Q2) What is the pH at which a buffer composed of CO32- and HCO3- would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook
Sol.
As Ka of HCO3- = 4.8 × 10-11
So , pKa = - log(Ka) = - log( 4.8 × 10-11 ) = 10.32
As Henderson - Hasselbalch equation ,
pH = pKa + log ( [CO32-] / [HCO3-] )
pH would be most effective , when , the concentration of conjugate base , CO32- and concentration of acid , HCO3- are equal
That is , [HCO3-] = [CO32-]
So , pH = pKa + log ( 1 ) = pKa
pH = 10.32
Q2) What is the pH at which a buffer composed of CO32- and HCO3- would be...
What is the pH at which a buffer composed of CO32- and HCO3- would be most effective at resisting pH change? I think the answer is 10.32 but I wanted to check.
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What is the pH at which a buffer composed of NH3 and NH4+ would be most effective at resisting pH change? Round your answer to 2 decimal places.
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