K2SO4+ Na2HPO4=?
NaHCO3 + Sr(NO3)2=?
3 answers
I don't believe either of these react. In water they will dissolve to form the corresponding ions.
An ionic exchange reaction only occurs when dissolved ions are removed from solution as (1) a precipitate (solid), (2) a gas, or (3) form a molecule that remains in the liquid phase.
Sodium- and Potassium- -Biphosphates (and -Phosphates) are soluble. Sodium- and Potassium- -Sulfates (and -Bisulfates) are soluble. No reaction occurs.
However, Strontium Carbonate is insoluble.
NaHCO3(aq) + Sr(NO3)2(aq) = SrCO3(s) + NaNO3(aq) + HNO3(aq)
Sodium- and Potassium- -Biphosphates (and -Phosphates) are soluble. Sodium- and Potassium- -Sulfates (and -Bisulfates) are soluble. No reaction occurs.
However, Strontium Carbonate is insoluble.
NaHCO3(aq) + Sr(NO3)2(aq) = SrCO3(s) + NaNO3(aq) + HNO3(aq)
I agree that SrCO3 is insoluble; however, I believe the reaction (or lack of it) will form Sr(HCO3)2 and I believe that is soluble as is Ca(HCO3)2 and Ba(HCO3)2.
Ca(HCO3) can be formed by bubbling CO2 through a suspension of CaCO3.
Ba(HCO3)2 can be formed by bubbling CO2 through a (cold) suspension of BaCO3.
Therefore, I think Sr(HCO3)2 can be formed by bubbling CO2 through a cold suspension of SrCO3 and that Sr(HCO3)2 is soluble. However, I can't confirm that. I suspect in real life that no ppt will form (or perhaps a slight haze), then with standing the solution will lose CO2 and a ppt of SrCO3 will form.
Ca(HCO3) can be formed by bubbling CO2 through a suspension of CaCO3.
Ba(HCO3)2 can be formed by bubbling CO2 through a (cold) suspension of BaCO3.
Therefore, I think Sr(HCO3)2 can be formed by bubbling CO2 through a cold suspension of SrCO3 and that Sr(HCO3)2 is soluble. However, I can't confirm that. I suspect in real life that no ppt will form (or perhaps a slight haze), then with standing the solution will lose CO2 and a ppt of SrCO3 will form.
1 answer