11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
show all work Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 2.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following. HA (aq) + H2O(l) ⇌ A (aq) + H3O (aq) The neutralization reaction between HA and NaOH can be expresses as the following. HA (aq) + NaOH (aq) NaA (aq) + H2O (l) Answer the following questions. A) What will be the initial...
A 0.10 M solution of a weak acid, “HA”, has a pH of 5.20. Calculate [H3O+]. Keep 2 sig figs in your answer.
ASAP! What is Ka for the weak acid, HA, if a 0.020 M solution of the acid has a pH of 3.29 at 25ºC? a. 5.1 × 10-2 b. 6.9 × 10-2 c. 2.6 × 10-4 d. 1.3 × 10-5 e. 1.0 × 10-6 What is the conjugate acid of H2PO4–(aq)? a. H3O+ b. H3PO4 c. HPO42– e. PO43–
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 50.00 mL sample of a 0.150 M aqueous solution of a weak acid HA is titrated with a 0.300 M aqueous solution of NaOH. At which point in the titration will the pH of the solution equal pKa of the acid? a) After addition of 50.00 mL of the NaOH solution b) After addition of 25.00 mL of the NaOH solution c) After addition of 12.50 mL of the NaOH solution d) After addition of 6.25 mL of the...
15. 50 ml of a solution which is 0.050 M in the acid HA, pKa = 3.80 and 0.10 M in HB, pKa = 8.20, is titrated with 0.2 M NaOH. Calculate the pH (a) at the first equivalence point and (b) at the second equivalence point.
The weak acid HA has a Ka of 4.5×10−6. If a 1.4 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HA(aq)+H2O(l)⇋H3O+(aq)+A−(aq)
A weak acid (HA) has a pKa of 4.468. If a solution of this acid
has a pH of 4.736, what percentage of the acid is not ionized?
(Assume all H in solution came from the ionization of HA.)
A weak acid (HA) has a pKa of 4.161. If a solution of this acid has a pH of 4.140, what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)