(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the base at 25°C has a pH of 10.88. (Enter your answer in scientific notation.)
(b) Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH 5.19 at 25°C.
(c) Calculate the pH of a 0.011 M NaF solution. (Ka for HF = 7.1 × 10−4.)
(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the...
Determine the Kb of a weak base if a 0.52 M solution of the base has a pH of 10.68 at 25°C. Kb = ? × 10 ? (Enter your answer in scientific notation.)
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...
Be sure to answer all parts. An aqueous solution of a strong base has pH 10.88 at 25°C. Calculate the concentration of base in the solution: (a) if the base is LiOH. [LiOH] = M (b) if the base is Ba(OH)2. [Ba(OH)2] = × 10 M (Enter your answer in scientific notation.)
2. The pH of a 1.79 M solution of a weak base B is measured to be 11.64 Determine Kb of the base Determine Ka of the weak bases's conjugate acid, HB+ Determine [H+] in a 2.00 M solution of the chloride salt, HBCl M Determine the pH of a 2.00 M solution of the chloride salt, HBCl
1) The pH of an aqueous solution of 0.442 M caffeine (a weak base with the formula C8H10N4O2) is ______ 2) The hydroxide ion concentration, [OH-], of an aqueous solution of 0.442 M diethylamine (a weak base with the formula (C2H5)2NH) , Kb = 6.9×10-4, is: [OH-] = ________ M.
NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.048 M in NH4Cl at 25 °C? pH=_______?
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...
Enter your answer in the provided box. Determine the Kb of a weak base if a 0.30 M solution of the base has a pH of 11.98 at 25 ° C.
The hydronium ion concentration of an aqueous solution of 0.539 M morphine (a weak base with the formula G7Hi90N) is .. (H,01- M. In the laboratory, a general chemistry student measured the pH of a 0.539 M aqueous solution of morphine, C1,H190,N to be 10.783. Use the information she obtained to determine the K, for this base. Kb(experiment)-
Calculate the pH of a 0.20 M solution of the weak base pyridine. (C5H5N; Kb = 1.7 x 10-9). What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 ´ 10–5]