This is the exact question I faced on an exam. Calculate the pH of 0.05 M NaX2COX3 (HX2COX3:Ka,1=4×10−7, Ka,2=4.7×10−11)
Solution
NaX2COX3⟶2NaX++COX3X2−
I suppose nothing that can contribute to the pH of a solution happens to NaX+ ions and we proceed with COX3X2− which has a concentration of 0.05 M
COX3X2−+HX2O−⇀↽−HCOX3X−+OHX−
To calculate pH, I need to first figure out concentration of OHX− ions, and to do so I have to know Kb dissociation constant for COX3X2−
On equilibrium concentration of species are as follows: [COX3X2−]=0.05 M−x,[HCOX3X−]=[OHX−]=x
So, we have:
x20.05−x=Kb
All I need to know is Kb value for COX3X2− ion. I tried to derive Kb from Ka values using Ka×Kb=1×10−14 but apparently obtained the incorrect answer. What method should I use to do it the right way?
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