Of the species below, only electrolyte: is not an Select one: 0 A Ar B. HCI C KOH D. NaCl E Rb2SO4
The Correct Answer and Explanation is:
The correct answer is: A. Ar
Explanation:
Among the listed species:
- A. Ar (Argon)
- B. HCl (Hydrochloric acid)
- C. KOH (Potassium hydroxide)
- D. NaCl (Sodium chloride)
- E. Rb₂SO₄ (Rubidium sulfate)
The question asks which of these is not an electrolyte.
What is an Electrolyte?
An electrolyte is a substance that produces ions when dissolved in water, allowing the solution to conduct electricity. Electrolytes can be:
- Strong electrolytes: Completely dissociate in water (e.g., NaCl, HCl, KOH).
- Weak electrolytes: Partially dissociate (e.g., acetic acid).
- Non-electrolytes: Do not produce ions in solution (e.g., sugar, ethanol).
Analysis of Each Option:
- A. Argon (Ar):
- Argon is a noble gas, chemically inert.
- It does not ionize in water.
- It does not conduct electricity.
- Therefore, not an electrolyte.
- B. HCl (Hydrochloric Acid):
- A strong acid.
- Dissociates completely in water:
HCl→H++Cl−\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^-HCl→H++Cl− - Conducts electricity well → Electrolyte.
- C. KOH (Potassium Hydroxide):
- A strong base.
- Fully dissociates:
KOH→K++OH−\text{KOH} \rightarrow \text{K}^+ + \text{OH}^-KOH→K++OH− - Strong electrolyte.
- D. NaCl (Sodium Chloride):
- Ionic salt, dissolves in water:
NaCl→Na++Cl−\text{NaCl} \rightarrow \text{Na}^+ + \text{Cl}^-NaCl→Na++Cl− - Strong electrolyte.
- Ionic salt, dissolves in water:
- E. Rb₂SO₄ (Rubidium Sulfate):
- An ionic compound, dissolves into:
Rb2SO4→2Rb++SO42−\text{Rb}_2\text{SO}_4 \rightarrow 2\text{Rb}^+ + \text{SO}_4^{2-}Rb2SO4→2Rb++SO42− - Strong electrolyte.
- An ionic compound, dissolves into:
Conclusion:
All options except Argon (Ar) are substances that dissociate into ions in water, making them electrolytes.
Therefore, the correct answer is:
A. Ar – the only one that is not an electrolyte.
