8 -Chem. Eq Chemical Equilibrium Record All Data and observations Here brium I.

Question

8 -Chem. Eq Chemical Equilibrium Record All Data and observations Here brium I. studying the Dissociation HC HolAS Wal color of original equilibrium mixture color change after addition ofNaCHson: oran color change after heating mixture sama, Yellow color change after cooling mixture: Orange IL ng the IC MCoguzo briu color of original equilibrium mixture: Purple color change after addition of distilled water: color change after addition of 12MHCI: color change after addition of distilled water: color change after heating mixture: dark blue color change after cooling mixture: LIL. udying the tion of NH4CI in Water Equilibrium initial appearance of equilibrium mixture: u change after addition of 1 white rero at beth m ckov un eating mixture for34 minutes: change a clear t wa at initial appearenu

Explanation / Answer

Ans 1;- The chemical equation for the dissociation of HC2H3O2 + H2O -> H3O+ + C2H3O2-

Ans 2:- The solution colour is rotten pink which indicates that H3O+ concentration in the initial equilibrium mixture is relatively high,because the concentration of H3O+ required to shift the equilibrium differs for different indicators.Here H3O+ is greater than 10-4 , so it is relatively high.

Ans 3. After addition of sodium acetate NaC2H3O2 , the colour of the equilibrium mixture has changed to orange. The added salt sodium acetate has an ion in common with acetic acid , a weak acid that dissociates in water to give acetate ions .Now addition of acetate ion produces a change in the colour of the indicator.

Ans 4:- When sodium acetate dissolves in water it breaks up into Na+ and C2H3O2- ions. The indicator changes colour with changing H3O+ concentration.The effect on the dissociation of acetic acid that is produced by adding sodium acetate is called the common ion effect.

Ans 5. Yes, they are in accordance with Le Chateliers principle because according to the principle, it states that there will be a shift in such a way that it will counteract any stress placed on the position of equilibrium.When we are adding sodium acetate to a solution of acetic acid we can increase the concentration of acetate anion and the equilibrium will shift to the left. This shift to the left will consume acetate anions and produces unionized acetic acid.

Ans 6. The reaction is endothermic as acetic acid is a weak electrolyte which means they do not dissociate completely, so it needs the external energy to undergo dissociation.

Ans 7. The reaction is

HC2H3O2 + H2O + heat -> H3O+ + C2H3O2-

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