Question 4 (2 points) The pH of a solution of 1.1 MH2A (Kal = 1.0 x...
Q. The pH of a solution of 1.1M H2A (Ka1 = 1.0 x 10^-6 an Ka2 = 1.0 x 10^-10) is: a. 10.00 b. 5.96 c. 11.02 d. 2.98 e. None of these
Calculate the OH and the pH of a solution with an (H] = 1.1 x 10-8 M at 25 °C. [OH-] = pH = Calculate the (H+) and the pH of a solution with an [OH"] = 6.6 x 10-9 M at 25°C. pH = Calculate the (H+) and the [OH-] of a solution with a pH = 5.96 at 25 °C. [OH-] =
What is the pH for a 0.30M weak base solution with Kb 3.7 x 10-6 1) 9.5x 10-12 2) 0.0011 3) 2.98 4) 9.5 5) 11.02
Calculate the pH of a solution that is 0.0420 M in Na H2PO4 (Ka a 7.11 x 10, Ka = 6.32 x 10-) pH= NaHC204 (Kal 5.60 x 10-, Ka = 5.42 x 105) pH= Na H2PO3 (Kal = 3 x 10-2, K = 1.62 x 107) pH= NaHSO3 (Ka 1.23 x 10-, K= 6.6 x 10) pH NaHS (Kai 9.6 x 10, K- 1.3 x 10-14) pH f H2NC2 H4NH, CI (K-1.42 x 107, Kg - 1.18 x 10...
what is the answer for this? :) Calculate the pH when 200.0 mL of a 1.00 M solution of H2A(Kal = 1.0 x 10-6, K22 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. 600.0 mL of 1.00 M NaOH A) 13.40 B) 11.70 C) 14.00 D) 10.00 E) none of these
what is the answer?? Calculate the pH when 200.0 mL of a 1.00 M solution of H2A(Kal = 1.0 104, K22 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. 3. 600.0 mL of 1.00 M NaOH A) 13.40 B) 11.70 C) 14.00 D) 10.00 E) none of these
The pH of a 1.1 M solution of 4-pyridinecarboxylic acid (HC,H,NO,) is measured to be 2.46. Calculate the acid dissociation constant K of 4-pyridinecarboxylic acid. Round your answer to 2 significant digits. Ķe = 0 x 6 ?
Which of the following is most acidic? A. A solution with [H,0+] = 1.0 x 10-10 B. A solution with [H,0+] = 1.0 x 10-5 C. A solution with [OH-] = 1.0 x 10-10 D. A solution with [OH-] = 1.0 x 10-5 E. A solution with a pH of 5. Question 5 Which of the following is most basic? A. CA solution with [H,0+] = 1.0 x 10-10 B. A solution with [H0+] = 1.0 x 10-5 C. A...
Valine (HV) is a diprotic amino acid with Kal = 5.18 x 10-3 and K 2 = 1.91 x 10-10. Determine the pH of each of the solutions. A 0.288 M valine hydrochloride (H, V+Cl-) solution. pH = 1.44 A 0.288 M valine (HV) solution. pH = 5.12979 A 0.288 M sodium valinate (Na+vº) solution. pH = 11.59
For the diprotic weak acid H2A, Kal = 3.5 x 10 and K 2 = 7.9 x 10 9. What is the pH of a 0.0750 M solution of H, A? pH = What are the equilibrium concentrations of H, A and AP in this solution? [H,A] = [A-]=