Chemical Forums
Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: orgo814 on November 06, 2013, 01:45:05 AM
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1) What is the pH of a solution containing 0.2 g/L sodium carbonate and 0.1 g/L sodium hydrogen carbonate? (Ka1 = 4.1 x 10^-7, Ka2 = 5.6 x 10^-11)
I know to use the henderson-hasselbach equation but I'm unsure of which Ka to use for my pKa. Any insight would be great. I would assume Ka1?
2) What is the standard enthalpy of a reaction for which the equilibrium constant increases by a factor of ten when the temperature is increased from 273 K to 298 K?
I know the equation is lnK2/K1 = -delta H/R (1/T2 - 1/T1). I'm just confused on the wording "increased by a factor of ten". Would I put something like 30 as my K2 and 20 as my K1? Or would I just do the natural log of 10?
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I know to use the henderson-hasselbach equation but I'm unsure of which Ka to use for my pKa. Any insight would be great. I would assume Ka1?
You have CO32- and HCO3- present in the solution - which Ka value described their equilibrium?
I know the equation is lnK2/K1 = -delta H/R (1/T2 - 1/T1). I'm just confused on the wording "increased by a factor of ten". Would I put something like 30 as my K2 and 20 as my K1? Or would I just do the natural log of 10?
It means K2=10K1.
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I would say ka1 because it only went through one step?
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Write both dissociation steps, write Ka for each one. Which contains concentrations of the substances present in the solution?
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CO3(2-) + H2O yields HCO3-. Is that not the first step?
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No.
http://www.chembuddy.com/?left=pH-calculation&right=polyprotic-dissociation-constants
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Well then I'm confused as to what it is
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Oh HCO3- yields CO32- so second ionization. First would be starting with h2co3
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Exactly.