Multiple Choice
What is the ion product constant (Kw) of pure water at 50.0°C, if the pH is 6.630?
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17. Acid and Base Equilibrium
Auto-Ionization
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What are the products formed when water undergoes auto-ionization?
A
H2 and O2
B
H3O+ and OH-
C
H+ and O2-
D
H+ and H2O
Verified step by step guidance1
Understand that auto-ionization of water is a process where two water molecules react with each other to produce ions.
Write the chemical equation for the auto-ionization of water: \(\mathrm{2\ H_2O (l) \rightleftharpoons H_3O^+ (aq) + OH^- (aq)}\).
Recognize that one water molecule donates a proton (H\(^+\)) to another water molecule, forming a hydronium ion (H\(_3\)O\(^+\)) and a hydroxide ion (OH\(^-\)).
Note that the products are not elemental hydrogen (H\(_2\)) or oxygen (O\(_2\)), nor are they free protons (H\(^+\)) alone or oxide ions (O\(^{2-}\)).
Conclude that the correct products of water auto-ionization are hydronium ions (H\(_3\)O\(^+\)) and hydroxide ions (OH\(^-\)).
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