Problem: In water, the equilibrium 2H2O(l) ⇌ H3O+ (aq) + OH−(aq)      Kc = 10−14 determines the concentrations of H3O+(aq) and OH -(aq). If the pH is 9.2, what is the OH - concentration? (note H3O+(aq) and H+(aq) are equivalent ways of representing a solvated proton and pH = -log[H+(aq)].) a) 9.76x10−6 b) 2.31x10−5 c) 3.88x10−4 d) 1.58x10−5 e) 2.54x10−6

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In water, the equilibrium

2H2O(l) ⇌ H3O+ (aq) + OH(aq)      Kc = 10−14

determines the concentrations of H3O+(aq) and OH -(aq). If the pH is 9.2, what is the OH - concentration? (note H3O+(aq) and H+(aq) are equivalent ways of representing a solvated proton and pH = -log[H+(aq)].)

a) 9.76x10−6

b) 2.31x10−5

c) 3.88x10−4

d) 1.58x10−5

e) 2.54x10−6

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