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Sagot :
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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