Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which fluorine-containing species are present in solution. HF(g)+H2O(l)H3O+(aq)+F−(aq) $$Ka=1.10×10−3 Is fluoride in pH 7.00 drinking water more likely to be present as F–(aq) or HF2–(aq)? Choose one: F- (aq) HF2- (aq) What is the equilibrium constant for this equilibrium? 2HF(g)+H2O(l)H3O+(aq)+HF−2(aq)
Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which fluorine-containing species are present in solution. HF(g)+H2O(l)H3O+(aq)+F−(aq) $$Ka=1.10×10−3 Is fluoride in pH 7.00 drinking water more likely to be present as F–(aq) or HF2–(aq)? Choose one: F- (aq) HF2- (aq) What is the equilibrium constant for this equilibrium? 2HF(g)+H2O(l)H3O+(aq)+HF−2(aq)
Chemistry by OpenStax (2015-05-04)
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Chapter15: Equilibria Of Other Reaction Classes
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Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which fluorine-containing species are present in solution.
HF(g)+H2O(l)H3O+(aq)+F−(aq) $$Ka=1.10×10−3
Is fluoride in pH 7.00 drinking water more likely to be present as F–(aq) or HF2–(aq)?
Choose one:
F- (aq)
HF2- (aq)
What is the equilibrium constant for this equilibrium?
2HF(g)+H2O(l)H3O+(aq)+HF−2(aq)
Ka=
What is the equilibrium concentration of HF2– in a 0.110 M solution of HF?
M [HF2-]eq
M [HF2-]eq
What is the pH at equilibrium of a 0.110M solution of HF?
= pH
= pH
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