Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH,PO4(s) and 28.0 g of Na, HPO4(s) in water and then diluting to 1.00 L. 2.82 pH = Incorrect Answer
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- Hh.83.H2SO4+ 2 NAOH 2 H2O + Na2SO4 If you require 33.35 mL of 0.541 M NaOH solution to titrate 210.1 mL of H,SO4 solution, what is the concentration of the H2SO4 solution? Type answer:Solve #4 please 65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. pH = 2.190 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = 12.6603 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = 12.6625 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. pH = ?
- Q1Question 4 Part A Calculate the pH of a buffer solution that contains 0.750 M CH₂NH₂ and 0.850 M CH₂NH₂Cl. (K. = 4.4x10-4). pH of buffer= Part B 75.0 mL of 1.15 M NaOH is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the NaOH(aq) is added? pH after NaOH added = Part C 80.0 mL of 1.20 M HNO is added to 250.0 mL of the buffer solution described in Part A. What is the pH of the solution after the HNO, is added? pH after HNO₂ added: =A 700.0 mL solution is 0.209 M CH₂CH₂CH₂COOH (K₁-1.5 x 10%) and 0.253 M NaCH-CH₂CH₂COO. What is the pH after the addition of 5.00 mL of 0.750 M NaOH? (4) 4.76 B) 4.93 4.89 4.72
- I need both hand written solution onlyChemistry Trisma (NH2C(CH2OH)3) is a weak base and is a commonly used buffer. It has a molecular weight of 121.14 g/mol and a pKa of 8.3. What is the pH of a 1.00-L solution that contains 3.01 g of Trisma and 0.030 mol of HCl?An aqueous solution contains 0.414 M ethylamine (C2H5NH2).How many mL of 0.214 M nitric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.500? Answer:_____