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Water molecules react to form H3O+H_3O^+H3O+ and OH−OH^-OH− ions
Hydronium ion (H3O+H_3O^+H3O+) and hydroxide ion (OH−OH^-OH−)
Dynamic equilibrium
Ionic product of water / equilibrium constant
Kw=[H+][OH−]K_w = [H^+][OH^-]Kw=[H+][OH−]
1.0×10−141.0 \times 10^{-14}1.0×10−14 mol2^22 dm−6^{-6}−6
They are equal
1.0×10−71.0 \times 10^{-7}1.0×10−7 mol dm−3^{-3}−3
7
KwK_wKw increases as temperature increases
Self-ionisation is endothermic
Yes, remains neutral because [H+][H^+][H+] still equals [OH−][OH^-][OH−]
pH=−log[H+]\text{pH} = -\log[H^+]pH=−log[H+]
[H+]=Kw[H^+] = \sqrt{K_w}[H+]=Kw
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