It is case of amphiprotic salt anion
VETU.. 3. Consider a hypothetical diprotic acid (H2A) with Kai-4.0 * a 0.080M solution of NaHA?...
A diprotic acid, H2A, has acid dissociation constants of Kai = 3.52 x 10-4 and Ka2 = 2.03 × 10-11 . Calculate the pH and molar concentrations of H2A, HA, and A2- at equilibrium for each of the solutions. A 0.206 M solution of H,A. pH = H2A] HA1 A 0.206 M solution of NaHA pH- [H2A] = [HA-] = A 0.206 M solution of Na,A. pH- [H2A] EA T [A21
(10) 1. The diprotic acid, H2A, has Kai i.e. (K1) = 1.00 X 10 and K2 = 1.00 X 108. a) Consider a solution of 0.100 M H2A. Calculate the pH, and calculate the following concentrations: (H2A), (HA) and (A2). b) Consider a solution of 0.100 M NaHA. Calculate the pH, and calculate the following concentrations: (H2A), CHA') and (AP).
For the diprotic weak acid H2A, Ka1 = 4.0 × 10-6 and Ka2 = 6.1 × 10-9. What is the pH of a 0.0800 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
4.0 x 10 5.1 x 10-9 and Ka2 For the diprotic weak acid H2A, Kal What is the pH of a 0.0800 M solution of H, A? pH What are the equilibrium concentrations of H, A and A2- in this solution? [H2A] М [A2- М =
Consider the titration of 100.0 mL of the weak diprotic acid H2A (0.10 M) with 0.20 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) 1. Before any NaOH is added 2. After 25.0 mL of 0.20 M NaOH is added 3. After 50.0 mL of 0.20 M NaOH is added 4. After 75.0 mL of 0.20 M NaOH is added 5. After 200.0...
Consider a diprotic acid, H2A, with the following Ka values. Ka1 = 0.01 Ka2 = 0.008 If you have a 0.01 M solution of H2A, what is [H3O+] and the pH ? Hint: The Ka values are too close together to ignore the second equilibrium.
1. Titration of a diprotic acid, H2A. Consider the titration of 50 mL of 0.02 M H2A with 0.1 M NaOH. pKa1 = 4.00 and pKa2 = 8.00. For each point in the titration, calculate [H+]. a) Before any titrant is added b) after 5 mL of titrant added c) after 6 mL titrant is added d) after 10 mL titrant is added e) after 15 mL titrant is added f) after 17 mL titrant is added g) after 20...
Consider a diporitc acid, H2A, where Kai - 2.88E-4 and Ka2 = 5.10E-9. Answer the following questions regarding this solution: If the initial concentration of the acid is 0.32M, what is the pH of the solution? Submit Answer Tries 0/98 What will the concentration of A2 be at equilibrium? Submit Answer Tries 0/98
Consider the following diprotic acid. H2AH20 Ho+HA Kal-5.0x105 +A2- The initial concentration of H2A = 1.0 × 10-5 M. HA" + H20 H30" Kai = 4.5 x 10-5 Lal 1. Since the Ka and Ka2 values are very close, treat both reactions simultaneously. (a) Determine the H3+ at equilibrium 2 Now, as a comparison, ignore the second reaction (a) Determine the [H0. 3. Is the approximation of ignoring the second reaction valid?
A student titrated a 25.00-mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of 0.1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample. (a) 9.184 x 10‒4 M (b) 3.674 x 10‒2 M (c) 7.304 x 10‒2 M (d) 7.347 x 10‒2 M (e) 1.469 x 10‒1 M