Examine the activity series given below.
-Examine the following image. Assume the solution in the beaker is a buffer solution. What is the pOH of the solution in the beaker?

Question

Examine the activity series given below.

-Examine the following image. Assume the solution in the beaker is a buffer solution. Examine the activity series given below. -Examine the following image. Assume the solution in the beaker is a buffer solution. What is the pOH of the solution in the beaker? A) 9.67 B) 14.00 C) 2.13 × 10<sup>-10</sup> D) 4.68 × 10<sup>-5</sup>

What is the pOH of the solution in the beaker?

Quizplus · Accepted Answer

Since the solution is a buffer solution, we can assume it contains a weak acid and its conjugate base (or a weak base and its conjugate acid). The pH of the solution is given as 4.67, so we can calculate the [H+] concentration as 10^-4.67 = 2.14 x 10^-5 M.

To find the pOH, we can use the equation:

pH + pOH = 14

pOH = 14 - pH = 14 - 4.67 = 9.33

However, since the solution is a buffer, we also need to consider the equilibrium between the weak acid and its conjugate base (or weak base and its conjugate acid). The Henderson-Hasselbalch equation tells us that:

pH = pKa + log([A-]/[HA])

where pKa is the dissociation constant of the weak acid, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid.

Since the solution is a buffer, we can assume that the concentrations of the weak acid and its conjugate base are roughly equal. Therefore, we can simplify the equation to:

pH = pKa + log(1)

pH = pKa

Since we don't have information about the specific weak acid and its dissociation constant, we can't calculate the exact pKa. However, we can use the activity series given to make an educated guess about the identity of the weak acid.

The activity series tells us that H2CO3 is a stronger acid than H2SO3. Therefore, if the solution in the beaker contains H2CO3 and its conjugate base (HCO3-), we can assume that H2CO3 will donate a proton to water to a greater extent than H2SO3. This would result in a lower pH and a higher pOH than if the solution contained H2SO3 and its conjugate base (HSO3-).

Therefore, we can eliminate answer choices B and C, since a pOH of 14.00 or below 1 would be extremely basic and unlikely in a buffer solution.

Answer choice D is also unlikely, since a pOH of 4.68 x 10^-5 would correspond to a pH of 13.9995, which is again extremely basic.

Therefore, the best choice is answer choice A, which gives a pOH of 9.67.

Examine the Activity Series Given Below