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...
Part A Find the pH of a 0.120 M solution of a weak monoprotic
acid having Ka= 1.8×10−5. Part B Find the percent dissociation of
this solution. Part C Find the pH of a 0.120 M solution of a weak
monoprotic acid having Ka= 1.4×10−3. Part D Find the percent
dissociation of this solution. Part E Find the pH of a 0.120 M
solution of a weak monoprotic acid having Ka= 0.15. Part F Find the
percent dissociation of this...
Part C
Find the pH of a 0.120 M solution of a weak
monoprotic acid having Ka= 1.7×10−3.
Express your answer to two decimal places.
Part D
Find the percent dissociation of this solution.
Express your answer using two significant figures
Part E
Find the pH of a 0.120 M solution of a weak
monoprotic acid having Ka= 0.15.
Express your answer to two decimal places.
Part F
Find the percent dissociation of this solution.
Express your answer using two...
24.
A)The pH of an aqueous solution of 0.475 M
triethylamine (a weak base with the formula
(C2H5)3N) is_____?
B)The hydroxide ion concentration, [OH-], of an
aqueous solution of 0.475 M
ammonia is ___________M.