Reaction of AgNO3, CaCl2, and Al2(SO4)3 with Ba(NO3)2 and then NaCl?

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Discussion Overview

The discussion revolves around the expected reactions of an unlabeled bottle containing either AgNO3, CaCl2, or Al2(SO4)3 when tested with Ba(NO3)2 and subsequently with NaCl. Participants explore the behavior of these compounds in terms of precipitation and net ionic equations, focusing on theoretical predictions rather than experimental outcomes.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested
  • Mathematical reasoning

Main Points Raised

  • One participant outlines potential reactions for each compound with Ba(NO3)2, suggesting that AgNO3 would produce AgCl as a precipitate when NaCl is added, while CaCl2 would not produce a precipitate.
  • Another participant interprets the question as requiring separate tests for each reagent rather than a combined reaction, prompting a discussion on the clarity of the question's wording.
  • There is a suggestion to rewrite the reactions as net ionic equations, with some participants expressing uncertainty about how to proceed with NaCl's addition after Ba(NO3)2.
  • One participant acknowledges the ambiguity in the question and considers the implications of mixing ions from both reagents.
  • Participants discuss the presence of ions in the mixture and the potential for reactions based on those ions, particularly in the context of precipitation reactions.

Areas of Agreement / Disagreement

Participants express differing interpretations of the question, with some believing that both reagents are added to the same sample while others argue for separate tests. There is no consensus on the correct approach to the reactions involving NaCl.

Contextual Notes

There is a lack of clarity regarding the sequence of adding reagents and how that affects the expected reactions. Participants also note the importance of including state information in the reaction equations, which may impact understanding.

Who May Find This Useful

This discussion may be useful for students or individuals interested in chemical reactions, particularly in the context of precipitation and net ionic equations, as well as those exploring the nuances of interpreting experimental questions.

Widow
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1. The question is as follows: "You know that unlabeled bottle contains one of the following: AgNO3, CaCl2, or Al2(SO4)3. A friend suggests that you test a portion of the bottle with Ba(NO2)3 and then with NaCl. What behavior would you expect when each of these compounds is added to the unlabeled bottle?"2.

a) AgNO3(aq) + Ba(NO2)3 (s) = AgNO3 (aq) + Ba(NO2)3 (aq)

b) CaCl2 (aq) + Ba(NO2)3 (s) = BaCl2 (aq) + Ca(NO3)2 (aq)

c) Al2(SO4)3 (aq) + 3Ba(NO2)3 (s) = 3BaSO4 (s) + 2Al(NO3)3 (aq)

However, where I am stuck is figuring out how NaCl (s) reacts with the products of those three reactions. I'm aware that the first will produce AgCl as a precipitate and the second will not produce a precipitate, but I'm finding it difficult to figure out and balance the equations with three reactants. My tries are below, but I feel as if I am doing something wrong. Any help is greatly appreciated! I'm tearing my hair out! :P3.

a) AgNO3 + Ba(NO3)2 + NaCl = NaNO3 + AgCl + BaCl2 (do I list Ba(NO3)2 and AgNO3 again as the ions can recombine?)

b) BaCl2 + Ca(NO3)2 + NaCl = NaCl + BaCl2 + NaNO3 + CaCl2

c) BaSO4 (s) + Al(NO3)3 + NaCl = Na2SO4 + NaNO3+ BaCl2 + AlCl3
 
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As I understand the question it is not adding the second reagent to the mixture, but splitting the mixture into two parts and testing each part separately.

Add state information (as (s), (aq)) to your reaction equations, they will be easy to follow both for you and us.

Do you know what a net ionic reaction is? If so, try to rewrite the reactions as net ionic.
 
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Sorry about the lack of state information; I was in a bit of a rush and in a state of upset. I've added them now.

Do you think so? I thought the phrase "you test a portion of the bottle with Ba(NO3)2 and then with NaCl" indicates that you add NaCl to the same sample right after the Ba(NO3)2 (s) ? It also says "What behavior would you expect when each of these compounds is added to the unlabeled bottle," so I'm assuming there's only one unlabeled bottle to which you're adding these two compounds? Please correct me if I'm wrong. :)

I do know how to write a net ionic equation, and I would have had I not run into this problem :P.

I can write them out for the first step, yes, but since I'm confused with the addition of NaCl (s), I can't write those out yet.

a) No net ionic - no reaction

b) No net ionic - no reaction

c) 3SO42- (aq) + 3Ba2+ (aq) = 3BSO4 (s)

I know you said that you think that the Ba(NO3)2 (s) and the NaCl (s) are added separately, but is it possible to add the NaCl (s) right after the Ba(NO3)2 (s) and have a reaction with all those ions floating around (especially in reactions a and b). I hope I'm not being too confusing or vague.

I really appreciate your help! :)
 
OK, perhaps I am misreading the question - it is a little bit ambiguous to me, but then English is my second language.

Assuming you have to add both salts to the same sample - think what ions are present in the mixture. It really isn't much harder than mixing two salts, you just look what ions are present and what can happen. So far you are right with Ba(NO3)2 - a & b no reaction, c precipitation of solid.
 
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