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Chapter 16: Problem 35

Predict the direction that predominates in this reaction: $$\mathrm{F}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HF}(a q)+\mathrm{OH}^{-}(a q)$$

Short Answer

Expert verified
The reaction primarily proceeds from right to left, towards the reactants.

Step by step solution

01

Identify the reactants and products

The reactants are fluoride ion (\(F^-\)) and water (\(H_2O\)). The products are hydrofluoric acid (\(HF\)) and hydroxide ion (\(OH^-\)).
02

Understand the acid-base properties

Fluoride ion (\(F^-\)) is the conjugate base of \(HF\) and \(OH^-\) is the conjugate base of \(H_2O\). In terms of acidity, \(HF\) is a weak acid and \(H_2O\) is even weaker (practically neutral). When comparing the basicity, \(F^-\) is a weak base while \(OH^-\) is a strong base.
03

Apply Le Chatelier's Principle

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system responds by opposing the change to reach a new equilibrium. Since \(OH^-\) is a stronger base than \(F^-)\), it would be expected for the reaction to shift to the left to minimize the effect, favoring the reactants. This is due to the fact that the position of equilibrium will shift towards the weaker acid-base pair to minimize the change.
04

Predict the reaction direction

Based on the principles described, in this reaction, the equilibrium lies to the left, in favor of the reactants. Therefore, the reaction primarily proceeds from right to left.

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Most popular questions from this chapter

Prove the statement that when the concentration of a weak acid HA decreases by a factor of 10 , its percent ionization increases by a factor of \(\sqrt{10}\). State any assumptions.

Define \(\mathrm{pH}\). Why do chemists normally choose to discuss the acidity of a solution in terms of \(\mathrm{pH}\) rather than hydrogen ion concentration, \(\left[\mathrm{H}^{+}\right] ?\)

Compare the strengths of the following pairs of acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SeO}_{4},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\).

Identify the acid-base conjugate pairs in each of these reactions: (a) \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{HCN} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CN}^{-}\) (b) \(\mathrm{HCO}_{3}^{-}+\mathrm{HCO}_{3}^{-} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}+\mathrm{CO}_{3}^{2-}\) (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{NH}_{4}^{+}\) (d) \(\mathrm{HClO}+\mathrm{CH}_{3} \mathrm{NH}_{2} \rightleftharpoons \mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{ClO}^{-}\) (e) \(\mathrm{CO}_{3}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-}\) (f) \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-}\)

Prediet the \(\mathrm{pH}(>7,<7,\) or \(\approx 7)\) of the aqueous solutions containing the following salts: (a) \(\mathrm{KBr}\) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (c) \(\mathrm{BaCl}_{2}\) (d) \(\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}\).
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