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For a diprotic acid, H2A, the pKay and pKaz is 3.54 and 9.68, respectively. Which species...
4. A diprotic acid has the following pK values: pKa1 = 5.50, pKa2 = 9.50 A. At what pH does [H2A] = [HA- ]? B. At what pH doe [HA- ] = [A2- ]? C. Which is the principal species at pH = 3.50, H2A, HA- , or A2- ? Justify your answer using the Henderson-Hasselbach equation. D. Which is the principal species at pH = 7.5, H2A, HA- , or A2- ? Justify your answer (don’t use Henderson-Hasselbach equation,...
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, 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
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- ].
Consider the acid dissociation reactions and for the diprotic acid H2A: H2A(aq) + H2O (l) --><-- HA-(aq) + H3O+(aq) pKa1= 3 H2A(aq) + H2O (l) --><-- A2- (aq) + H3O+(aq) pKa2= 8 Would a salt solution of KHA be acidic, basic or neutral? a) Acidic b) Basic c) Neural
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-) =
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...
Consider the acid dissociation reactions and for the diprotic acid H2A: H2A(aq) + H2O(1) =HA (aq) + H2O+(aq) pKQ1 = 6 HA (aq) + H20(I) = A2-(aq) + H20+ (aq) pRaz = 10 Would a salt solution of KHA be acidic, basic or neutral? neutral basic O acidic
(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, 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-] =