Le Chatelier's Principle and equilibrium (1 Viewer)

[AnAn]

Q1.Arrange the following aqueous systems in order of their ability to dissolve CO2. Assume that, prior to exposure to 10% CO2 in Ar, they have been allowed to equilibrate with air:
1) distilled water
2) 1 M HCl solution
3) 1 M sodium hydroxide solution

Q2 Explain why we can dissolbe more carbon dioxide in an aqueous solutionof ammonia than in pure water

** can anyone explain Le Chatelier's Principle and equilibrium?? coz i dun know how to write balance equations.

thx for help~~

 

[CM_Tutor]

The answer to question 1 is (in increasing order of solubility) (2) then (1) then (3). The reason is that the dissolution of CO₂ in water produces acid, in an equilibrium. The presence of acid thus pushes the equilibrium position left (hence, low solubility in acidic solution), and the presence of base causes acid to be consumed, thereby drawing the equilibrium position to the right (hemce, high CO₂ in basic solution).

As for question 2, read this thread http://www.boredofstudies.org/community/showthread.php?s=&threadid=31258 and then come back and ask if you need more help.