Write the balanced molecular equation and net ionic equation for the neutralization reaction between hydrochloric acid and strontium hydroxide. Include the phase of each species.

Answer 1

Sr(OH)2 is slightly soluble in water and the equations will be slightly different depending upon if the solid Sr(OH)2 or a solution of Sr(OH)2 is used. I'll write both.
First for the solid Sr(OH)2.
molecular equation:
2HCl(aq) + Sr(OH)2(s) ==> 2H2O(l) + SrCl2(aq)
Ionic equation:
2H^+(aq) + 2Cl^-(aq) + Sr(OH)2(s) ==> 2H2O(l) + Sr^2+(aq) + 2Cl^-(aq)
net ionic equation:
2H^+(aq) + Sr(OH)2(s) ==> 2H2O(l) + Sr^2+(aq)
Using solution of Sr(OH)2 and I suspect this is what your professor wants.
molecular equation:
2HCl(aq) + Sr(OH)2(aq) ==> 2H2O(l) + SrCl2(aq)
Ionic equation:
2H^+(aq) + 2Cl^-(aq) + Sr^2+(aq) + 2(OH)^-(aq) ==> 2H2O(l) + Sr^2+(aq) + 2Cl^-(aq)
Net ionic equation:
2H^+(aq) + 2OH^-(aq) ==> 2H2O(l)