Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution...
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.) (a) pH = 3.79 (b)pH = 4.15 (c) pH = 4.86
Homework Answers
Here we can see that the solution is a basic buffer solution. So we can use Henderson-Hasselbalch equation. Using this equation and getting the pkb value of aniline from chart we can easily find out the ratio asked in the question. The solution is given below.
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Consider a solution that contains both C6H5NH2 and C6H5NH3+.
Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution...
A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.65....
A buffered solution containing dissolved aniline, C6H5NH2, and
aniline hydrochloride, C6H5NH3Cl, has a pH of 5.65.
a) Determine the concentration of C6H5NH3 in the solution if the
concentration of C6H5NH2 is 0.230 M. The pKb of aniline is
9.13.
[C6H5NH3+] =
______M
b)Calculate the change in pH of the solution, ?pH, if 0.386 g
NaOH is added to the buffer for a final volume of 1.45 L. Assume
that any contribution of NaOH to the volume is negligible.
pH
=...
a. Calculate the pH of a 0.205 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10)...
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
A titration of 25.0 mL of a solution of the weak base aniline, C6H5NH2, requires 25.67...
A titration of 25.0 mL of a solution of the weak base aniline, C6H5NH2, requires 25.67 mL of 0.175 M HCl to reach the equivalence point. C6H5NH2(aq) + HCl(aq)--> C6H5NH3+ (aq) + Cl- (aq) The Kb for aniline, C6H5NH2, is 4.0 x10-10 a. What was the concentration of aniline in the original solution? b. What is the concentration of C6H5NH3+at the equivalence point (AND after equilibrium is established)? c. What is the pH of the solution at the equivalence point?
Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH = C6H5NH3+ + HCOO Which of the...
Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH = C6H5NH3+ + HCOO Which of the following is a conjugate acid-base pair? O a. C6H5NH3+ and HCOO- O b. HCOOH and C6H5NH3+ a C6H5NH2 and HCO2H هنا Od. C6H5NH3 and C6H5NH2 e. HCOO and C6H5NH2
a) Kb for aniline (C6H5NH2) is 4.3×10−10. Calculate KaKa for the C6H5NH3+C6H5NH3+ cation.. b) Calculate the...
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).
Calculate the concentration of all species in a 0.220 molL−1 C6H5NH3Cl solution. (Kb for C6H5NH2 is...
Calculate the concentration of all species in a 0.220 molL−1 C6H5NH3Cl solution. (Kb for C6H5NH2 is 7.50×10−10.) Find [C6H5NH3+], [Cl−], [C6H5NH2], [H3O+], [OH−]
1.A buffer solution is made using a weak acid, HA , that has a pKa of...
1.A buffer solution is made using a weak acid, HA , that has a pKa of 5 . If the pH of the buffer is 8 , what is the ratio of [A−] to [HA] ? 2. 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 0.320 M.. The pKb of aniline is 9.13. B. Calculate the change...
A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.58...
A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.58 A. Determine the concentration of C6H5NH+3 in the solution if the concentration of C6H5NH2 is 0.275 M. The p?b of aniline is 9.13. A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.58 . A. Determine the concentration of C6H5NH+3 in the solution if the concentration of C6H5NH2 is 0.275 M. The p?b of aniline is 9.13. B....
A buffer solution contains 0.379 M C6H5NH3Br and 0.355 M C6H5NH2 (aniline). Determine the pH change...
A buffer solution contains 0.379 M C6H5NH3Br and 0.355 M C6H5NH2 (aniline). Determine the pH change when 0.084 mol HCl is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change =__
A buffer solution contains 0.202 M C6H5NH3Br and 0.445 M C6H5NH2 (aniline). Determine the pH change...
A buffer solution contains 0.202 M C6H5NH3Br and 0.445 M C6H5NH2 (aniline). Determine the pH change when 0.114 mol HClO4 is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change =
A buffered solution containing dissolved aniline, C6H5NH2, and
aniline hydrochloride, C6H5NH3Cl, has a pH of 5.65.
a) Determine the concentration of C6H5NH3 in the solution if the
concentration of C6H5NH2 is 0.230 M. The pKb of aniline is
9.13.
[C6H5NH3+] =
______M
b)Calculate the change in pH of the solution, ?pH, if 0.386 g
NaOH is added to the buffer for a final volume of 1.45 L. Assume
that any contribution of NaOH to the volume is negligible.
pH
=...
Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH = C6H5NH3+ + HCOO Which of the following is a conjugate acid-base pair? O a. C6H5NH3+ and HCOO- O b. HCOOH and C6H5NH3+ a C6H5NH2 and HCO2H هنا Od. C6H5NH3 and C6H5NH2 e. HCOO and C6H5NH2
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