Question

The base ionization constant for ethylamine, C2H5NH2, in aqueous solution is kb = 6.41 x 10^-4

The base ionization constant for ethylamine, C2H5NH2, in aqueous solution is kb = 6.41 x 10^-4. C2H5NH2 (aq) + H2O (l) <> C2H5NH3^+ (aq) + OH^- (aq) Calculate the pH of a solution that results when you mix 40.0 mL of 0.100 M ethylamine with 40.0 mL of 0.100 M Hal. Hint: this is the equivalence point.


Comments
  • sorry, it should be 40 mL of 0.100 M HCl. Kai commented over 2 years ago