Which of the following will increase the percent of HF that...

Which of the following will increase the percent of HF that is converted to the fluoride ion in water?
$$
\begin{array}{l}{\text { (a) addition of NaOH }} \\ {\text { (b) addition of } \mathrm{HCl}} \\ {\text { (c) addition of } \mathrm{NaF}}\end{array}
$$

Key Concepts

Common Ion Effect

The common ion effect is the shift in equilibrium that occurs when an ion common to the equilibrium is added to the solution. In acid-base equilibria, adding a salt that contains either the conjugate acid or conjugate base can suppress the dissociation of the weak acid or weak base, influencing the overall percent conversion within the system.

Acid-Base Equilibrium

Acid-base equilibrium concerns the balance between acids and bases in a solution, particularly the dissociation of weak acids. In aqueous solutions, weak acids like HF do not fully dissociate, and the equilibrium expression helps determine the concentrations of the acid and its conjugate base under various conditions.

Chemical Equilibrium

Chemical equilibrium involves the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. Understanding equilibrium is crucial when analyzing how changes to the system, such as adding or removing substances, will shift the balance of the reaction.

Le Chatelier's Principle

Le Chatelier's Principle states that if an external change is imposed on a system at equilibrium, the system will adjust itself to partially counteract that change and re-establish equilibrium. This principle is key to predicting the direction in which the reaction will shift when additional substances are introduced to the system.

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