Aniline CoH5NH2, a weak base, has a Kb = 4.3 x 10-10 at 25°C. (a) What would be the pH of a 2.05 M solution of aniline? (8 pts) (b) What is the Ka of aniline's conjugate acid? (3 pts)
What is the pH of a 0.200 M solution of aniline (C6H5NH2, Kb = 4.3 x 1010)?
The pH in a 0.13 M solution of aniline (Kb=4.3×10−10). pH=8.87 Calculate the concentration of C6H5NH+3 in a 0.13 M solution of aniline. Calculate the concentration of OH− in a 0.13 M solution of aniline. Calculate the concentration of H3O+ in a 0.13 M solution of aniline.
Aniline (C6H5NH2, Kb=4.3 x 10^-10 at 25C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 3.90g of aniline in enough water to make 100mL of solution
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]
What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10) A) 5.12 B) 8.88 C) 13.18 D) 9.42 E) 10.24
1. Calculate the pH of a 0.447 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10). 2. Calculate the pH of a 0.0590 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). 3. Calculate the percent ionization of a 0.545 M solution of hydrocyanic acid.
What is the pH of a 0.25 M solution of anilinium nitrate, C6H5NH3NO3? Kb for aniline is 4.3 × 10-10.
Calculate the pH of a 5.7 M solution of aniline (C6H5NH2; Kb = 3.8 x 10^-10)
A 0.20 M solution of a base is 1.8% hydrolyzed (a = 0.018). Find Kb. Kb