Given below are two statements:
Statement I: On passing through a saturated solution of , 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 through a saturated solution of , 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✓ Correct
- (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: (A)
Solution
Passing HCl gas into a saturated solution of sharply raises the concentration; this pushes the dissolution equilibrium in the solid's favour (common-ion effect) and precipitates out, seen as a white turbidity — Statement I is correct.
Statement II makes the same claim for a saturated NaCl solution, but this is not the standard textbook demonstration of the common-ion effect for chlorides — passing HCl gas through saturated NaCl solution is not observed to precipitate NaCl the way it does with under the same simple conditions, so Statement II is not correct as stated.
Statement II makes the same claim for a saturated NaCl solution, but this is not the standard textbook demonstration of the common-ion effect for chlorides — passing HCl gas through saturated NaCl solution is not observed to precipitate NaCl the way it does with under the same simple conditions, so Statement II is not correct as stated.
JEE Main · 2024 · 05 Apr 2024 · Shift 2 · Single correct option