2. Phoebe was tasked to ensure that an enzyme responsible for keeping her species from extinction remains biologically active. To do so, she needs to store it in a buffer solution with a pH of10.00. Unfortunately, only three buffer systems are available in their laboratory:Buffer System Weak Acid Component K₂Conjugate Base SaltPAHBenzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COOSADBoric acid, H3BO35.81 x 107 NaH₂BO3DOHHydrogen cyanide, HCN 6.20 X 10-10 NaCNA. In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme?In your solution sheet, show calculations and briefly explain to support your answer.B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheetC. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.

Answered: Image /qna-images/answer/640df177-d820-4c9e-8ae3-3b9afbcb0442.jpg

2. Phoebe was tasked to ensure that an enzyme responsible for keeping her species from extinction remains biologically active. To do so, she needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component K₂ Conjugate Base Salt PAH Benzoic acid, C6H5COOH 6.25 x 10-5 NaCH₂COO SAD Boric acid, H3BO3 5.81 x 107 NaH2BO3 DOH Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.

2. Phoebe was tasked to ensure that an enzyme responsible for keeping her species from extinction remains biologically active. To do so, she needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component K₂ Conjugate Base Salt PAH Benzoic acid, C6H5COOH 6.25 x 10-5 NaCH₂COO SAD Boric acid, H3BO3 5.81 x 107 NaH2BO3 DOH Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________
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Calcium hydroxide, Ca(OH)2, dissolves in water to the extent of 1.78 g per liter. What is the value of Ksp for Ca(OH)2? Ca(OH)2(s)Ca2+(aq)+2OH(aq)
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Suppose you are asked to prepare a buffer solution for an upcoming experiment using stock solutions of the weak acid and its conjugate base. Use the following information to determine the volumes of weak acid, conjugate base and distilled water you will need to make the buffer solution: You have 1.0 M stock sodium hydrogencarbonate (NaHCO3) solution, pKa=10.33 You also have 1.0 M stock disodium carbonate (NaCO3) solution The final buffer solution should have a concentration of 80 mM, a volume of 500 mL, and a pH of 9.60 First, use the HH equation to calculate the ratio of the two stock solutions you will need to mix together to reach the target pH, and report this ratio. Next, calculate and report the volumes of weak acid, conjugate base and dH2O you will need to prepare the buffer. No sample calculation is necessary. Hints: • Calculate the volume of distilled water by considering the HA and A- stock solutions as a single mixture of 1.0 M buffer. This way, it's easier to calculate the…
1) For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K, data in the ALEKS Data tab. Does solubility change with pH? highest solubility compound pH = 4 pH = 6 pH = 7 O yes KCI O no O yes ABCN O no O yes PBCI, O no 2) Suppose a 500. mL flask is filled with 2.0 mol of N, and 1.0 mol of NO. The following reaction becomes possible: N, (g) +0,(g) = 2NO(g) The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. OM PLEASE PLEASE PLEASE ANSWER ALL!
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