Question #6 For 0.4847 M KNO, what is the pH of a 3.367e-2 solution of acetic...

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Question #6 For 0.4847 M KNO, what is the pH of a 3.367e-2 solution of acetic acid? Again, using the two alternate definitions of pH. For the concentration definition of pH you should ignore activity (i.e., solve in the usual way). You can assume because the KNO3 concentration is high that it determines the ionic strength, i.e. you can assume that the contributions of H+,OH- and acetate are negligible compared to the total ion concentration in solution. The size parameter for acetate is 0.450 nm. Use Ka=10-4.75 for both methods, but in concentration units for the concentration-based pH and in activity units for activity based pH. 1. pH=-log[H*]= 2. pH=-log(H*)= Question #6 For 0.4847 M KNO, what is the pH of a 3.367e-2 solution of acetic acid? Again, using the two alternate definitions of pH. For the concentration definition of pH you should ignore activity (i.e., solve in the usual way). You can assume because the KNO3 concentration is high that it determines the ionic strength, i.e. you can assume that the contributions of H+,OH- and acetate are negligible compared to the total ion concentration in solution. The size parameter for acetate is 0.450 nm. Use Ka=10-4.75 for both methods, but in concentration units for the concentration-based pH and in activity units for activity based pH. 1. pH=-log[H*]= 2. pH=-log(H*)=

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Let us denote the ions as H and A So Firstly the co... View the full answer