Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+ (aq) a.Suppose a strong base (OH-) is added to the buffer system above. Which two species could react and why? b.Write the chemical reaction for the reaction of hydroxide ion (OH-) being neutralized by reacting with the hydrofluoric acid. c.Explain why the addition of a small amount of strong base will not cause a significant change in the pH of the solution as long as the HF is not used up. d. Suppose a strong acid (H3O+) is added to the buffer system above. Which species could react and why? e.Write the chemical reaction for the reaction of hydronium ion (H3O+) being neutralized by reacting with the fluoride ion. f.Explain why the addition of a small amount of strong acid will not cause a significant change in the pH of the solution as long as the fluoride ion (F ̄) is not used up.
Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+ (aq)
a.Suppose a strong base (OH-) is added to the buffer system above. Which two species could react and why?
b.Write the
c.Explain why the addition of a small amount of strong base will not cause a significant change in the pH of the solution as long as the HF is not used up.
d. Suppose a strong acid (H3O+) is added to the buffer system above. Which species could react and why?
e.Write the chemical reaction for the reaction of hydronium ion (H3O+) being neutralized by reacting with the fluoride ion.
f.Explain why the addition of a small amount of strong acid will not cause a significant change in the pH of the solution as long as the fluoride ion (F ̄) is not used up.
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