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Originally Posted by elias
shouldn t calcium carbonate start to dessolve in a liquid sustance that at low ph
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Well, you'd think it would...
Maybe this explaind it..
"Acetic acid is classified as a weak acid, because it does not completely dissociate into its component ions when dissolved in aqueous solution. At a concentration of 0.1 M, only about 1% of the molecules are ionized. In solution, there is a dynamic equilibrium between the neutral molecules and the acetate and hydronium ions."
What this tells us (if my chemistry is intact) is that in aqueous solution, this weak acid only contibutes modestly to the overall [H+] and therefore does not react strongly with the CaCO3. You may see a proportionaltely greater amount of dissolution if you do not mix the acid with water. Be aware though, that acetic acid can burn your skin and appropriate precautions should be taken before testing this
Disclaimer: It's been some time since chem class
