Question

In: Chemistry

Calculate the concentration of pyridine, C5H5N, in a solution that is 0.70 M pyridinium bromide, C5H5NHBr....

Calculate the concentration of pyridine, C5H5N, in a solution that is 0.70 M pyridinium bromide, C5H5NHBr. (Assume Kw is 1.0 10-14.) What is the pH of the solution?

Expert Solution

SOLUTION:

Given that, Concentration of pyridinium bromide, [C₅H₅NHBr] = 0.70 M

From ICE table:

	C₅H₅NH⁺(aq)	C₅H₅N (aq)	H₃O⁺(aq)
Initial (M)	0.7	0	0
Change (M)	-x	+x	+x
End (M)	0.7-x	x	x

We have,

K_b for C₅H₅N = 1.77 x 10^-9

Also We have, K_a x K_b = K_w

K_a x 1.77 x 10^-9 = 1.0 x 10^-14

K_a = ( 1.0 x 10^-14)/(1.77 x 10^-9 )

K_a = 5.6497 x 10^-6

Now, K_a expression is given by,

(since, x <<< 0.7) =>

That is:

Therefore, pH is given by:

queen_honey_blossom answered 2 years ago

Calculate the pH of a 0.177 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and...

Calculate the pH of a 0.177 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C5H5N]equilibrium = M [C5H5NH+]equilibrium = M

what is the pH of 0.124 M pyridine (C5H5N)?

In a buffer solution prepared from 10 mL of 3.0 M Pyridine (C5H5N) added to 20...

In a buffer solution prepared from 10 mL of 3.0 M Pyridine (C5H5N) added to 20 mL of 2.0 M Pyridine Hydrochloride (C5H5NHCl) and diluted to a total volume of 200 mL- Calculate each of the following: a. The original pH of the buffer solution b. The pH upon addition of 25.0 mL of 2.0 M NaOH to part a c. The pH upon addition of 10.0 mL of 2.0 M HCl to part b

Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.140 M pyridine, C5H5N(aq) with 0.140 M HBr(aq):

Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.140 M pyridine, C5H5N(aq) with 0.140 M HBr(aq): (a) before addition of any HBr (b) after addition of 12.5 mL of HBr (c) after addition of 20.0 mL of HBr (d) after addition of 25.0 mL of HBr (e) after addition of 37.0 mL of HBr

Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x...

Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x 10-9). Record your pH value to 2 decimal places. Calculate the pH of a 0.17 M solution of KNO2 (Ka for HNO2 = 4.0 x 10-4). Record your pH value to 2 decimal places.

Calculate the titration of 25.0 ml of 0.110M pyridine C5H5N(aq) with 0.110M HBr before the additiom...

Calculate the titration of 25.0 ml of 0.110M pyridine C5H5N(aq) with 0.110M HBr before the additiom of any Hbr, after the additiion of 12.5 mL of Hbr, after the addition of 23 mL of Hbr after the adddition of 25 mL of Hbr and after the addition of 33 mL of Hbr

Pyridine (C5H5N) is a particularly foul-smelling substance used in manufacturing pesticides and plastic resins. Calculate the...

Pyridine (C5H5N) is a particularly foul-smelling substance used in manufacturing pesticides and plastic resins. Calculate the pH of a 0.145 M solution of pyridine (Kb = .00000000140).

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide...

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide ion.

12. Calculate the pH of a buffer solution made from 0.30 M hydrofluoric acid and 0.70...

12. Calculate the pH of a buffer solution made from 0.30 M hydrofluoric acid and 0.70 M sodium fluoride after the addition of 0.08 mol of NaOH to 1.0 L of this solution. Assume no change in volume. The Ka for HF is 3.5 • 10-4. Can someone guide me through this question? The answer is below but I can figure out how they got this answer. Answer: pH = 4.01

A) Calculate the concentration of all species in a 0.490 M solution of H2SO3. B) Calculate...

A) Calculate the concentration of all species in a 0.490 M solution of H2SO3. B) Calculate the concentration of all species in a 0.165 M solution of H2CO3.