From their Kb values, which of the following bases would be best for preparing a buffer of pH 9.00: (i) NH3 (ammonia, Kb = 1.8 3 1025), (ii) C6H5NH2 (aniline, Kb = 4.0 3 10210), (iii) H2NNH2 (hydrazine, Kb = 9.5 3 1027), (iv) C5H5N (pyridine, Kb = 1.6 3 1029)?
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From their Kb values, which of the following bases would be best for preparing a buffer of pH 9.00: (i) NH3 (ammonia, Kb = 1.8 3 1025), (ii) C6H5NH2 (aniline, Kb = 4.0 3 10210), (iii) H2NNH2 (hydrazine, Kb = 9.5 3 1027), (iv) C5H5N (pyridine, Kb = 1.6 3 1029)?
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- The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant. Determiner the ff. volume of NaOH used moles of OH- usedConsider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?
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- A buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation of albumin. Which among the following buffer solution is best fitted for said purpose? Justify your answer. A. Acetate buffer=4.73B. Tris- (hydroxymethy) aminomethane =8.08C. Phosphate buffer =7.20 Calculate and measure the amounts.