Question

In: Chemistry

1. (9 pts) Consider a buffer solution composed of C6H5NH3+ and C6H5NH2. (Kb for the amine...

1. (9 pts) Consider a buffer solution composed of C6H5NH3+ and C6H5NH2. (Kb for the amine base is 3.9 x 10-10)

a. What is the optimum buffer range for this mixture?

b. What ratio of C6H5NH2 to C6H5NH3+ would be needed to buffer a solution at pH 4.10?

c. What is the pH of a solution containing 0.35 M C6H5NH3+ and 0.45 M C6H5NH2?

d. What is the pH after addition of 0.0015 mol of HBr to 20 mL of the solution in part c?

Solutions

Expert Solution


Related Solutions

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
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 (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)...
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)...
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...
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.
Consider the titration of 60.0 mL of 0.0400 M C6H5NH2 (a weak base; Kb = 4.30e-10)...
Consider the titration of 60.0 mL of 0.0400 M C6H5NH2 (a weak base; Kb = 4.30e-10) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: a) 45.6 mL
1. ______ / (10 pts): Theoretical Buffer Solution: Preparing a 0.050 M buffered solution using a...
1. ______ / (10 pts): Theoretical Buffer Solution: Preparing a 0.050 M buffered solution using a conjugate weak acid/weak base pair. You will prepare 100 mL of buffered solution with pH = ____7___. The formal concentration of this buffer should be 0.050 F (i.e., the total concentration of the weak acid and its conjugate base is 0.050 M). (You will lose 5 points if your first attempt at these calculations in incorrect) • Record your calculations below, clearly showing all...
What is the pH of a buffer solution that is composed of a weak acid, HA...
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=8.02×10–9), and the conjugate base, A–, after 3.24 mL of 0.089 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.58 M and [A–]=0.61 M. Enter your value to two (2) decimal places.
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...
A buffer solution is composed of 1.843 g of KH2PO4 and 4.225 g of Na2HPO4 ....
A buffer solution is composed of 1.843 g of KH2PO4 and 4.225 g of Na2HPO4 . (Ka for dihydrogen phosphate ion is 6.2x10^-8.) A. What is the pH of the buffer solution? pH =_______ B.What mass of KH2PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =____
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT