Calculate the pH of the following buffer solutions:
(a) a solution made by dissolving 4.550 g KH2PO4 and 1.871 g K2HPO4 in water to give 350. mL of solution.
(b) a solution made by mixing 35.00 mL 0.35 M N2H4 with 15.00 mL 0.21 M N2H5Cl.
The base dissociation constant Kb is 8.50 x 10-7 for N2H4 . Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
First calculate molarity of both KH2PO4 and K2HPO4 and then molarity equation M1V1+M2V2=M(V1+V2) and calculate pH.From formula M(V1+V2)=M1V1+M2V2, calculate M, then pH.
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.550 g...
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
6. What is the pH of a buffered system made by dissolving 17.42 g of KH2PO4 and 20.41 g of K2HPO4 in water to give a volume of 200.0 mL? The Ka2 for dihydrogen phosphate is 6.2 x 10-8 and the equilibrium reaction of interest is H2PO4 (4) + H20 <-> H30* ( HPO4 (4) 7. Determine the pH of a 0.188 M NH3 solution at 25°C. The Kh of NH3 is 1.76 x 10-5. 8. Calculate the pH of...
what is the pH of a buffet solution that is made by dissolving 16.6 g of KClO in 495 mL of .355 M HClO? (total volune is 495 mL) 1. What is the pH of a buffer solution that is made by dissolving 16.6 g of KCIO in 495 mL of 0.355 M HCIO? (You can assume the total volume is 495 mL).
A solution is made by mixing 50 mL of 2.0 M K2HPO4 and 25 mL of 2.0 M KH2PO4. The solution is diluted to a final volume of 200 mL. What is the pH of the final solution?
What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 35.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3. 9.26 9.58 8.93 11.69
4) A buffer solution is prepared by dissolving 5.40 g of ammonium chloride in 20.0 mL of water a mixing it with 35.0 mL of 10.0 Mammonia. Ky for ammonia is 1.8x10° a) What is the pH of this buffer solution b) This buffer solution is diluted with water to volume of 100.0 mL and 5.00 mL of 0.500 M HCl are added to the 100.0 mL of buffer. What is the expected pH of the buffer solution after the...
Phosphate buffer (pH range 5.8 – 8.0). Assume you have prepared two separate stock solutions: Solution A: 0.1M solution of monobasic potassium phosphate (KH2PO4) and Solution B: 0.1M solution of dibasic potassium phosphate (K2HPO4) The equilibrium: H2PO4 - H+ + HPO4 2-; pKa= 6.86 In order to get 200 mL of the desired buffer, you take 50 mL of solution A, add to it some amount of solution B, and then adjust the total volume to 200 mL by adding...
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need...
Calculate the pH of the following solutions: a) Calculate the pH of the solution obtained by mixing 20.00 mL of 1.00 M HCl with water until a volume of 2000 mL. b) Calculate the pH by mixing 5.00 mmol of HNO3 with 5.00 mmol of KOH, in a total volume of 1000 mL of solution c) Calculate the pH by mixing 5.00 mmol of C6H5COOH with 3.00 mmol NaOH, and bring up to volume 300 mL. d) Calculate the pH...
Calculate the pH of a solution made by adding 42 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water to make 300. mL of solution. Hint given in feedback. The K, for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Answer: Calculate the pH of a solution made by adding 59 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water...