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Chapter 15: Problem 63

To which side does the dissociation equilibrium lie for a strong electrolyte? For a weak electrolyte?

Short Answer

Expert verified
For strong electrolytes, the dissociation equilibrium lies far to the right, favoring dissociation into ions. For weak electrolytes, the dissociation equilibrium lies more to the left, favoring the undissociated compound.

Step by step solution

01

Definition of Strong Electrolytes

Strong electrolytes are compounds that dissociate completely into ions when dissolved in water. In other words, they separate into their ionic components when dissolved in a solution. Common examples of strong electrolytes are salts (like NaCl) and strong acids (like HCl) or bases (like KOH).
02

Definition of Weak Electrolytes

Weak electrolytes are compounds that partially dissociate into ions when dissolved in water. This means that when they dissolve in a solution, a significant portion of the molecules remain intact and do not separate into their ionic components. Weak electrolytes are usually weak acids (like acetic acid, CH₃COOH) or weak bases (like ammonia, NH₃).
03

Dissociation Equilibrium for Strong Electrolytes

For a strong electrolyte, the dissociation is nearly complete when it dissolves in a solution. As a result, there is a negligible amount of the undissociated compound in the solution, and the dissociation equilibrium lies far to the right. In other words, the concentration of the ions formed is much greater than the concentration of the undissociated molecules, so the equilibrium favors dissociation.
04

Dissociation Equilibrium for Weak Electrolytes

For a weak electrolyte, the dissociation is partial when it dissolves in a solution, which means that a significant fraction of the compound remains undissociated in the solution. Consequently, the dissociation equilibrium for weak electrolytes lies to the left, favoring the undissociated compound rather than the dissociated ions. In summary, the dissociation equilibrium of strong electrolytes lies far to the right (favoring dissociation), while the equilibrium of weak electrolytes lies more to the left (favoring the undissociated compound).

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Most popular questions from this chapter

Write the mathematical definition of \(\mathrm{pH}\), and explain what fundamental change there would be in the pH scale if you left the negative out.

Write the mathematical expression that allows you to solve for the \(\mathrm{OH}^{-}\) concentration in water when you know only the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration.

Indicate whether each compound is an electrolyte or a nonelectrolyte in water: (a) \(\mathrm{N}_{2}\) (b) \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) (c) \(\mathrm{HI}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) (propane) (e) \(\mathrm{Li}_{3} \mathrm{PO}_{4}\) (f) \(\mathrm{AgNO}_{3}\) (g) \(\mathrm{CCl}_{4}\)

An aqueous solution has an \(\mathrm{H}_{3} \mathrm{O}\) ' concentration of \(1.0 \mathrm{M}\). What is the OH concentration? Is this solution acidic or basic? Justify your answer.

Perchloric acid, \(\mathrm{HClO}_{4}\), is a strong acid. (a) Write the chemical equation for the reaction between perchloric acid and water. (b) List all species present in an aqueous solution of perchloric acid in order of concentration, highest to lowest. (c) Calculate the concentration of all species (except \(\mathrm{H}_{2} \mathrm{O}\) ) present in a \(0.100 \mathrm{M} \mathrm{HClO}_{4}\) solution. (d) What is the \(\mathrm{pH}\) of this solution?
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