Respuesta :

maacastrobr

Answer:

Kb = 3.64x10⁻⁵

Explanation:

First we calculate the pOH of the solution:

  • pOH = 14 - pH
  • pOH = 2.18

Then we calculate [OH⁻]:

  • pOH = -log[OH⁻]
  • [OH⁻] = [tex]10^{-pOH}[/tex]
  • [OH⁻] = 0.0066 M

For a weak base solution with a relatively high concentration, we can use the following formula:

  • [OH⁻] = [tex]\sqrt{Kb*C}[/tex]

Where C is the concentration of the weak base solution (1.2 M in this case).

With the formula above we can calculate Kb:

  • 0.0066  = [tex]\sqrt{Kb*1.2}[/tex]
  • Kb = 3.64x10⁻⁵

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