16 Calculate the pH of the solution resulting from the addition of 20.0 mL of 0.100 M NaOH to 30.0 mL of 0.100 M HNO3. (a) 1.35 (b) 1.70 (c) 1.95 (d) 2.52 (e) 2.80

The H3O+ ion mole concentration of the following solution was measured at 25 °C. Find pH and pOH of each solution.   (a) 1.5X10-5 mol/dm3(b) 1.5 mmol/dm

25) Consider 0.14 M monoprotic acid (HA) that is 12% ionized. (a) Show the reaction of dissociation (ionization) of HA (b) Calculate the [H+] in the solution. (c) Calculate the Ka of HA.

7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethavois acid (CH;COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

If 0.50 L 0.20 M HF solution is mixed with solution A to make a mixed solution with a total volume of 1.00 L. Kw = 1.00x10-14; Ka(HF) = 6.6x10-4 at T=298K. (a) If solution A is 0.50 L 0.20 M HNO3, calculate the pH of the mixed solution. Ka(HNO3) = 100 (b) If solution A is 0.50 L 0.20 M NH4CI, calculate the pH of the mixed solution. Ko(NH3) = 1.8×10-5 %3D (c) If solution A is 0.50 L 0.20 M HNO2, calculate the pH of the mixed solution. Ka(HNO2) = 5.1×104 Hint: First list an equation that shows electrical neutrality in the solution. Also, neglect the [H*] contribution from water. Then use [H*] and the equilibrium constant(s) to express the anion concentrations in the equation you obtained for electrical neutrality, and you will find there is single unknown [H*] in the equation.

Methylamine (CH3NH2) has Kb = 4.4 x 10–4. What is the pH of 0.15 M aqueous solution of methylamine?           (A) 1.68            (B) 2.09            (C) 11.91          (D) 13.18

Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e – 04) at a 1.800 M concentration, with 115 mL of a 1.400 M solution of C'sOH ? O (a) 3.250 O (b) 1.696 O (c) 3.392 O (d) 3.192 O (e) 0.308

Consider 1.3 M HNO2 solution. (a) Show the reaction of dissociation (ionization) of HNO2.  (b) Calculate the [H+] in the solution. (c) Calculate the pH of the solution.

Calculate the pH of solutions having the following [H+]: (a) 0.0055 M (b) 1.54 x 10-8 M (c) 3.47 M

Calculate the pH of solutions having the following [H+]: (a) 0.68 M (b) 1.42 M (c) 4.5 × 10-5 M