A diprotic acid, H2A,H2A, has acid dissociation constants of ?a1=4.15×10−4Ka1=4.15×10−4 and ?a2=3.73×10−12.Ka2=3.73×10−12. Calculate the pH and molar concentrations of H2A,H2A, HA−,HA−, and A2−A2− at equilibrium for each of the solutions.
A 0.176 M0.176 M solution of H2A.H2A.
pH =
[H2A]=[H2A]=
MM
[HA−]=[HA−]=
MM
[A2−]=[A2−]=
MM
A 0.176 M0.176 M solution of NaHA.NaHA.
pH=
[H2A]=[H2A]=
MM
[HA−]=[HA−]=
MM
[A2−]=[A2−]=
MM
A 0.176 M0.176 M solution of Na2A.Na2A.
pH=
[H2A]=[H2A]=
MM
[HA−]=[HA−]=
MM
[A2−]=[A2−]=
M
A diprotic acid, H2A,H2A, has acid dissociation constants of ?a1=4.15×10−4Ka1=4.15×10−4 and ?a2=3.73×10−12.Ka2=3.73×10−1...
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
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A diprotic acid, H,A, has acid dissociation constants of Ka molar concentrations of H,A, HA-, and A2- at equilibrium for each of the solutions 1.42 x 10-4 and Ka2 = 4.07 x 1012. Calculate the pH and = A 0.210 M solution of H,A H2A] = pH HA- A2- М М A 0.210 M solution of NaHA HA pH= М
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...
A diprotic acid, H 2 A , has acid dissociation constants of K a1 = 3.21 × 10 − 4 and K a2 = 5.67 × 10 − 12 . Calculate the pH and molar concentrations of H 2 A , HA − , and A 2 − at equilibrium for each of the solutions. A 0.130 M solution of H 2 A . pH = [ H 2 A ] = ? [ HA − ] = ? [...
Given a diprotic acid, H2A , with two ionization constants of ?a1=2.0×10−4 and ?a2=3.1×10−12 , calculate the pH for a 0.120 M solution of NaHA.
Oxalic acid, H2C2O4 has acid dissociation constants of ?a1=5.90×10−2 and ?a2=6.40×10−5. Calculate the pH and molar concentrations of H2C2O4 , HC2O−4 , and C2O2−4 at equilibrium for each of the solutions. A 0.117 M solution of H2C2O4 A 0.117 M solution of Na2C2O4
For the diprotic weak acid H2A, Kal = 2.8 x 10-6 and Ka2 = 6.8 x 10-9. What is the pH of a 0.0550 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A2- in this solution? [HA] = [A2-) =
For the diprotic weak acid H2A, ?a1=3.0×10−6 and ?a2=7.3×10−9 . What is the pH of a 0.0500 M solution of H2A ? pH= What are the equilibrium concentrations of H2AH2A and A2−A2− in this solution? [H2A]= [A2−]=