18. Aqueous Equilibrium

Calculate the pH of the solution resulting from the mixing of 175.0 mL of 0.250 M HNO₃ with 75.0 mL of 0.200M Ba(OH)₂.

Calculate the pH of the solution resulting from the mixing of 175.0 mL of 0.250 M HNO₃ with 75.0 mL of 0.200 M Ba(OH)₂.

Calculate the pH of the solution resulting from the titration of 110.0 mL of 0.300 M HCl with 330.0 mL of 0.100 M LiOH.

A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:

(c) 20.0 mL.

A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:

(a) 15.0 mL

(b) 19.9 mL.

Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false. (a) More base is required to reach the equivalence point for the strong acid than the weak acid.

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) NH₃ titrated with HCl.