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
Aniline (C6H5NH2, Kb=4.3 x 10^-10 at 25C) is an industrially important amine used in the making...
What is the pH of a 0.200 M solution of aniline (C6H5NH2, Kb = 4.3 x 1010)?
a) Kb for aniline (C6H5NH2) is 4.3×10−10. Calculate KaKa for the C6H5NH3+C6H5NH3+ cation.. b) Calculate the pH of 0.40 MNH3 (Kb=1.8×10−5).
Aniline, C6H5NH2, is commonly used as a precursor for making dyes. Aniline is a weak base when dissolved in water. Choose the correct, balanced equation for aniline in water. a. C6H5NH2 + H20 + C6H5NH + H307 O b. C6H5NH2 + H20 ++ C6H5NH2 + OH Oc C6H5NH3 + H20 ++ C6H5NH4+ + OH O d. C6H5NH2 + H20 ++ C6H5NH3+ + OH e C6H5NH2 + H20 ++ C6H5NH2 + H307
Calculate the pH of a 5.7 M solution of aniline (C6H5NH2; Kb = 3.8 x 10^-10)
Calculate the pH of a 0.10 M solution of aniline(C6H5NH2, Kb=3.8 x 10-10.) A. 11.21 B.5.21 C. 9.42 D.2.79 E. 8.79
Find the [OH-] of a 0.28 M aniline (C6H5NH2) solution. (The value of Kb for aniline (C6H5NH2) is 3.9 x 10-10.) Express your answer to two significant figures and include the appropriate units. TE Å R O ? mo [OH-] = 1.04 • 10-5 Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining - Part B Find the pH of a 0.28 M aniline (C6H5NH2) solution. Express your answer using two decimal places. O AU O O...
Determine the pH of a 2.0 x10^-4 M solution of aniline hydrochloride (C6H5NH3Cl). Kb aniline (C6H5NH2) = 3.98 x10^-10
all questions please
WER. Write the word or phrase that best completes each statement or answer the question KT ANSWER, W, 1.2) In order for the reaction 1. the Ka of HA must be for the reaction HAHSO3" -A- H2SO to have an equilibrium constant K (greater, less than the Ka of HSOY. 12) 3) The pH of a 0.045 M KOH solution MULTIPLE CHOICE Choose the Choose the one alternative that best completes the statement or answers the question....
a. Calculate the pH of a 0.205 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H5NH2]equilibrium = M [C6H5NH3+]equilibrium = M b. Calculate the pH of a 0.0555 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C5H11N]equilibrium = M [C5H11NH+ ]equilibrium = M
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