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Registered Member #3883
Joined: Fri May 13 2011, 06:30PM
Location: Norway
Posts: 87
I don't think the titration examples are relevant for your experiment. In a titration the acid would be added very slowly to a basic bicarbonate solution, and CO2 will only be liberated once the pH has reached 7 (or slightly above). In your experiment you mix a strong acid and bicarbonate directly, so the pH would always be far below 7.
Randomsiences example with strong sulfuric acid is somewhat misleading, with very strong acids you get to a point where there virtually isn't any water left in the solution. The acid would initially attack the vessel just as a weak acid, but the lack of water prevents the reaction products (iron sulphate) from dissolving into the acid. So instead of dissolving the metal it is simply passivated with a thin layer of insoluble iron sulphate. This would be relevant for glacial acetic acid, but not dilute solutions like 1M.
As for dissociation of acids you'll need to read up on chemical equilibrium. This describes reactions that are reversible following a pattern like this: a + b <=> c + d
The dissociation of acetic acid will be : CH3COOH + H2O <=> CH3COO- + H3O+ Which can be generalized into AH + H2O <=> A- + H3O+
Strong acids will be shifted almost completely to the right, meaning all the acid will be disassociated. Weak acids will be shifted more to the left, meaning that most of the acid is present in the non-disassociated state. In reality the process is continual, meaning it will go back and forth between the two states continuously. The equilibrium is determined statistically by reaction rates in both directions. So a strong acid will react quickly from left to right, but very slowly from right to left, while a weak acid behaves in the opposite manner.
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Reaction between sodium bicarbonate and acetic acid