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10 questions from this quiz
Only slightly
Relatively few H+\text{H}^+H+ ions
A quantitative measure of strength
A stronger weak acid
A weaker acid with less dissociation
Ka=[H+][A−][HA]K_a = \frac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}Ka=[HA][H+][A−]
Concentration of hydrogen ions
Concentration of the conjugate base
Concentration of undissociated acid
Values are often very small
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