Chemistry-equilibrium reaction question

  • Thread starter Thread starter Puchinita5
  • Start date Start date
  • Tags Tags
    Reaction
AI Thread Summary
Mixing 3mL of 0.10 M acetic acid with 1.0 M sodium acetate shifted the equilibrium towards the left due to an increase in acetate ions, resulting in a color change from reddish to yellow with methyl orange indicator. The discussion explores alternative solutions that could also shift the equilibrium left, specifically considering the addition of a strong acid like HCl or HBr, which would increase H3O+ ions. The contributor believes this would cause a similar shift and color change, although they seek confirmation of their reasoning. Responses affirm the contributor's understanding, indicating that their logic is sound. The conversation highlights the relationship between acid-base equilibria and color indicators in chemistry.
Puchinita5
Messages
178
Reaction score
0

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
 
Physics news on Phys.org
Your thinking seems correct to me :smile:

--
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
View full post »

Similar threads

Chemistry How to calculate pH at equivalence point using this alternative?
Replies
7
Views
1K
Chemistry Are there typos in this snippet causing confusion?
Replies
2
Views
1K
Equilibrium Constant for Alcohol and Acetic Acid Reaction at 25°C | Homework
Replies
15
Views
3K
Lowest concentration of ethanoate ions
Replies
2
Views
2K
Chemistry How to take into account autoprotolysis in weak base solution?
Replies
8
Views
2K
Chemistry Understanding how to calculate pH of a buffer solution
Replies
2
Views
1K
Chemistry How to think about increased temperature effect on water autoprotolysis equilibrium constant?
Replies
4
Views
1K
Chemistry How do we interpret the steps in the algorithm to balance a redox equation?
Replies
7
Views
2K
Calculate Equilibrium Constant for Polyprotic Acid Reaction
Replies
2
Views
2K
What Happens to Copper (II) Chloride Solution Under Different Conditions?
Replies
3
Views
4K

Hot Threads

Recent Insights

Back
Top