Solubility for hydrated calcium sulfate in HCl

[Kruz87]

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?

 

[symbolipoint]

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)

 

[Blueshift5]

I would like to clarify that the reaction you have provided is not the solubility reaction for hydrated calcium sulfate in HCl. The solubility reaction would be written as CaSO4 (hydrated) + 2HCl → CaCl2 + H2SO4. This reaction indicates that hydrated calcium sulfate (CaSO4) reacts with 2 molecules of hydrochloric acid (HCl) to form calcium chloride (CaCl2) and sulfuric acid (H2SO4). The sulfuric acid may further dissociate to form H+ and SO4^2- ions.

Now, coming to your question about the role of chloride ions (Cl^-) in this reaction, they do not participate in the reaction itself but serve as a counterion to balance the charges of the resulting ions. Calcium chloride (CaCl2) is a salt that dissociates in water to form Ca^2+ and 2Cl^- ions, which can be considered as spectator ions in this reaction. They do not undergo any chemical changes and remain in solution.

I hope this clarifies your doubts about the role of chloride ions in the solubility reaction of hydrated calcium sulfate in HCl. it is important to carefully examine the chemical equations and understand the role of each component to accurately interpret the reactions.