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10 questions from this quiz
Kw=[H+][OH−]K_w = [\text{H}^+][\text{OH}^-]Kw=[H+][OH−]
1.00×10−141.00 \times 10^{-14}1.00×10−14 mol² dm⁻⁶
mol² dm⁻⁶
KwK_wKw increases
They are equal
[H+]=Kw[\text{H}^+] = \sqrt{K_w}[H+]=Kw
Far to the left
pH decreases slightly
It fully dissociates
[H+]=Kw[OH−][\text{H}^+] = \frac{K_w}{[\text{OH}^-]}[H+]=[OH−]Kw
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