Definition of $pH$ and $pOH$

Tutorial 2

        

Ionization of water, pH and pOH definition $ [\; ] $ Denotes molarity = concentration in mole per liter $ H_3O^+ $ is the hydronium ion $ OH^- $ is the hydroxide ion Ionization of water $ 2H_2O $ $ \leftrightarrows $ $H_3O^+ $ $ + $ $OH^- $ $ [H_3O^+] [OH^-] $ $ = $ $ 10^{-14} $ $ = $ $ K_e $ This relationship is valid both for pure water and for any dilute aqueous solution STP Definition of pH $pH$ $=$ $-log[H_3O^+]$ so: $[H_3O^+]$ $=$ $10^{-pH}$ Definition of pOH $pOH$ $=$ $-log[OH^-]$ so: $[OH^-]$ $=$ $10^{-pOH}$ Relation between pH and pOH $pOH$ $+$ $pOH$ $=$ $14$ This relationship holds for both pure water and any dilute aqueous solution STP

What is the value of the dissociation equilibrium constant K of water (considered as an acid) at 25^oC :

a) K = [ H₂O ] = 55.5 M b) K = K_e = 1.0 x 10^-14 c) K = K_e * [ H₂O ] = 5.6 x 10^-13 d) K = K_e / [ H₂O ] = 1,8 x 10^-16

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