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STATEMENT-1: HCl is a strong acid and tr...

STATEMENT-1: HCl is a strong acid and true electrolyte.
STATEMENT-2: Liquid HCl is bad conductor of electricity.

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-12

B

Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-12

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False, Statement-2 is True

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the two statements regarding HCl, we will evaluate each statement step by step. ### Step 1: Evaluate Statement 1 **Statement 1:** HCl is a strong acid and true electrolyte. - **Explanation:** HCl (hydrochloric acid) is indeed a strong acid. This means that when HCl is dissolved in water, it completely dissociates into its ions: \[ \text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- \] This complete dissociation is characteristic of strong acids. Therefore, the first part of the statement is true. - **True Electrolyte:** However, the term "true electrolyte" refers to substances that exist as ions in their pure state. HCl in its pure form (gaseous state) does not exist as ions; it exists as neutral molecules. Therefore, while HCl behaves as an electrolyte when dissolved in water, it is not a "true electrolyte" in its pure state. **Conclusion for Statement 1:** The first statement is **false** because HCl is not a true electrolyte in its pure state. ### Step 2: Evaluate Statement 2 **Statement 2:** Liquid HCl is a bad conductor of electricity. - **Explanation:** Liquid HCl, when in its pure form, does not contain free ions because it exists as neutral molecules. Since electrical conductivity in liquids is primarily due to the presence of free-moving charged particles (ions), a liquid that does not contain these charged particles will not conduct electricity well. Therefore, liquid HCl is indeed a bad conductor of electricity. **Conclusion for Statement 2:** The second statement is **true** because liquid HCl does not conduct electricity effectively due to the lack of free ions. ### Final Conclusion - **Statement 1:** False (HCl is a strong acid but not a true electrolyte in its pure state). - **Statement 2:** True (Liquid HCl is a bad conductor of electricity). ### Answer The correct option is **D**: Statement 1 is false, and Statement 2 is true. ---
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