Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has a pH of 4.39. What is the Ka of the acid? |
Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has...
Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has a pH of 4.39. What is the Ka of the acid?
Part A) Calculate the pH of a weak acid HA. The solution concentration is 0.035 M in HA. Ka=4.5*10^-6 Part B) Calculate the pH of 0.00012 M KOH solution.
Be sure to answer all parts. In a 0.25 M solution, a weak acid is 3.6% dissociated. (a) Calculate the [H30+ ], pH, [OH ], and pOH of the solution. [H30+]= M [OH]= X 10 pH = pOH = (b) Calculate Kg of the acid. KA=
Be sure to answer all parts. Calculate the Ka of a weak acid if a 0.063 M solution of the acid has a pH of 2.85 at 25 ° C. Ka = × 10 (Enter your answer in scientific notation.)
A 0.035 mol sample of a weak acid, HA, is dissolved in 437 mL of water and titrated with 0.46 M NaOH. After 28 mL of the NaOH solution has been added, the overall pH = 4.1938. Calculate the Ka value for HA. Enter your answer in the format: 1.23e-4
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+(aq) + A'(aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, Ka? Answer in scientific notation. Answer: A...
Be sure to answer all parts. In a 0.20 M solution, a weak acid is 2.6% dissociated. (a) Calculate the [H3O+], pH, [OH], and pOH of the solution. [H30+] = _ M [OH] = * 10 M pH= pOH = (b) Calculate Kg of the acid.
A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA has a pH of 1.890 at 25°C. HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq) What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =
A 0.013 M solution of a weak acid (HA) has a pH of 4.38. What is the K, of the acid? Ka = 10 (Enter your answer in scientific notation.)
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.