-3 A solution is prepared at 25 °C that is initially 0.40M in diethylamine ((C₂H₂)₂NH), a a weak base with K = 1.3 × 10 * ((C₂H₁)NH₂Br) Calculate the pH of the solution. Round your answer to 2 decimal places. bromide pH = 0 X and 1.2M in diethylammonium

What is the pH of a solution that is 0.25 M CH3NH2 (methylamine) and 0.43 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0  10-14.)

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.

3. H̟CO, 2Ħ+HCO,¯ K, = 4.3 × 10-7 HCO, H* + Co, K, = 5.6 × 10-" The acid dissociation constants for the reactions above are given at 25°C. (a) What is the pH of a 0.050-molar solution of H,CO, at 25°C? (b) What is the concentration of CO,- ions in the solution in (a)? (c) How would the addition of each of the following substances affect the pH of the solution in (a)? (i) HCl (ii) NaHCO, (iii) NaOH (iv) NaCl

A solution is prepared at 25 °C that is initially 0.44M in ammonia (NH,), a weak base with K,= 1.8 × 10°, and 0.16M in ammonium bromide (NH Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH =

Enter your answer in the provided box. Determine the pH of (a) a 0.20 M NH3 solution. (b) a solution that is 0.20 M NH3 and 0.35 M NH,CI. K, for NH, is 1.8 x 10-5

1. The pOH of an aqueous solution of 0.540 M acetylsalicylic acid (aspirin), HC9H7O4, is   2. The hydroxide ion concentration of an aqueous solution of 0.540 M hydrofluoric acid is     [OH-] = M.   3. The pH of an aqueous solution of 0.540 M benzoic acid , C6H5COOH is