-3 M in equilibrium with solid nickel hydroxide (Ni(OH)2), given that the Ksp is 6.0 x 10^-16.