The pH of an acid solution is 6.00. Calculate the Ka for the monoprotic acid. The initial acid concentration is 0.010 M.
Ka =
HA <-----------> H+ + A-
pH = 6.00
[H+] = 10-pH = 10-6.00 = 1.0 x 10-6 M
at equilibrium [H+] = [A-] = 1.0 x 10-6 M
[HA] = 0.010 - 1.0 x 10-6 = 0.009999 M
Ka = [H+] [A-] / [HA]
Ka = [1.0 x 10-6] [1.0 x 10-6] / [0.009999]
Ka = 1.00 x 10-10
The pH of an acid solution is 6.00. Calculate the Ka for the monoprotic acid. The...
The pH of an acid solution is 5.48. Calculate the Ka for the monoprotic acid. The initial acid concentration is 0.010 M.
The pH of a 4.39×10-3 M solution of a weak monoprotic acid is 4.40. Calculate Ka for this monoprotic acid to three significant figures.
Calculate the Ka of a weak monoprotic acid (HA) if the pH of a 1.0 M solution is 2.3. Ka = ___
A) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 1.5×10−5. B) Find the percent dissociation of this solution. C) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 2.0×10−3. D) Find the percent dissociation of this solution. E) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 0.14. F ) Find the percent dissociation of this solution.
1. Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.9×10−5. Find the percent dissociation of this solution. 2. Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.3×10−3 Find the percent dissociation of this solution. 3. Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.19. Find the percent dissociation of this solution.
What is the pH of a 0.010 M monoprotic acid is Ka=9.5x10^-8?
a.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 1.0×10−3. b.) Find the percent dissociation of this solution c.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 0.11. d.) Find the percent dissociation of this solution.
The Ka of a weak monoprotic acid is 9.23e-11. Calculate the pH of a 0.391 M solution in water.
1a. Benzoic acid, HC7H5CO2, is a weak monoprotic acid with Ka = 6.5 × 10−5. Calculate the pH of a 0.213 M solution of this acid. Report your answer to TWO places past the decimal. 1b. Acetylsalicylic acid, HC9H7O4, is a weak monoprotic acid with Ka = 3.3 × 10−4. Calculate the pH of a 0.728 M solution of this acid. Report your answer to TWO places past the decimal. 1c. Benzoic acid, HC7H5CO2, is a weak monoprotic acid with...
The pH of a 0.14 M solution of an unknown monoprotic acid is 5.85. Calculate the Ka of the acid.