2. Phoebe was tasked to ensure that an enzyme responsible for keeping her species from extinction remainsbiologically active. To do so, she needs to store it in a buffer solution with a pH of 10.00. Unfortunately, onlythree buffer systems are available in their laboratory:Buffer System Weak Acid ComponentKaConjugate 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 toprepare 250 mL of a 0.650 M buffer pH 10.00.

Buffer solution is mixture of weak acid and salt of weak acid or weak base and salt of weak acid. It…

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 Ka Conjugate Base Salt PAH SAD DOH Benzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COO Boric acid, H3BO3 5.81 x 10-7 NaH₂BO3 Hydrogen cyanide, HCN 6.20 X 10-10 NaCN

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 Ka Conjugate Base Salt PAH SAD DOH Benzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COO Boric acid, H3BO3 5.81 x 10-7 NaH₂BO3 Hydrogen cyanide, HCN 6.20 X 10-10 NaCN

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Which of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M sodium nitrite 0.31 M ammonium bromide + 0.31 M ammonia 0.29 M hydroiodic acid + 0.23 M potassium iodide 0.16 M potassium fluoride + 0.21 M hydrofluoric acid O 0.39 M acetic acid + 0.25 M potassium acetate
GW 18b 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH. Determine: (a) pH of the acid solution before any base is added; (b) volume (in mL) of base needed to get to the equivalence point; (c) pH halfway to equivalence point; (d) pH at equivalence point; (e) pH when 0.100 mL NaOH is added beyond the equivalence point. (K₂ of HF = 7.1 × 104)
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Please solve the question step by step and way with the correct answer.
5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?
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Chemistry (Part -3) =============
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A 29.6 mL sample of 0.271 M dimethylamine, (CH3)2NH, is titrated with 0.237 M hydrobromic acid. After adding 12.9 mL of hydrobromic acid, the pH is Use the Tables link in the References for any equilibrium constants that are required.
+ pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as HA (aq) → H¹ (aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base is added, the base will react with H+, reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into H+ and A™. In both instances. [H] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: A] pH =pK₂ +log HA ▼ Part A pH = What is the pH of a buffer prepared by adding 0.607 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K₁ of HA is 5.66 x 10-7 Express the pH numerically to three…
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For different enzymes, there is an optimum pH at which the enzyme is most active. For example, for enzymes of gastric juice optimum pH 1-2, for duodenal enzymes pH 7.7, for liver enzymes pH 9.5, etc. Determine which medium (a or b) is most favorable for each of the enzymes mentioned above if the following substances are added to 1.0 liter of water: a) 0.040 mol KOH and 0.030 mol HBr; b) 4.0 10-9 mol HNO3. Neglect the change in the volume of the solution. Confirm your answer with calculations.