Chemistry Equilibrium ETEA 2023
PMDC Verified Question 39 of 102
If ionic product is less than \( K_{sp} \) then:
A
Solution will be saturated
B
Precipitation will occur
C
Solution will be super saturated
D
No precipitation will occur
Tap any option to test your recall and reveal the step-by-step Propolis autopsy.

Propolis Cognitive Error Autopsy

Official Correct Choice:
Option D: No precipitation will occur
Concept:

The relationship between the ionic product (\( Q_{sp} \)) and the solubility product (\( K_{sp} \)) dictates whether a solution can hold more dissolved ions or if it will precipitate.

Formula:

$$ \text{If } Q_{sp} < K_{sp} \implies \text{Unsaturated Solution} $$

Solution:

  • \( K_{sp} \) is the maximum equilibrium threshold for dissolved ions.


  • When the actual ionic product (\( Q_{sp} \)) is less than \( K_{sp} \), the solution has not yet reached its maximum capacity.


  • This describes an unsaturated solution. Because there is room for more solute to dissolve, no precipitation will occur.


Why other options are incorrect:

Saturated means \( Q_{sp} = K_{sp} \). Supersaturated (leading to precipitation) means \( Q_{sp} > K_{sp} \).

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