Question

# Write a balanced net ionic equation to show why the solubility of Ca(OH)2(s) increases in the...

Write a balanced net ionic equation to show why the solubility of Ca(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s). + + K =

Solubility equilibrium for Ca(OH)2 is :

Ca(OH)2(s)<------>Ca2+(aq) + 2OH-(aq), K1= Ksp = 7.9×10-6

And in strong acid H3O+ are present which would react with OH- as follows H3​​​​​​O+(aq) + OH​​​​​​-(aq) <-----> 2H2O(l), K2=1014

Combining two times of second equation with Ca(OH)2 equation and cancelling common terms, we get net ionic equation as follows:

Ca(OH)2(s) + 2H3​​​​​​O+(aq) <-----> Ca2+(aq) +4H2​​​​​​O(l),

Note if you write H+ in place of H3O+ then write 2H+ on left and 2H2O on right side instead of 4H2O.

Keq= K1×K22 (as second equation is multiplied by two, so K2 raised to power 2)= 7.9×10-6×(10​​​​​14)2= 7.9×1022, which is very high.

Comment in case of any doubt.

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