Chemical Reactions and Observations: Barium Chloride and Sodium Sulfate

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Discussion Overview

The discussion revolves around predicting the outcomes of chemical reactions involving barium chloride and sodium sulfate, particularly in the context of solubility and precipitate formation. Participants explore the implications of adding various reagents to solutions containing different ionic compounds, focusing on theoretical predictions rather than experimental results.

Discussion Character

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

Main Points Raised

  • One participant presents two scenarios involving different ionic solutions and asks for help in determining the presence or absence of specific compounds based on theoretical predictions.
  • Another participant suggests consulting a solubility chart to identify which compounds are insoluble and would form precipitates when mixed.
  • Some participants emphasize the relationship between solubility and precipitate formation, stating that soluble compounds do not produce precipitates while insoluble ones do.
  • A participant expresses confusion regarding the application of the solubility chart, particularly in relation to the addition of hydrochloric acid and its effect on the solubility of the compounds in the first scenario.
  • Another participant attempts to clarify the presence of specific compounds in the scenarios, suggesting that silver nitrate is present in the first scenario and questioning the meaning of "your next step."
  • There is a discussion about the specific insoluble compounds, such as AgCl, AgBr, and BaSO4, and whether they can be concluded to be present based on the reactions described.
  • One participant questions whether the order of solubility affects the outcomes, indicating a potential source of confusion in interpreting the solubility chart.

Areas of Agreement / Disagreement

Participants express varying levels of understanding regarding the application of the solubility chart and the implications of precipitate formation. There is no consensus on the correct interpretation of the scenarios or the next steps to take, indicating ongoing confusion and disagreement.

Contextual Notes

Participants reference specific ionic compounds and their solubility, but there are unresolved questions about how the addition of hydrochloric acid influences the solubility of the compounds in the first scenario. The discussion also highlights the complexity of interpreting solubility data and the conditions under which precipitates form.

Who May Find This Useful

Individuals interested in chemical reactions, solubility principles, and the interpretation of solubility charts may find this discussion relevant.

Joules23
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1) A solution contains one or more of the following:
Silver nitrate
Potassium sulfate
iron(III) nitrate
Barium bromide

You add one drop of hydrochloric acid (solution). There is a precipitate.

Next you add one drop of barium nitrate (solution). There is no observable reaction.

Present: ______
Absent: ______
Your next step: ______

--------------------------------
2) A solution contains none or some of the following:
Silver nitrate
Copper(II) sulfate
iron(III) chloride
barium nitrate

You ad one drop of barium chloride (solution). There is no observable change.
Next you add one drop of sodium sulfate (solution). There is no observable change.

Present: ______
Absent: ______
Next step: _______

--------------------

Anyone have any idea as to how i would find this out, without actually performing the experiment?
 
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Last edited by a moderator:
also remember this:

if A Compound in water...

is soluble = no precipitant
insoluble = precipitant

use the solubility chart/table to determine what is soluble/insoluble. Shouldnt be that difficult...
 
i still don't understand i looked on the chart for #1 and they all are Soluble... how would adding the HCl factor in with the chart

HNO3 (3 is subscript)
HSO4 (4 is subscript)
3NO3H (2nd 3 is subscript)
HBr2 (2 is subscript)

Those are what i got after adding the HCl to the silver nitrate, potassium sulfate, etc... Now where do i go from there?
 
Last edited:
ok please let me know if i got this right

for #1, the only one present is silver nitrate

for #2 the only ones present are Copper(II) sulfate and iron(III)chloride

Also what is meant by, "your next step?"
 
AgCl, AgBr and BaSO4 are insoluble; every other combination is soluble...
 
im still not understanding it... ok, insoluble = precipitate .. so are you saying for both #1 and #2, the ones present are AgCl, AgBr and BaSO4 ?

btw, yes i am stupid
 
Last edited:
Joules23 said:
im still not understanding it... ok, insoluble = precipitate .. so are you saying for both #1 and #2, the ones present are AgCl, AgBr and BaSO4 ?
#1. If you add HCl and there is a precipitate (=insoluble) and the only insoluble substance among those could be AgCl, what do you conclude? If you add Ba++ and there is no precipitate, knowing that the only insoluble substance could be BaSO4, what do you conclude? Ecc.
 
When you use the solubility chart the higher always prevails, is that where your getting caught?
 

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