# Question 1: Rainwater is acidic because CO2 (g) dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3), forming calcium bicarbonate, Ca(HCO3)2

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Question 1: Rainwater is acidic because CO2 (g) dissolves in the water,
creating carbonic acid, H2CO3. If the rainwater is too acidic,
it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3), forming calcium bicarbonate, Ca(HCO3)2

CO2(g) + H2(l)$\leftrightharpoons$H+(aq) +HCO3(aq)

H+(aq) + CaCO3(s)$\leftrightharpoons$Ca+(aq) + HCO3 (aq)

1. Write the equilibrium expression of the forward and reversed reactions for each of the reversible reactions above.
2. Calculate the concentrations of hydrogen ion, bicarbonate ion (HCO3)
and calcium ion in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 ×10-5 M?
3. What is the equilibrium constant of the second reversible reaction?
4. What will happen to each of the reactions if the environment’s temperature increases?