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Sagot :
Answer:
Ka = 3.45x10⁻⁶
Explanation:
First we calculate [H⁺], using the given pH:
- pH = -log[H⁺]
- [H⁺] = [tex]10^{-pH}=10^{-5.6}[/tex]
- [H⁺] = 2.51x10⁻⁶ M
To solve this problem we can use the following formula describing a monoprotic weak acid:
- [H⁺] = [tex]\sqrt{C*Ka}[/tex]
We input the data that we already know:
- 2.51x10⁻⁶ = [tex]\sqrt{0.530*Ka}[/tex]
And solve for Ka:
- Ka = 3.45x10⁻⁶
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