Friday, January 3, 2020

acid base - How to calculate pH of the Na2CO3 solution given ambiguous Ka values


This is the exact question I faced on an exam. Calculate the pH of 0.05 M NaX2COX3 (HX2COX3:Ka,1=4×107, Ka,2=4.7×1011)


Solution


NaX2COX32NaX++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+HX2OHCOX3X+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 Mx,[HCOX3X]=[OHX]=x


So, we have:


x20.05x=Kb


All I need to know is Kb value for COX3X2 ion. I tried to derive Kb from Ka values using Ka×Kb=1×1014 but apparently obtained the incorrect answer. What method should I use to do it the right way?




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