calculate the ph of a .36 M of ethylamine and .52 M methylammonium bromide. the base...

calculate the ph of a .36 M of ethylamine and .52 M methylammonium bromide. the base dissociation constant kb oa 5.6 x10^-4

a) what is the ph of 39 mL offf .60 M offf a strong acid like HCl is added to 100 mL is the buffet solution?

b) what if a strong base like NaOH is added with the same amount instead ?

Expert Solution

queen_honey_blossom answered 2 years ago

The pH of an aqueous solution of 0.538 M ethylamine (a weak base with the formula...

The pH of an aqueous solution of 0.538 M ethylamine (a weak base with the formula C2H5NH2) is _________

a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4)...

a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4) b. Calculate the pH of a 0.0473 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3).

Methylamine is a weak base with pKb = 3.36. Calculate the pH of a 0.010 M...

Methylamine is a weak base with pKb = 3.36. Calculate the pH of a 0.010 M solution of methylamine in water. A)3.36 B)7.00 C)10.64 D)11.26 E)12.05 Which answer is correct and show all work.

The pH of a 0.120 M solution of a weak base is 10.97 at 25ºC. Calculate...

The pH of a 0.120 M solution of a weak base is 10.97 at 25ºC. Calculate the pH of a 0.0316 M solution of this base at 25ºC.

Calculate the pH for 200. mL of a 0.750 M solution of the weak base, ethanolamine...

Calculate the pH for 200. mL of a 0.750 M solution of the weak base, ethanolamine (HOCH2CH3NH2), Kb=3.20x10-5 ) being titrated with 0.750 M HCl at the following positions in the titration. a) The initial pH (before any HCl has been added). a. 2.300 b. 3.542 c. 8.945 d. 11.690 e. 13.976 b) The pH of the solution after 75.0 mL of 0.750 M HCl has been added. a. 0.769 b. 9.727 c. 3.564 d. 8.654 e. 13.230 c)The pH...

C. Calculate the pH of a 0.10 M aqueous solution of the weak base ammonia, NH3...

C. Calculate the pH of a 0.10 M aqueous solution of the weak base ammonia, NH3 , if the degree of dissociation is 1.34%.

Ethylamine, C2H5NH2, is a weak base. 250.0 mL of a 0.160 M C2H5NH2 solution is titrated with...

Ethylamine, C2H5NH2, is a weak base. 250.0 mL of a 0.160 M C2H5NH2 solution is titrated with 0.500 M HCl (aq). Find the KbKb value in a lecture slide. Calculate the pH at the following points. 30. mL of HCl solution added. At the halfway point. At the equivalence point. Verify any assumption you made. 90. mL of HCl solution added.

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calculate the ph of a .36 M of ethylamine and .52 M methylammonium bromide. the base...

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