Chemistry
What will happen if hydrochloric acid is added to the following equilibrium system?
H+(aq) + 2 CrO42-(aq) ⇔ Cr2O72-(aq) + OH-(aq)
yellow orange
a) The concentration of CrO42- will increase.
b) The concentration of Cr2O72- will increase.
c) The concentration of H+ will decrease.
d) The solution will become more yellow.
e) None of the above
None of the above.
When hydrochloric acid (HCl) is added to the equilibrium system, it will react with the hydroxide ions (OH-) present on the right side of the equation. The reaction can be represented as:
HCl + OH- → H2O + Cl-
This reaction will shift the equilibrium to the left side, reducing the concentration of hydroxide ions (OH-) and increasing the concentration of chloride ions (Cl-). However, it will not directly affect the concentrations of the other species in the equilibrium (H+, CrO42-, and Cr2O72-).
Therefore, none of the given options (a, b, c, or d) is correct.
are you sure?
Apologies for the confusion. I made an error in my previous response.
When hydrochloric acid (HCl) is added to the equilibrium system, it will donate hydrogen ions (H+) to the solution. This increase in the concentration of H+ will disrupt the equilibrium and shift it to the left side, favoring the formation of H+(aq) and reducing the concentration of hydroxide ions (OH-).
Therefore, the correct answer is c) The concentration of H+ will decrease.
what is the correct answer?
Apologies for the confusion in my previous responses. Let me provide you with the correct answer.
When hydrochloric acid (HCl) is added to the equilibrium system:
H+(aq) + 2 CrO42-(aq) ⇔ Cr2O72-(aq) + OH-(aq)
Since HCl donates hydrogen ions (H+), the addition of HCl will increase the concentration of H+ in the system. According to Le Chatelier's principle, an increase in H+ concentration will shift the equilibrium to the left side, favoring the reactants. Therefore, in this equilibrium system, the correct answer is c) The concentration of H+ will increase.
I apologize for the confusion caused previously.
To determine what will happen if hydrochloric acid (HCl) is added to the equilibrium system, let's analyze the equation:
H+(aq) + 2 CrO42-(aq) ⇔ Cr2O72-(aq) + OH-(aq)
According to Le Chatelier's principle, when a stress is applied to a system at equilibrium, the system will shift in a way that minimizes the effect of that stress.
Adding hydrochloric acid (HCl) to the system would increase the concentration of H+ ions in the solution.
The H+ ions will combine with the OH- ions to form water (H2O), resulting in the shift of the equilibrium to the right to consume the additional H+ ions. This shift will cause a decrease in the concentrations of the H+ and OH- ions.
Looking at the equation, we see that the H+ ions are on the left side of the equation and produce yellow-orange CrO42- ions. So, if the concentration of H+ decreases, the production of the yellow-orange CrO42- ions will also decrease. Therefore, the solution will become less yellow and more orange.
From the given options, the correct answer would be:
d) The solution will become more yellow.
The other statements are not accurate based on the addition of hydrochloric acid to the equilibrium system.