A common buffer for stabilizing antibodies is 100 mM Histidine at pH 7.0. Describe the preparation of this buffer beginning with L-Histidine monohydrochloride monohydrate and 1 M NaOH. Be certain to show the buffering reaction that includes the conjugate acid and base.
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A common buffer for stabilizing antibodies is 100 mM Histidine at pH 7.0. Describe the preparation of this buffer beginning with L-Histidine monohydrochloride monohydrate and 1 M NaOH. Be certain to show the buffering reaction that includes the conjugate acid and base.
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- Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Kb Ammonia NH3 NH4+ 1.8 x 10-5 Methylamine CH3NH2 CH3NH3 + 4.38 x 10-4 Ethylamine C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Aniline C6H5NH3 + 3.8 x 10-10 CH;NH, C,H,N Pyridine CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Name Formula Kb 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, 4.38 x 10-4 C₂H5NH₂ 5.6 x 10-4 Ethylamine Aniline CHẠNH, 3.8 x 10-10 Pyridine CsHsN 1.7 x 10-⁹ 2. Compute for pKb Conjugate Acid NH4+ CH;NH * C₂H5NH3+ CH,NH,* CH,NH*•The pKa for acetic acid is 4.756 and the pKa for NH4+ is 9.245. What pH do you expect for the solutions with [A-]init [HA]init? Explain this by referring to the acid = dissociation constant expressions (Ka) for NH4+ and CH3COOH as well as your answer to part (a). Do your measurements agree with your expectations (make specific reference to your experimental data and consider uncertainty)?
- Rank the following in order of increasing pH. Explain the basis of your ranking. Assume the concentrations are all 0.10 M. Attached Table Below. Piperazine Pyridine hydrochloride Phenylalanine Disodium phthalate Sodium prolinate Phosphoric acid.Calculate the concentrations of the weak acid and conjugate base for the best possible buffer at pH 3.50 knowing that the concentration of the more concentrated species between the two will be 0.2 M. Choose the buffer system you think would be best between the following three. You will need to look up literature values for the Ka/pKa on your own. Remember that a strong buffer has similar concentrations of the buffering components. Formic acid/formate Acetic acid/acetate Hypobromous acid/HypobromiteA chemist titrates 90.0 mL of a 0.5350M trimethylamine ((CH3)N) solution with 0.1600M HCl solution at 25 °C. Calculate the pH at equivalence. The pK₂ of trimethylamine is 4.19. Round your answer to 2 decimal places. ? Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = ☐ X Ś olo
- Using the table of the weak base below, you have chosen Aniline as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.71 M in this salt. The desired pH of the buffer should be equal to 3.8. Values of K₁ for Some Common Weak Bases Conjugate Acid Name Formula Kb Ammonia NH4+ 1.8 x 10-5 NH3 CH,NH, Methylamine CH3NH3 + 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3 + 3.8 x 10-10 Pyridine C,H,N CH;NH* 1.7 x 10-⁹ 3. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).A chemist titrates 120.0 ml. of a 0.7695 M trimethylamine ((CH₂)₂N) solution with 0.1789M HNO, solution at 25 °C. Calculate the pH at equivalence. The PK, of trimethylamine is 4.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO, solution added. PH-0Calculate the pH of a 0.345 M aqueous solution of acetylsalicylic acid (aspirin, HC9H7O4) and the equilibrium concentrations of the aspirin and its conjugate base. Ka = 3.0 x 10-4. Be sure to report appropriate sig figs and units. pH = [HC9H704] = [C9H704] =
- Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CH;NH, CH3NH3 + 4.38 x 10-4 C₂H5NH₂ C₂H5NH3 + 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3 + 3.8 x 10-10 Pyridine C,H,N CşH;NH+ 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (answer in 2 decimal places)The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.