# Compare the solubility of cobalt(II) carbonate in each of the following aqueous solutions:Clear All0.10 M Co(CH;C00)2More soluble than in purewater.0.10 M (NH4)½CO3Similar solubility as in purewater.0.10 M KCH;CO0Less soluble than in purewater.0.10 M NH,NO3 Compare the solubility of cobalt(II) sulfide in each of the following aqueous solutions:Clear All0.10 M Co(NO3)2More soluble than in purewater.0.10 M K2SSimilar solubility as in purewater.0.10 M KCH;CO0Less soluble than in purewater.0.10 M NH4NO3

Question
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The Ksp for Cobalt carbonate is : 8.0 × 10-13

Ksp for colbat sulfide is :

 CoS 5.9 × 10-21
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Step 1

Common ion effect can be defined as the decrease in solubility of a sparingly soluble salt when a solution of common ion added to it.

This can be explained based on Lechatleir's principle when a system at equilibrium is subjected to a change in tempearture, concentration or pressure of gaseous substrates ,then the equilibrium will shift in such a direction that it nullifies the change.

ex:

AmXn (s) <=> An+ (aq) + Xm- (aq)

when An+ ions are added to the above system,then concentration on right side increases and it shifts the equilibrium towards left side.

Hence, the solubility of the salt AmXdecreases.

Step 2

Given,

Cobalt carbonate is a sparingly soluble salt.

When 0.1M Co(CH3COO)2 is added, then the solubility of CoCO3 salt further decreases due to common ion effect.

When 0.1M (NH4)2CO3 is added, then the solubility of CoCO3 salt further decreases due to common ion effect.

When 0.1M K(CH3COO) is added, then there is no change in...

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