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:
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:
- Statement I is correct but Statement II is incorrect
- Both Statement I and Statement II are incorrect
- Statement I is incorrect but Statement II is correct
- Both Statement I and Statement II are correct
The Correct Option is A
Approach Solution - 1
To determine the correctness of the statements, consider the solubility and precipitation behavior of BaCl2 and NaCl in the presence of HCl(g):
Step 1: Analyze Statement I When HCl(g) is bubbled through a saturated solution of BaCl2, the concentration of Cl− ions increases significantly due to the dissociation of HCl. The increased Cl− ions reduce the solubility of BaCl2 through the common ion effect, causing the precipitation of BaCl2 as white turbidity.
Statement I is correct.
Step 2: Analyze Statement II Sodium chloride (NaCl) is highly soluble in water. Passing HCl(g) through a saturated solution of NaCl does not lead to precipitation because the solubility of NaCl is not significantly affected by the common ion effect under these conditions.
Statement II is incorrect.
Step 3: Conclusion From the above analysis: - Statement I is correct, but Statement II is incorrect.
Final Answer: (1)
Approach Solution -2
Statement I: On passing HCl(g) through a saturated solution of BaCl₂ at room temperature, white turbidity appears.
Explanation: Passing HCl gas into a saturated BaCl₂ solution leads to the formation of insoluble BaCl₂·2H₂O crystals due to a decrease in solubility. The appearance of white turbidity confirms this precipitation.
Hence, Statement I is correct.
Step 2: Analyze Statement II.
Statement II: When HCl gas is passed through a saturated solution of NaCl, sodium chloride is precipitated due to the common ion effect.
Explanation: NaCl is already highly soluble in water, and adding HCl gas does not lead to precipitation. Instead, it increases the solubility of NaCl because of hydration effects. Thus, NaCl is not precipitated under these conditions.
Hence, Statement II is incorrect.
Step 3: Conclusion.
Statement I is correct but Statement II is incorrect.
Final Answer: Statement I is correct but Statement II is incorrect.
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