What is the result of adding KF to an equilibrium mixture of the weak acid HF?

\[ \text{HF(aq) ⇔ H}^+ \text{(aq) + F}^- \text{(aq)} \]

A. \(\text{F}^- \) concentration decreases
B. The dissociation constant, \( K \), increases
C. \(\text{HF} \) concentration decreases
D. \(\text{H}^+ \) concentration decreases

Answer D. Follow Le Chatelier's principle.

Answered by Yipes | 2024-06-10

When gaseous hydrogen chloride is passed through a sodium chloride solution, precipitation of the** sodium chloride** occurs as a result of an excess of chloride ions in the solution (caused by the dissociation of HCl). Here the **concentration **of H⁺ decreases. The correct option is D .
What is common-ion effect?
When another electrolyte (which includes an ion that is also present in the first electrolyte, i.e., a common ion) is added, the **common ion effect **suppresses the ionisation of the first electrolyte. It is thought to be a result of Le Chatlier's principle , often known as the equilibrium law.
An increase in the concentration of one of the ions dissociated in the solution by the addition of another species containing the same ion will result in an increase in the degree of association of ions in a solution where there are several species associating with each other via a chemical equilibrium process.
Here the common ion 'F' in KF supresses the dissociation of HF.
Thus the correct option is D .
To know more about** common ion effect**, visit;
https://brainly.com/question/30772969
#SPJ3

Answered by nidhivaishnav | 2024-06-17

Adding KF to an equilibrium mixture of HF increases the concentration of fluoride ions, which shifts the equilibrium to the left, resulting in a decrease in the concentrations of both H F and H + . The best answer to the question is option C, stating that the concentration of H F decreases. Option D is also applicable as H + concentration decreases.
;

Answered by nidhivaishnav | 2024-10-02