Acids increase the concentration of what in water? H+ ions hydrate ions hydroxide ions OH- ions
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Answer:
H+ ions...
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Answer:
Water dissociation (autoionization; self-ionization) occurs endothermically d due to electric field fluctuations between neighboring molecules. Dipole librations [191], resulting from thermal effects and favorable localized hydrogen bonding, [567] together with nuclear quantum effects [2025], cause these fluctuations. The process may be facilitated by exciting the O-H stretch overtone vibration [393]. Once formed (at an average concentration of about 1 M H2O-H+···OH- [1984]),h the ions may separate by means of the Grotthuss mechanism but normally (>99.9%) rapidly recombine (≈ 20 ps [2171]) with a frequency in the terahertz range. Rarely (about once every eleven hours per molecule at 25 °C, or less than once a week at 0 °C), the localized hydrogen bonding arrangement breaks before allowing the separated ions to return [191]. The pair of ions (H+, OH-)g hydrate independently and continue their separate existence a for about 70 μs (this lifetime also dependent on the extent of hydrogen-bonding, being shorter at lower temperatures). They tend to recombine when separated by only one or two water molecules.
H2O equilibrium arrows H+ + OH-
Kw = [H+] ˣ [OH-]
Kw is a dimensionless number (= 13.995 ; 25 °C [IAPWS]) as the included concentrations are relative to the molal standard states (e.g., 1 mol ˣ Kg-1). n This low occurrence of the ions means that at neutrality (pH 7 at 25 °C) c, similarly charged ions are, on average, separated by vast distances (≈ 0.255 μm) in molecular terms and (for example) bacteria contain only a few tens of free hydrogen ions (~ 30 in an Escherichia coli). Contributing to this effect are the high dielectric constant (encouraging charge separation) and high concentration of H2O (≈ 55.5 M; increasing the absolute amount dissociated). The mean lifetime of a hydroxonium ion (1 ps; about the same as that of a hydrogen bond) is such that the charge could be associated with over 107 molecules of water before neutralization.
Although the extent of dissociation is tiny ([H+]/[H2O] = 2.8 ˣ 10-9 at 37 °C), the dissociation and consequential changes in the tiny concentrations of hydrogen ions have absolute importance to living processes. Hydrogen and hydroxyl ions are produced already hydrated.
H2O (liq) equilibrium arrows H+(aq) + OH- (aq)
where the subscripts 'liq' and ‘aq’ indicate that the species are in or within the aqueous liquid phase. l
Hydration enthalpies of protons and hydroxides,