The diprotic acid, H2A, has Ka1 i.e. (K1) = 1.00 X 10-4 and K2 = 1.00 X 10-8.
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], [HA- ] and [A2- ].
The diprotic acid, H2A, has Ka1 i.e. (K1) = 1.00 X 10-4 and K2 = 1.00...
(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).
10-4. Consider the diprotic acid H A with Ki = 1.00 X 10" and K = 1.00 X 10 8. Find the pH and concentrations of H2A, HA", and A2- in (a) 0.100 M H2A; (b) 0.100 M NaHA;
A diprotic acid, H2A, has acid dissociation constants of Ka1=1.01×10−4 and Ka2=4.08×10−12. Calculate the pH and molar concentrations of H2A, HA−, and A2−at equilibrium for each of the solutions. A diprotic acid, H, A, has acid dissociation constants of Kal = 1.01 x 104 and K22 = 4.08 x 10-12. Calculate the pH and molar concentrations of H, A, HA, and A? at equilibrium for each of the solutions. A 0.176 M solution of H, A. pH= pH = 1...
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
A diprotic acid, H,A, has acid dissociation constants of Ka1 = 4.05 x 10-4 and Ka2 = 4.12 x 10-". Calculate the pH and molar concentrations of H,A, HA, and A2- at equilibrium for each of the solutions. A 0.133 M solution of H, A H,A= pH 0.126 2.15 м A2- HA- М 4.12 x10-11 7.14 x10-3 М A 0.133 M solution of NaHA H,A pH= HA- A2-1 |м м A 0.133 M solution of Na, A H,A= |м pH...
For the diprotic weak acid H2A, Kal = 2.8 x 10-6 and K2 = 6.5 x 10-9. What is the pH of a 0.0400 M solution of H,A? pH = What are the equilibrium concentrations of H, A and A2- in this solution? [HA] = [A-] =
Given a diprotic acid, H2A, with two ionization constants of Ka1 = 3.5× 10–4 and Ka2 = 5.7× 10–12, calculate the pH for a 0.113 M solution of NaHA. PH=
For the diprotic weak acid H2A, Ka1 = 2.7 × 10-5 and Ka2 = 5.2 × 10-7. What is the pH of a 0.0550 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 3.1 × 10-5 and Ka2 = 8.2 × 10-7. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
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?