Rainwater is acidic because CO2 (g) dissolves in the water

Question 1

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

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?

Question 2

Question 3

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). Calculate the concentrations of carbonic acid, bicarbonate ion (HCO^3-) and carbonate ion (CO3^2-) that are 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.

Answer to question 1

Answer to question 2

Answer to question 3

Step 1

Given: Raindrop pH = 5.60

Step 2

Now, reaction equation for the given reaction is as follows.

Step 3

Step 4