#Ca^+2(aq)# + #Co3^-2(aq)rightleftharpoons # #CaCo3(S)# the amount of dissolved Caco3 can be increased on adding a.#Caco3(s)# b.#KNo3(s)# c.#Na2Co3(s)# d.#CH3Co oH(s)# #?#

1 Answer
anor277
May 20, 2018

Would it not be #d.#?

Explanation:

We gots the solubility equilibrium....

#Ca^(2+) + CO_3^(2-)rightleftharpoonsCaCO_3(s)#

And we could address this equilibrium quantitatively had we #K_"sp"# for calcium carbonate.....the addition of SOLID calcium carbonate will have no effect on the equilibrium...the addition of potassium nitrate will no effect...the addition of SOLUBLE sodium carbonate will drive the equilibrium to the RIGHT as we face the page....

However, the addition of acetic acid will likely result in the reaction...

#H_3C-CO_2H + CO_3^(2-) rarr H_3C-CO_2^(-) + HCO_3^(-)#

...and so #[CO_3^(2-)]# will be REDUCED...and the solubility equilibrium should be driven to the left...

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