Question

Given below are two statements:
Statement I: On passing HCl$_{(g)}$ through a saturated solution of BaCl$_2$, at room temperature white turbidity appears.
Statement II: When HCl gas is passed through a saturated solution of NaCl, sodium chloride is precipitated due to common ion effect.
In the light of the above statements, choose the most appropriate answer from the options given below:

• A. Statement I is correct but Statement II is incorrect
• B. Both Statement I and Statement II are incorrect
• C. Statement I is incorrect but Statement II is correct
• D. Both Statement I and Statement II are correct

Answer 1

The Correct Option is A

Evaluate the validity of the assertions by examining the solubility and precipitation of BaCl₂ and NaCl when exposed to HCl(g):
Step 1: Examine Assertion I Introducing HCl(g) into a saturated BaCl₂ solution increases the Cl⁻ ion concentration due to HCl dissociation. This elevated Cl⁻ concentration suppresses BaCl₂ solubility via the common ion effect, triggering BaCl₂ precipitation, evident as a white precipitate.
Assertion I is valid.
Step 2: Examine Assertion II Sodium chloride (NaCl) exhibits high solubility in water. The introduction of HCl(g) to a saturated NaCl solution does not induce precipitation, as the common ion effect does not substantially impact NaCl solubility under these circumstances.
Assertion II is invalid.
Step 3: Conclusion Based on the foregoing analysis: - Assertion I is valid, whereas Assertion II is invalid.
Final Answer: (1)