For a 0.0299 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw...

For a 0.0299 M aqueous solution of aniline, C₆H₅NH₂ (K_b = 7.4E-10), determine the following. K_w = 1.0E-14.

What are the major and minor species present? Include phase.

What is the major species (other than water)?

What is the minor species (other than H3O+ and OH-)?

What is the concentration of the minor species in the solution? (M)

What is the concentration of the major species in the solution? (M)

What is the concentration of H₃O⁺ in the solution? (M)

What is the concentration of OH^- in the solution? (M)

Find the pH.

Expert Solution

queen_honey_blossom answered 1 year ago

For a 0.0301 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw...

For a 0.0301 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw = 1.0E-14. What are the major and minor species present? Include phase. What is the major species (other than water)? What is the minor species (other than H3O+ and OH-)? What is the concentration of the minor species in the solution? (M) What is the concentration of the major species in the solution? (M) What is the concentration of H3O+ in the solution? (M)...

Calculate the pH of a .215 M aqueous solution of aniline C6H5NH2, Kb= 7.4x10^-10 and the...

Calculate the pH of a .215 M aqueous solution of aniline C6H5NH2, Kb= 7.4x10^-10 and the equilibrium concentrations of the weak base and it’s conjugate acid Calculate the pH of a 0.0454 M aqueous solution of triethelyene C2H5(3)N, Kb= 5.2x10^-4 and the equilibrium concentrations of the weak base and its conjugate acid

Calculate the pH of 4.55 M aniline, C6H5NH2 ( Kb = 4.0 x 10^-10)

Calculate the pH of the following: a) A 0.50 M solution of aniline (C6H5NH2) b) A...

Calculate the pH of the following: a) A 0.50 M solution of aniline (C6H5NH2) b) A 0.015 M hydrochloric acid solution c) A 0.0140 M solution of CA(OH)2 d) A 0.500 M solution of NaNO3 e) A 0.05 M Na2O Solution

You have 15.00 mL of a 0.100 M aqueous solution of the weak base C6H5NH2 (Kb...

You have 15.00 mL of a 0.100 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...

1. The pH of 0.070 M aniline (C6H5NH2) is 8.73. What are its Kb and pKb?...

1. The pH of 0.070 M aniline (C6H5NH2) is 8.73. What are its Kb and pKb? 2. What mass of potassium hydrogen sulfate is required to make 309 mL of a solution with a pH of 2.27? (The Ka of HSO4? = 0.012.) 3.What is the pKa of iodic acid if the iodate ion concentration in a 0.058-M solution of HIO3 is 0.045 M? --I got the answer 1.457 but it is marking it as wrong and im not sure...

Calculate the concentration of all species in a 0.240 M C6H5NH3Cl solution. For C6H5NH2, Kb=7.5×10−10. [C6H5NH3+],[Cl-],[C6H5NH2],[H3O+],[OH-]...

Calculate the concentration of all species in a 0.240 M C6H5NH3Cl solution. For C6H5NH2, Kb=7.5×10−10. [C6H5NH3+],[Cl-],[C6H5NH2],[H3O+],[OH-] Express your answer using two significant figures.

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.61....

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.61. a) Determine the concentration of C6H5NH3 in the solution if the concentration of C6H5NH2 is 0.200 M. The pKb of aniline is 9.13. b) Calculate the change in pH of the solution, ΔpH, if 0.387 g NaOH is added to the buffer for a final volume of 1.75 L. Assume that any contribution of NaOH to the volume is negligible.

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.47....

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.47. a) Determine the concentration of C6H5NH3+ in the solution if the concentration of C6H5NH2 is 0.200 M. The pKb of aniline is 9.13. b) Calculate the change in pH of the solution, delta pH , if 0.393 g NaOH is added to the buffer for a final volume of 1.55 L. Assume that any contribution of NaOH to the volume is negligible.

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.40....

A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.40. a) Determine the concentration of C6H5NH3 in the solution if the concentration of C6H5NH2 is 0.215 M. The pKb of aniline is 9.13. b) Calculate the change in pH of the solution, ΔpH, if 0.362 g NaOH is added to the buffer for a final volume of 1.45 L.

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