I\'m doing my chemistry lab homework.. in the lab we took 1M stock acetic acid a

Question

I'm doing my chemistry lab homework.. in the lab we took 1M stock acetic acid and for the first solution we added about 15 mL of it to a 100mL flask then filled the rest of it with DI water and got a concentration of solution 1 to be 0.100M. In the homework we have to find the equilibrium concentration of CH3CO2- .. the relationship between the concentration of the hydronium ion and acetate ion is expressed by the equilibrium:

H20 + HCH3CO2 --> <-- CH3CO2- + H30+

When i look for the [CH3CO2-] at equilibrium do i use 1M for [HCH3CO2](initial concentration) of the stock acetic acid or 0.1M(initial concentration) from the solution????

Explanation / Answer

You have used 1M for [HCH3CO2](initial concentration) of the stock acetic acid because, it is only molar concentration from where you will get the equilibrium after the addition of water into you staock solution.

since you have to find the equilibrium concentraion of CH3CO2- using water as the other solvent, so it must to consider 1M solution as initial for the given reaction

H20 + HCH3CO2 --> <-- CH3CO2- + H30+

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