IDNLearn.com connects you with a global community of knowledgeable individuals. Explore thousands of verified answers from experts and find the solutions you need, no matter the topic.
Sagot :
To determine the effect on the equilibrium when the pH is increased, we must consider how the system will respond according to Le Chatelier's principle. Le Chatelier’s principle states that a system in equilibrium will adjust to counteract any changes imposed on it.
We are given the following chemical equilibrium reactions:
[tex]\[ CO _{2(g)}+ H _2 O _{(l)} \longleftrightarrow H _2 CO _{3(aq)} \][/tex]
[tex]\[ H _2 CO _{3(aq)} \longleftrightarrow H ^{+}(aq)+ HCO _3^{-}(aq) \][/tex]
Step-by-Step Solution:
1. Understanding pH Increase:
- Increasing the pH of a solution means reducing the concentration of hydrogen ions ([tex]\( H^+ \)[/tex]) in the solution, making it less acidic.
2. Response to the Change in [tex]\( H^+ \)[/tex] Concentration:
- According to Le Chatelier's principle, the equilibrium will shift to counteract the decrease in [tex]\( H^+ \)[/tex] ions. To increase the [tex]\( H^+ \)[/tex] ion concentration, the system will favor the direction that produces more [tex]\( H^+ \)[/tex].
3. Identifying Affected Equilibria:
- The second equation directly involves [tex]\( H_2CO_3 \)[/tex] dissociating into [tex]\( H^+ \)[/tex] and [tex]\( HCO_3^- \)[/tex]:
[tex]\[ H_2CO_3(aq) \longleftrightarrow H^+(aq) + HCO_3^-(aq) \][/tex]
- To counteract the reduction in [tex]\( H^+ \)[/tex], the reverse reaction (formation of [tex]\( H_2CO_3 \)[/tex] from [tex]\( H^+ \)[/tex] and [tex]\( HCO_3^- \)[/tex]) will be favored.
4. Effect on the First Equation:
- As more [tex]\( H_2CO_3 \)[/tex] is formed, the equilibrium of the first reaction will also be affected:
[tex]\[ CO_2(g) + H_2O(l) \longleftrightarrow H_2CO_3(aq) \][/tex]
- With more [tex]\( H_2CO_3 \)[/tex] being in demand to balance the [tex]\( H^+ \)[/tex] ions being consumed, this equilibrium will shift towards producing more [tex]\( H_2CO_3 \)[/tex] from [tex]\( CO_2 \)[/tex] and [tex]\( H_2O \)[/tex].
5. Final Conclusion:
- The overall effect of increasing the pH (reducing [tex]\( H^+ \)[/tex] concentration) will lead the system to produce more [tex]\( H_2CO_3 \)[/tex] to counteract the loss of [tex]\( H^+ \)[/tex] ions.
Therefore, the equilibrium will shift such that:
More [tex]\( H_2CO_3 \)[/tex] will be produced.
This detailed analysis leads us to conclude that the correct answer is:
- More [tex]\( H_2CO_3 (aq) \)[/tex] will be produced.
We are given the following chemical equilibrium reactions:
[tex]\[ CO _{2(g)}+ H _2 O _{(l)} \longleftrightarrow H _2 CO _{3(aq)} \][/tex]
[tex]\[ H _2 CO _{3(aq)} \longleftrightarrow H ^{+}(aq)+ HCO _3^{-}(aq) \][/tex]
Step-by-Step Solution:
1. Understanding pH Increase:
- Increasing the pH of a solution means reducing the concentration of hydrogen ions ([tex]\( H^+ \)[/tex]) in the solution, making it less acidic.
2. Response to the Change in [tex]\( H^+ \)[/tex] Concentration:
- According to Le Chatelier's principle, the equilibrium will shift to counteract the decrease in [tex]\( H^+ \)[/tex] ions. To increase the [tex]\( H^+ \)[/tex] ion concentration, the system will favor the direction that produces more [tex]\( H^+ \)[/tex].
3. Identifying Affected Equilibria:
- The second equation directly involves [tex]\( H_2CO_3 \)[/tex] dissociating into [tex]\( H^+ \)[/tex] and [tex]\( HCO_3^- \)[/tex]:
[tex]\[ H_2CO_3(aq) \longleftrightarrow H^+(aq) + HCO_3^-(aq) \][/tex]
- To counteract the reduction in [tex]\( H^+ \)[/tex], the reverse reaction (formation of [tex]\( H_2CO_3 \)[/tex] from [tex]\( H^+ \)[/tex] and [tex]\( HCO_3^- \)[/tex]) will be favored.
4. Effect on the First Equation:
- As more [tex]\( H_2CO_3 \)[/tex] is formed, the equilibrium of the first reaction will also be affected:
[tex]\[ CO_2(g) + H_2O(l) \longleftrightarrow H_2CO_3(aq) \][/tex]
- With more [tex]\( H_2CO_3 \)[/tex] being in demand to balance the [tex]\( H^+ \)[/tex] ions being consumed, this equilibrium will shift towards producing more [tex]\( H_2CO_3 \)[/tex] from [tex]\( CO_2 \)[/tex] and [tex]\( H_2O \)[/tex].
5. Final Conclusion:
- The overall effect of increasing the pH (reducing [tex]\( H^+ \)[/tex] concentration) will lead the system to produce more [tex]\( H_2CO_3 \)[/tex] to counteract the loss of [tex]\( H^+ \)[/tex] ions.
Therefore, the equilibrium will shift such that:
More [tex]\( H_2CO_3 \)[/tex] will be produced.
This detailed analysis leads us to conclude that the correct answer is:
- More [tex]\( H_2CO_3 (aq) \)[/tex] will be produced.
We value your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Thank you for choosing IDNLearn.com. We’re here to provide reliable answers, so please visit us again for more solutions.
