A 0.324 M solution of a weak base (B:) is made. The Kb for this acid...
1) A 0.224 M solution of a weak acid (HA) is made. The Ka for this acid is 7.73 ⋅ 10-5 . -What is the pH of this solution? -What is the pOH of this solution? 2)A 0.238 M solution of a weak base (B:) is made. The Kb for this acid is 7.34⋅10-3. -What is the pOH of this solution? -What is the pH of this solution?
For a weak base (B), a 0.0100 M and a 0.100 M solution was made. Students obtained the following pH value for the solution. Fill in the table. Report all answers (except pH or pOH values) in scientific notation. 0.0100 M B 0.100 M B pOH 4.32 3.48 [OH-] [BH+] [B] (at equilibrium) Kb For the same solution fill out the following information: 0.0100 M B 0.100 M B pH (Do not...
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
If a buffer solution is 0.100 M in a weak base (Kb = 5.0 * 10%) and 0.490 M in its conjugate acid, what is the pH? Number pH = 18.6
a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ...
If a buffer solution is 0.210 M in a weak base (Kb = 4.9 × 10 − 5 M) and 0.480 M in its conjugate acid, what is the pH?
If a buffer solution is 0.170 M in a weak base (Kb = 8.5×10−5 M) and 0.480 M in its conjugate acid, what is the pH?
If a buffer solution is 0.240 M in a weak base (Kb = 8.9 × 10-5) and 0.420 M in its conjugate acid, what is the pH?
If a buffer solution is 0.220 M in a weak base (Kb = 8.1 × 10-5) and 0.540 M in its conjugate acid, what is the pH?
If a buffer solution is 0.290 M in a weak base (Kb = 7.3 × 10-5) and 0.470 M in its conjugate acid, what is the pH?