Chemistry-equilibrium reaction question

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SUMMARY

The discussion centers on the equilibrium reaction involving acetic acid (HOAC) and its interaction with sodium acetate in a laboratory setting. When 3mL of 0.10 M acetic acid is mixed with 1.0 M sodium acetate, the equilibrium shifts to the left due to an increase in acetate ions (OAc-), resulting in a color change from reddish to yellow with methyl orange indicator. The participant correctly identifies that adding a strong acid, such as HCl or HBr, would also shift the equilibrium to the left by increasing hydronium ions (H3O+), potentially causing a similar color change.

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  • Understanding of chemical equilibrium principles
  • Knowledge of acid-base reactions
  • Familiarity with indicators like methyl orange
  • Basic concepts of molarity and solution preparation
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Homework Statement



In lab, we mixed 3mL of 0.10 M acetic acid.

I was given that the principal equilibrium is:
HOAC + H20 <----> H30+ + OAc-

We then added 1.0 M sodium acetate and a drop of methyl orange indicator. The color changed from redish to yellow.

I figured out (correctly) that the principal equilibrium shifts to the left because of the increase in OAc- ions.

The question is: What other solution could you have added to the acetic acid solution instead of one with acetate ion to cause the principal equilibrium in the acetic acid solution to shift in the same direction? Would this cause the same color change?

Homework Equations


The Attempt at a Solution



I THINK (though I'm honestly not very good with chemistry), that if I add a strong acid it will also shift to the left? For example, maybe HCl or HBr or something. I think this because the strong acid would increase the H3O+ ions, also shifting it to the left.

And I don't see why the color wouldn't change the same?

I have no way of checking if I'm correct which is why I'm asking. Any comments would be great! thank you
 
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