Why Do KNO3, BaCl2, Na2SO4, and KCl Solutions Show No Reaction?

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KNO3 (aq) and BaCl2 (aq) do not undergo a chemical reaction because they remain as dissociated ions in solution. Similarly, Na2SO4 (aq) and KCl (aq) also exist as separate ions in an aqueous environment, leading to no observable chemical change. The discussion highlights that since all compounds are soluble in water, they do not react with each other under these conditions. However, it is noted that BaSO4 could precipitate if BaCl2 and Na2SO4 were mixed, indicating a potential reaction under specific circumstances. The key point is that without the formation of a precipitate or a gas, the presence of these compounds in solution does not lead to a chemical reaction.
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can you just tell me why KNO3 (aq) and BaCl2 (aq) & Na2SO4 (aq) and KCl (aq) have no chemical change? Why is there no reaction between these?
 
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One possibility is that they are all in aqueous solution, so nothing really happens. They just float around in ionized form.

However, I think that BaSO4 would precipitate out...
 
textbooks said:
can you just tell me why KNO3 (aq) and BaCl2 (aq) & Na2SO4 (aq) and KCl (aq) have no chemical change? Why is there no reaction between these?

Do you mean all four in the solution at the same time?

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