Question

1)Calculate the pH of a solution that results from mixing 10 mL of 0.11 M ammonia with 39 mL of 0.11 M ammonium chloride. The K_b value for NH₃ is 1.8 x 10^-5

2)A buffer that contains 0.18 M of an acid, HA and 0.31 M of its conjugate base A^-, has a pH of 4.66. What is the pH after 0.034 mol of HCl are added to 0.6 L of the solution

3)Calculate the pH during the titration of 30.00 mL of 0.1000 M NaOH(aq) with 0.1000 M HNO₃(aq) after 12 mL of the acid have been added

4)Calculate the pH during the titration of 20.00 mL of 0.1000 M HBrO(aq) with 0.1000 M LiOH(aq) after 8 mL of the base have been added. K_a of hypobromous acid = 2.3 x 10^-9.

5)Calculate the pH during the titration of 20.00 mL of 0.1000 M methylamine, (CH₃)NH₂(aq), with 0.2000 M HCl(aq) after 7.5 mL of the acid have been added. K_b of methylamine = 3.6 x 10^-4

6)Calculate the pH during the titration of 30.00 mL of 0.1000 M dimethylamine, (CH₃)₂NH(aq), with 0.1000 M HBr(aq) after 29 mL of the acid have been added. K_b of dimethylamine = 5.4 x 10^-4

⁷⁾Determine the volume in mL of 0.2 M HCl(aq) needed to reach the equivalence (stoichiometric) point in the titration of 49 mL of 0.25 M NH₂NH₂(aq)(aq). The K_b of hydrazine is 1.7 x 10^-6

⁸⁾Determine the pH at the equivalence (stoichiometric) point in the titration of 23 mL of 0.12 M C₆H₅COOH(aq) with 0.22 M NaOH(aq). The K_a of benzoic acid is 6.5 x 10^-5