% dissociation = (x*100)/c
26.7= x*100/6.13*10^-2
x = 1.637*10^-2
HA dissociates as:
HA -----> H+ + A-
6.13*10^-2 0 0
6.13*10^-2-x x x
Ka = [H+][A-]/[HA]
Ka = x*x/(c-x)
Ka = 1.637*10^-2*1.637*10^-2/(0.0613-1.637*10^-2)
Ka = 5.962*10^-3
Answer: 5.96*10^-3
17. In a 6.13E-2 M solution of a monoprotic acid HA, the acid is 26.7% dissociated....
PERCENT DISSOCIATION AND Ka In a 5.44x10^-2 M solution, a monoprotic acid is 32.8% dissociated. Calculate the Ka for this acid
A 0.685 M solution of a weak acid HA has a pH of 4.50. What is the percent ionization of HA in the solution? Submit Answer Tries 0/98 For the solution described above, what is the K,? Submit Answer Tries 0/98 This discussion is closed. Ote E o Type here to search 6
A monoprotic acid, HA, dissociates partially in aqueous solution. At equilibrium and 298 K, the percent dissociation of 0.50 M HA is 1.75 percent. Calculate the acid dissociation constant, Ka, of HA at 298 K. (Report your answer to 2 sig figs)
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 =
7) Calculate the K, of butanoic acid (monoprotic) if a 0.025 M aqueous solution has a pH of 3.21 at 25°C 8) trans-cinnamic acid (C,H,O, monoprotic) has a K = 3.60 x 10-5 a. Calculate the pH of a 0.020 M aqueous solution of this acid. b. Calculate the percentage of acid dissociated (i.e., in the "A" form) in this solution using your calculations in (a). CHEM 120B-Activity #3 Acids and Bases Page 5
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. Based on all the given values, complete an ice table to determine concentrations of all reactants and products. Use this equation: (for the ice table) HA + H20 (double arrow) H3O+ + A- In addition, based on the ice table, and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify...
Consider a solution containing 1.90 M HA and 0.70 M A. IF HA has a k, of 5.40E-6, what would the pH of this solution be? Submit Answer Tries 0/98 This discussion is closed. Type here to search 09 Sus esc QwO@Ovo
A buffer solution is composed of 0.380 M HA, a weak monoprotic acid, and 0.760 M NaA, the sodium salt of the acid. The solution has a pH of 4.10. What is the Ka of the weak acid, HA? tks!!!!!!!!!!!!!
You make a 0.1 M solution with acid HA, a monoprotic acid. The Ka for this acid is 1.0E-8. If HA is mixed with a 50 M NaCl solution (no common ions with HA), determine the percent ionization of HA. So I calculated that the ionic strength of the solution is equal to 0.2 and found the activity coefficent to be 0.7469. When I plugged in the values into the Ka=(activity of A- * activity of H3O+)/activity of HA equation,...
16. Formic acid (HCOOH) is secreted by ants. Calculate [H3O+] for a 1.07E-2 M aqueous solution of formic acid (K = 1.80E-4). Submit Answer Tries 0/99