Which of the following types of compounds are considered strong electrolytes in aqueous solutions? Select all that apply. A. All ionic compounds B. Strong acids C. Strong bases D. Weak acids E. Weak bases F. Soluble molecular compounds G. Soluble ionic compounds
The correct answer and explanation is:
The correct answers are:
- B. Strong acids
- C. Strong bases
- G. Soluble ionic compounds
Explanation:
An electrolyte is a substance that, when dissolved in water, dissociates into ions and can conduct electricity. The strength of an electrolyte depends on how completely it dissociates into ions in solution.
- Strong acids (B) are considered strong electrolytes because they completely dissociate into hydrogen ions (H⁺) and their corresponding anions in water. For example, hydrochloric acid (HCl) dissociates fully in water: HCl→H++Cl−\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- This complete dissociation allows strong acids to conduct electricity efficiently.
- Strong bases (C) are also strong electrolytes as they dissociate completely in water to form hydroxide ions (OH⁻) and their corresponding cations. An example is sodium hydroxide (NaOH): NaOH→Na++OH−\text{NaOH} \rightarrow \text{Na}^+ + \text{OH}^- Since strong bases dissociate fully, they too can conduct electricity well in aqueous solutions.
- Soluble ionic compounds (G) dissociate into their constituent ions when dissolved in water, making them strong electrolytes. For example, sodium chloride (NaCl) dissociates as follows: NaCl→Na++Cl−\text{NaCl} \rightarrow \text{Na}^+ + \text{Cl}^- These compounds conduct electricity effectively because of the free movement of ions.
The following options are not considered strong electrolytes:
- A. All ionic compounds: Not all ionic compounds are strong electrolytes. Some ionic compounds, like lead(II) chloride (PbCl₂), are poorly soluble in water and do not dissociate significantly, so they are weak electrolytes.
- D. Weak acids: Weak acids, such as acetic acid (CH₃COOH), only partially dissociate in water. This partial dissociation results in fewer ions in solution, so weak acids are weak electrolytes.
- E. Weak bases: Weak bases, like ammonia (NH₃), also partially dissociate in water, producing fewer ions. Therefore, they are weak electrolytes.
- F. Soluble molecular compounds: Molecular compounds, like sugar (C₆H₁₂O₆), do not dissociate into ions in water. Since they don’t produce ions, they cannot conduct electricity and are not considered electrolytes.
In summary, strong electrolytes include strong acids, strong bases, and soluble ionic compounds, as they all fully dissociate into ions in solution.