If you have a solute of Ca(HCO3)2 and a solvent of H2O , what would you see(have) in the solution?

If you have a solute of Ca(HCO3)2 and a solvent of H2O , what would you see(have) in the solution?

The question boils down to, "to what does Ca(HCO3)2 ionize, in water"

Ca(HCO_3)_2 \,\rightleftharpoons\, Ca(HCO_3)^+ + HCO_3^- \,\rightleftharpoons\, Ca^{+2} + 2 HCO_3^-

Bicarbonate, also has its own equilibrium:

HCO_3^- \,\rightleftharpoons\, H^+ + CO_3^{-2}

If you wish, you can put "(aq)" after the ions, but normally one just assumes that.

Water, itself, also ionizes very slightly

H_2O \,\rightleftharpoons\,H^+ + OH^-