Solubility for hydrated calcium sulfate in HCl

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SUMMARY

The discussion focuses on the solubility of hydrated calcium sulfate (CaSO4·2H2O) in hydrochloric acid (HCl). The reaction is represented as CaSO4·2H2O + HCl <--> H3O^+ + Ca^2+ + SO4^2-. Participants clarify that the chloride ion (Cl^-) does not participate in the reaction, acting as a spectator ion. This is due to the high solubility of calcium chloride (CaCl2) in aqueous solutions, which allows Cl^- to remain freely ionized without forming a precipitate.

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  • Understanding of acid-base reactions
  • Knowledge of solubility rules in chemistry
  • Familiarity with ionic compounds and their behavior in solution
  • Basic principles of chemical equilibrium
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  • Research the solubility product constant (Ksp) for calcium sulfate
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Kruz87
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was asked to consider the solubility for hydrated calcium sulfate in HCl.
The principal acid my proffesor had posted for the solution was [ CaSO4(hyrdrated) + HCl <--> H30^+ + Ca^2+ + SO4^2- ]. I guess what I'm asking is what happened to the Cl^- and why isn't it reacting with Ca^2+ to produce CaCl2. ? It's not a spectator ion right? But if it is why?
 
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Chlorides are soluble, and the chloride ion will remain freely ionized. The "calcium chloride" will be present as ions of Ca(+2) and Cl(-1)
 

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