The question and the corresponding passage is below, but you probably just need up to Reaction 1 for the sake of this question.
I originally thought the answer was either B or C.
1) So for B, you can't dissolve a solid base with base? Because I thought like dissolves like.
2) For C, I thought addition of Na+ into the solution would drive the reaction to the left by Le Chatlier's principle, and the free M2+ would react with OH-? But then I guess this is not measureable?
3) Can you tell me what the experiment in D is doing? According to my understanding, adding strong acid HCl to a solid weak base will dissolve it and release it in its acidic form (since it gets protonated). I understand this much, but I don't undertand "The difference in the number of moles of HCl and NaOH required to reach the endpoint". Wouldn't there actually be no difference because ALL of the HCl added would be neutralized by NaOH?? Say for example we had add 1 mole of HCl, and 0.3 mole of H+ react with the RCO2 releasing it as fatty acid (this means that there are 0.3 moles of fatty acid present the precipitate), and the rest of the 0.7 moles of H+ just hangs out in the solution since there's no more weak base to react with. Now we add NaOH to titrate the solution, and because NaOH is a strong base, it neutralizes both the fatty acid and the H+ that is just hanging out in the solution, and we figure out that we used 1 mole of NaOH. So we put in 1 mole of HCl and added 1 mole of NaOH to neutralize it. There would be no difference that the answer explanation is talking about?? Or am I missing some sort of big picture/concept here?
4) I feel like I've over-thought this question, is there a simpler way to approach this question?
I originally thought the answer was either B or C.
1) So for B, you can't dissolve a solid base with base? Because I thought like dissolves like.
2) For C, I thought addition of Na+ into the solution would drive the reaction to the left by Le Chatlier's principle, and the free M2+ would react with OH-? But then I guess this is not measureable?
3) Can you tell me what the experiment in D is doing? According to my understanding, adding strong acid HCl to a solid weak base will dissolve it and release it in its acidic form (since it gets protonated). I understand this much, but I don't undertand "The difference in the number of moles of HCl and NaOH required to reach the endpoint". Wouldn't there actually be no difference because ALL of the HCl added would be neutralized by NaOH?? Say for example we had add 1 mole of HCl, and 0.3 mole of H+ react with the RCO2 releasing it as fatty acid (this means that there are 0.3 moles of fatty acid present the precipitate), and the rest of the 0.7 moles of H+ just hangs out in the solution since there's no more weak base to react with. Now we add NaOH to titrate the solution, and because NaOH is a strong base, it neutralizes both the fatty acid and the H+ that is just hanging out in the solution, and we figure out that we used 1 mole of NaOH. So we put in 1 mole of HCl and added 1 mole of NaOH to neutralize it. There would be no difference that the answer explanation is talking about?? Or am I missing some sort of big picture/concept here?
4) I feel like I've over-thought this question, is there a simpler way to approach this question?