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5) Calculate the pH of the following solutions a) 2.5 x 10 M HCI c) 9.5...
Which of the following solutions is the most basic ? 0.1 M HCI a solution PH=9.5 a solution POH=8.5 a solution with [OH-] = 1.0 x 10-11 M a solution with (H+) -1.0 x 10-6 M Calculate the equilibrium constant (K) for a balanced redox reaction that involves 6 electrons and has AG= 410000 joules at 25°C. a. 1.4 * 1072 b.8.9 x 10-73 C.1.35 x 10-72 d. 1,5x1024 0.4.6 x 10 31
. Calculate the pH of the following solutions: a. 1.00 x 6 M HCI b. 3.25 x 104 M HOC c. [OH]-1.0 x 103 10
Calculate the pH of the following solutions at 25 ℃ a) 1.0×10-5 M HCI c) 1.0×10-5 M NaOH Number Number pH b) 0.01 M HNO, d) 0.1 M KOH Number Numbero pH-
14. Calculate the [H,0+and the pH of each solution. a. 1 x105 M HCI c. 1 x 10-1 M H,SO, b. 5 x 103 M HC1 d. 1 105 MH,SO, 15. Calculate the (OH) and the pOH of each solution in problem 14. (-16. What is [H,O+] in each of the following solutions? a. orange juice, pH = 4.0 b. black coffee, pH = 5.0 c. pure water, pH = 7.0 d. phosphate detergent solution, pH = 9.5 e. seawater,...
Calculate the pH of each of the following solutions. (a) 2.5 x 10-4 M Ba(OH)2: Enter your answer in scientific notation.) (b) 6.3 x 10 MHNO3:
Calculate the pH of each of the following solutions. (a) 1.3 x 10-4 M Ba(OH)2: x 10 (Enter your answer in scientific notation.) (b) 1.7 x 10-4 M HNO3: Calculate the pH of a 0.025 M CHEN (pyridine) solution. The K, for pyridine is 1.7 x 10 9. pH =
8.99 x 10-7 M d. [Ht 1-1.89 x 10-10M fm 45 Calculate the pH corresponding to each of the pOH values listed, and indicate whether cach solution is poll = 4.32 c. pOH-1.81 pOH-8.90 d. pOH 13.1 .49 Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH . pH = 9.01 c. pH-1.02 . pH 6.89 d. pH 7.00 6.58 Calculate the pH of each of the following solutions of strong acids....
1. Calculate the pH of each of the following solutions and determine whether the solutions are neutral, acidic, or basic. a. [H] = 4.8 x 10-M b. [OH-] = 2.5 X 10M c. [OH-] = 3.2 X 10M
Calculate the pH and pOH of the solutions with the following hydronium ion [H3O+] or hydroxide ion [OH–] concentrations. Determine which solutions are acidic, basic or neutral. (1.a) [OH–] = 8.2 × 10–11 M (1.b) [OH–] = 7.7 × 10–6 M (1.c) [H3O+] = 3.2 × 10–4 M (1.d) [H3O+] = 1.0 × 10–7 M
5. (8 points) Calculate the pH of each of the following aqueous solutions at 25 °C. a. 0.65 M boric acid (B(OH), K. = 7.3 x 10-19) b. 3.15 M ammonia (NH3, Kb = 1.76 x 10) c. 0.82 M benzoic acid (CHCOOH, K. = 6.3 x 10) d. 0.100 M H,AsO. (K.1 = 2.5 x 10^, K2 = 5.6 x 10*, K3 = 3.0 x 10-13)