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PROBLEM SOLVING 1 AND 2 ONLY
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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?Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.Provide the chemical formulas and the names of the three predominant carbonic acid species indicated by arrows in the image below: Species 1 species 2 Species 3 Explain i) how you can determine the pH range at which a weak acid/conjugate base system will display buffering properties.ii) what is the reason/logic behind the rule applied in i)? and iii) indicate the pH ranges of the carbonic acid system based on the pka values provided above. Provide the chemical equilibrium that describes the carbonic acid buffer system that exists at pH 9.3. Clearly indicate the chemical formulas, identify the weak acid and it’s conjugate base, and the names of the chemical compounds.
- 1) You are asked to prepare a buffer for a protein assay. This protein works best at a slightly acidic pH of 5.5. a. From the list of Acids and conjugate bases which pair would you pick. (The list is in the attached image) b. You are asked to make a 1M stock solu on of the Buffer, how many grams of each acid and base would you need to make a 500mL stock. c. For the experiment, the final concentra on of the buffer should be 50mM. How many mL of your stock would you need to make 2L. Hint: M1V1=M2V2The Henderson-Hasselbalch equation: a. relates the pH of a solution to the pKa and the concentration of acid and salt. b. allows the graphical determination of the molecular weight of a weak acid from its pH alone. c. is equally useful with solutions of acetic acid and of hydrochloric acid. d. employs the same value for pKa for all weak acids.The pH of a 0.2L HNO2-NO2 buffer solution was determined to be 6.23. The solution was mixed with 4,.4g of HNO2. Considering that the pKa is 4.35, the approximate pH of the new solution is 4.68. a. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1.5 M of the solution is prepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label all parts accordingly.
- Use the Henderson-Hasselbalch equation to calculate the pH of the solution prepared by dissolving 0.55 mol of a weak acid (Ka=2.77x10-5) and 0.78 mol of its conjugate base in enough water to make 1.00L of buffer solution Group of answer choices 5.478 7.44 3.577 4.709 4.405In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation of albumin. Note that the pKa is 4.73. Calculate and measure the amounts (in grams if solid and in mL if liquid) of weak acid and conjugate base needed to be able to prepare the chosen buffer system in part A above. Express your answer in useful units (that is, prepare it from practical amounts or concentrations of starting materials). Show the solution step by step.11. The titration curve for an amino acid is given below. According to this titration curve, the questions given below please reply. A)How many amino acids is this? Does it have an ionizable group? B)Each of the ionizable groups What are the pKa values? C)A good buffer of this amino acid pH ranges in which it will function as Please specify. Graph buffering zones by enclosing a rectangle on you can show. D)This titration curve is composed of amino acids whose structures are given below. which may belong. Circle your choice of the amino acid you have chosen. specify your name.
- If the stoichiometric concentrations of Ac- and HAc in Solution C were known to be 0.02816 M and 0.07104 M, respectively after mixing, then calculate the theoretical pH of Solution C after mixing. Use the literature value for the pKa of acetic acid, which is 4.77. Report your final answer to 2 decimal places. Solution C contains 20mL of buffer and 5mL of HCl.Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is 0.00298 M ethylamine and 0.00546 M ethylammonium chloride.Acetic acid’s pKa is 4.75 and nitrous acid’s pKa is 3.16. If you made one buffer of equal parts acetic acid and its conjugate base, then a second buffer of equal parts nitrous acid and its conjugate base, how would the two buffers’ pHs compare to each other? Why? Note: no math is required to address this question.