Suppose 10.0 mL of HCl gas at 25 degree C and 734 torr is bubbled into 257 mL of

Question

Suppose 10.0 mL of HCl gas at 25 degree C and 734 torr is bubbled into 257 mL of pure water. What will be the pH of the resulting solution, assuming all the HCl dissolves in the water? One of the reactions that occurs in polluted air in urban areas is shown below. It is believed that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k [NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. A 1.0 M solution of acetic acid has a pH 2.37. What percentage of acetic acid is ionized in the solution?

Explanation / Answer

1) Number of mols of HCl gas bubbled = (734/760) atm* 0.010 L / (0.0821 L.atm/mol.K )(298 K) = 3.947*10-4 mol

      Thus, concnetration of HCl = (3.947*10-4 mol / (0.010+0.257) L = 1.478*10-3 mol/L

2) The mechanism for given rate law - , rate = k [NO2][O3] is -

       Step:1 ----> NO2 + O3 ---------> NO3 + O2

       step:2 -----> NO3 + NO2 ------> N2O5

3) since - pH = 2.37 ===> [H+] = 10-2.37 = 0.00426 M

% ionization = (0.00426 / 1)*100 = 0.42 %

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