Question
The equation for a base solution is B+H 2 O rightleftharpoons B * H ^ O H^ - The strength of the base in a solution is increased. How will the number of particles change? (1 point)
The number of B molecules will increase, and the number of water molecules will decrease.
The number of BH molecules will increase, and the number of water molecules will decrease
The number of OH ions will increase, and the number of BH molecules will decrease.
The number of B molecules will increase, and the number of OH ions will decrease.
The number of B molecules will increase, and the number of water molecules will decrease.
The number of BH molecules will increase, and the number of water molecules will decrease
The number of OH ions will increase, and the number of BH molecules will decrease.
The number of B molecules will increase, and the number of OH ions will decrease.
Answers
Answered by
GPT-4o mini
In the given equilibrium reaction for a base \( B \):
\[ B + H_2O \rightleftharpoons BH + OH^- \]
When the strength of the base \( B \) in a solution increases, it suggests that more molecules of \( B \) are reacting with water to produce \( BH \) and \( OH^- \) ions.
- As more \( B \) reacts with water, the number of \( BH \) molecules (the conjugate acid formed) will increase.
- Additionally, the increase in base strength will lead to an increase in the concentration of \( OH^- \) ions, since \( OH^- \) is produced during the reaction.
Therefore, the correct change in the number of particles when the strength of the base increases will be:
**The number of \( BH \) molecules will increase, and the number of \( OH^- \) ions will increase.**
However, in terms of the provided options, the closest and most relevant choice related to the discussion would be:
**The number of \( OH^- \) ions will increase, and the number of \( BH \) molecules will decrease.**
This option does not seem correct based on typical base behavior. A correct interpretation based on Le Chatelier's principle should indicate that increasing the base results in more \( OH^- \) and \( BH \) rather than a decrease in \( BH \).
The confusion likely arises in the phrasing of the options. The most accurate conclusion based on the equilibrium would emphasize an increase in \( BH \) and \( OH^- \). Thus, if the question allows interpretation or flexibility, it ultimately aligns with the general behavior rather than an exact match in the provided choices.
\[ B + H_2O \rightleftharpoons BH + OH^- \]
When the strength of the base \( B \) in a solution increases, it suggests that more molecules of \( B \) are reacting with water to produce \( BH \) and \( OH^- \) ions.
- As more \( B \) reacts with water, the number of \( BH \) molecules (the conjugate acid formed) will increase.
- Additionally, the increase in base strength will lead to an increase in the concentration of \( OH^- \) ions, since \( OH^- \) is produced during the reaction.
Therefore, the correct change in the number of particles when the strength of the base increases will be:
**The number of \( BH \) molecules will increase, and the number of \( OH^- \) ions will increase.**
However, in terms of the provided options, the closest and most relevant choice related to the discussion would be:
**The number of \( OH^- \) ions will increase, and the number of \( BH \) molecules will decrease.**
This option does not seem correct based on typical base behavior. A correct interpretation based on Le Chatelier's principle should indicate that increasing the base results in more \( OH^- \) and \( BH \) rather than a decrease in \( BH \).
The confusion likely arises in the phrasing of the options. The most accurate conclusion based on the equilibrium would emphasize an increase in \( BH \) and \( OH^- \). Thus, if the question allows interpretation or flexibility, it ultimately aligns with the general behavior rather than an exact match in the provided choices.