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10 questions from this quiz
They only partially dissociate
An equilibrium
They are formed in equal quantities
Ka=[H+]2[HA]K_\text{a} = \frac{[\text{H}^+]^2}{[\text{HA}]}Ka=[HA][H+]2
[H+]=Ka×[HA][\text{H}^+] = \sqrt{K_\text{a} \times [\text{HA}]}[H+]=Ka×[HA]
When pH is greater than 6
When Ka>10−2K_\text{a} > 10^{-2}Ka>10−2 mol dm−3^{-3}−3
10−710^{-7}10−7 mol dm−3^{-3}−3
Prepare standard solution and measure pH
[H+]=10−pH[\text{H}^+] = 10^{-\text{pH}}[H+]=10−pH
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