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- A. What two compounds would be best to use in preparing a pH 9.0 buffer solution? justify your answer. Assume you have the acids and the sodium salts of their conjugate bases available to you. Answer: The two compounds best fo preparing a buffer solution with a pH of 9.0 would be hydrocyanic (HCN) and phenol (HOc6H5) because their pKa values are 9.40 and 9.80 respectively making their pH levels the closest to 9. B. WHat mass ration of sodium to acid is needed to prepare this buffer? C. Can this buffer solution better resist pH changes from a string acid addition or strong base addition?Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2—Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 × 10−6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer?An employer is interviewing 4 applicants for a job as a laboratory technician and askseach of them how to prepare a buffer solution with a pH close to 11.000.Use these ka’s to help you: Show your workPropionic Acid, CH3CH2COOH, ka = 1.34 x 10-5 Ethanamine, CH3CH2NH2, kb = 6.3 x 10-4 Jung says he would mix CH3CH2COOH & CH4CH3COOHDominique says she would mix CH3CH2 NH2 & CH3CH2COOHJoshua says he would mix CH3CH2COOH & CH3COONaKyla says she would mix CH3CH2NH2 & CH3CH2NH3BrWho would you hire based on their ability to make a buffer?_________________________
- You are to prepare 100. mL of an acetate buffer of pH 5.00 using 1.0 M acetic acid (CH3CO2H, also written as HC2H3O2) and solid sodium acetate (NaC2H3O2). To prepare for the investigation, complete the following calculations. The pKa for HC2H3O2 is 4.74. The Henderson-Hasselbach equation is pH = pKa + log ([conjugate base]/[acid]) (a) What ratio of [NaC2H3O2] to [CH3CO2H] is required for a pH = 5.00? (b) You will want the concentrations relatively dilute, so use an acid concentration of 0.10 M. What volume of 1.0 M CH3CO2H would be needed to prepare 100. mL of buffer with the desired concentration of 0.10 M? Use M1V1 = M2V2 (c) Use the ratio from (a) and the concentration desired (discussed in (b)) to calculate how many grams of NaC2H3O2 · 3 H2O would be needed to prepare 100. mL of buffer if the acid concentration is 0.10 M?HIn(aq) + H2O(l) H3O+(aq) + In-(aq)red yellowThe acid base indicator methyl orange is red at pH values below 3 and is yellow at pH values above 6. Usingyour knowledge of pH, indicators and pKa values, predict the pKa of methyl orange.1) In a 0.1 M solution of a weak acid, 35% of the weak acid is dissociated. The solution has a pH=3.5. Calculate the pK. 2) You want to use acetic acid (pka=4.75) and NaOH to prep 1 liter 0.1 M buffer solution with a pH= 5.0. Keeping in mind that conc of acetic acid + conc of acetate= 0.1 M, how many moles of acetic acid and NaOH would you need to add to 1 L of water?
- describe the curve and why pH = pka at half equivalence pointMethodolody: (Include a short summary of the overall experimental plan you are going to run. You may use flow chart or bullet form for this part. Sketches of any experimental set-ups used in the experiment or the workup procedures). Preparation of buffers Prepare 250ml of the following buffer solutions. Concentration Buffer solution pka Desired ph 0.50 M Phosphate 2.12 3.03. Calculate the pH of the 0.02M 2-aminophenol ampholyte considering that 2-aminophenol has pka1 = 4.78, pKa2 = 9.97.Calculate the concentrations of all species in solution. 4. If you have 25 mL of the 2-aminophenol base and titrate with 0.015M perchloric acid and the volume at the first equivalence point is 10.9 mL. Calculate the reaction constant, and the concentration of the base in the system.
- A physician wishes to prepare a buffer solution at pH = 3.82 that efficiently resists changes in pH yet contains only small concentrations of the buffering agents. Determine which one of the following weak acids, together with its sodium salt, would probably be best to use: m-chlorobenzoic acid, Ka= 1.04 × 10-4 ; p-chlorocinnamic acid, Ka=3.89 × 10-5 ; 2,5-dihydroxybenzoic acid, Ka = 1.08 ×10-3 ; or acetoacetic acid, Ka= 2.62 × 10-4 . Explain.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.The normal pH of blood is 7.40 6 0.05 and is controlled in part by the H2CO3/HCO3- buffer system.(a) Assuming that the Ka value for carbonic acid at 25oC applies to blood, what is the [H2CO3]/[HCO3-] ratio in normal blood?(b) In a condition called acidosis, the blood is too acidic. What is the [H2CO3]/[HCO3-] ratio in a patient whose blood pH is 7.20?