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Hi, was wondering if anyone out there could help me with this acids/bases problem I'm stumped on:
The equilibrium constant for dissolving CaCO3 in water is 3.4E-9. What is the equilibrium constant for dissolving CaCO3 in the presence of acid? (Ka of H2CO3 = 4.2E-7; Ka of HCO3- = 4.8E-11)
a. 1.6E-19
b. 2.9E8
c. .008
d. 70.8
The correct answer is d.
I am confused about how to even approach this problem, or make use of the information being given. Also, the Ka for CO3^2- is 2.1E-4, not 3.4E-9, so I'm not even sure where that number comes from...
Any help would be greatly appreciated.
The equilibrium constant for dissolving CaCO3 in water is 3.4E-9. What is the equilibrium constant for dissolving CaCO3 in the presence of acid? (Ka of H2CO3 = 4.2E-7; Ka of HCO3- = 4.8E-11)
a. 1.6E-19
b. 2.9E8
c. .008
d. 70.8
The correct answer is d.
I am confused about how to even approach this problem, or make use of the information being given. Also, the Ka for CO3^2- is 2.1E-4, not 3.4E-9, so I'm not even sure where that number comes from...
Any help would be greatly appreciated.