Final answer:
The pOH of a 0.0337 M KOH solution is approximately 1.47, indicating that the solution is basic because the pOH is less than 7.
Step-by-step explanation:
To find the pOH of a 0.0337 M KOH solution, we first recognize that KOH is a strong base and dissociates completely in water. This means that the concentration of hydroxide ions, OH-, will be equal to the concentration of KOH, which is 0.0337 M. The pOH is calculated using the formula pOH = -log[OH-]. Therefore, pOH = -log(0.0337) which approximately equals 1.47.
To determine if the solution is acidic, neutral, or basic, we can use the pOH and pH relationship: pH + pOH = 14. If the pH is greater than 7, the solution is basic. Since the pOH is less than 7, we can infer that the pH is greater than 7 without calculating it explicitly, categorizing this solution as basic.
The solution represented by the beaker in the diagram is an acid-base solution. In this solution, the beaker contains many pale blue balls and 3 purple balls, which represent pale blue and purple ions respectively. The key provides information about the acid-base pairs and their conjugate forms, indicating that the solution involves the transfer of hydrogen ions (H+). In the diagram, the pale blue ball labeled with H+ represents the acid and the pale blue ball labeled with OH- represents the conjugate base. Therefore, the beaker represents an acid solution.