Calculate the pH of each of the following aqueous solutions at 25 °C. (Please help me solve #4 with your work, and check my answers for #1-3, if incorrect please show me why, Thank you)
1) 0.65 M boric acid (B(OH)3, Ka = 7.3 x 10-10) (pH=4.66)
2) 3.15 M ammonia (NH3, Kb = 1.76 x 10-5) (pH= 4.37)
3) 0.82 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) (pH=2.14)
4) 0.100 M H3AsO4 (Ka1 = 2.5 x 10-4, Ka2 = 5.6 x 10-8, Ka3 = 3.0 x 10-13) (Please help with this question)
Calculate the pH of each of the following aqueous solutions at 25 °C. (Please help me...
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)
pelase help 5. (8 points) Calculate the pH of each of the following aqueous solutions at 25 C 0.65 M boric acid (B(OH), K,-7.3 x 10") a. 3.15 M ammonia (NH, K.- 1.76 x 10) b. c. 0.82 M benzoic acid (CaH,COOH, K.-6.3 x 10) 0.100 M HASO4 (K,-2.5 x 10, Ke 5.6 x 10, K-3.0 x 10) d. (2 points) Determine whether each of the following salts are acidic, basic, or neutral. 6. a. Na SO b. CH NH...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the pH of the solution? Calculate the Ka of the acid. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? (2 points) Determine the percent ionization of a 0.0028 M HA solution. (Ka of HA = 1.4 x 10-9) (4 points) Lysine is triprotic amino acid (separately loses three H’s in...
46. What is the percent ionization of a 0.491 M aqueous solution of carbonic acid? Ka1= 4.2x10^-7; Ka2= 4.8x10^-11 47. What is the percent ionization of a 0.356 M aqueous solution of hydrosulfuric acid? Ka1= 9.5x10^-8; Ka2= 1x10^-19 48. What is the pH of a 0.387 M aqueous solution of acetic acid? Ka (CH3COOH) = 1.8x10^-5 49. What is the pH of a 0.0398 M aqueous solution of benzoic acid? Ka (C6H5COOH) = 6.5x10^-5 50. What is the pH of...
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2620 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2380 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M
5. Calculate the pH at 25°C of a 0.85 M aqueous solution of phosphoric acid (H3PO4). 5. (Ka1, Ka2, and Ka3 for phosphoric acid are 7.5 × 10−3, 6.25 × 10−8, and 4.8 × 10−13, respectively.)
Please help me figure out how to solve a problem like this: Using initial conjugate acid and conjugate base concentrations of 0.100 M Benzoic Acid (C6H5COOH), show that the pH calculated using a Ka expression is the same as the pH calculated using a kB expression.
Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M disodium maleate. The Ka values for maleic acid are 1.20 x 10 (Ka1) and 5.37 x 10-7 (Ka2) 1.8 pH A solution containing 0.0306 M succinic acid and 0.019 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 105 (Kal) and 2.31 x 10 (Ka2) pH
Calculate the pH of a 0.496 M aqueous solution of benzoic acid (C6H5COOH, Ka = 6.3×10-5) and the equilibrium concentrations of the weak acid and its conjugate base. pH = _____ [C6H5COOH ]equilibrium = _____M [C6H5COO- ]equilibrium = _____M