Consider a diporitc acid, HA, where Ka1 = 6.37E-4 and Kay = 8.14E-9. Answer the following...
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
A diprotic acid, H,A, has acid dissociation constants of Ka1 = 2.09 x 104 and Ka2 = 3.96 x 10-11. Calculate the pH and molar concentrations of H,A, HA-, and A2- at equilibrium for each of the solutions. A 0.183 M solution of H,A pH H,A= A2-1 HA] = A 0.183 M solution of N2HA. HA pH= HA A2- A 0.183 M solution of Na, A H,A ] pH= HA A2-1 M M A diprotic acid, H,A, has acid dissociation...
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...
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- ].
A 0.685 M solution of a weak acid HA has a pH of 4.50. What is the percent ionization of HA in the solution? Submit Answer Tries 0/98 For the solution described above, what is the K,? Submit Answer Tries 0/98 This discussion is closed. Ote E o Type here to search 6
Consider a solution containing 1.30 M HA and 0.30 M A . If HA has a K, of 3.90E-3, what would the pH of this solution be? Submit Answer Tries 0/98
For the diprotic weak acid H2A, Ka1=4.0×10−6 and ?a2=5.9×10−9 What is the pH of a 0.05500.0550 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= [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 a solution containing 0.40 M HA and 0.40 MA. If HA has a ka of 4.80E-3, what would the pH of this solution be? Submit Answer Tries 0/98
For the diprotic weak acid H2A, Ka1=2.3×10−6 and Ka2=7.2×10−9. What is the pH of a 0.0400 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M [A2−]= M