4th question A generic version for Drug X is applying registration to the FDA. For the generic drug to be approved,it must prove bioequivalence with an innovator/originator drug. However, the company registeringDrug X is applying for an exemption for in vivo bioequivalence testing. To qualify for this exemption,one of the requirements is to prove that it can be highly soluble in an aqueous buffer of pH 1.2, 4.5, 6.8.As the drug formulator, you need to prepare these buffers to test your sample.1. For the pH 4.5 buffer, you must use acetic acid and sodium hydroxide:СНЗСООН + NaOH — NaCНЗСОО + Н20The Ka of acetic acid is 1.8 x 10-5. Using the Henderson-Hasselbalch equation, calculate the molarratio of [conjugate base]/[weak acid] that must be used in preparing the buffer.А. 0.29В. 0.57С. 0.87D. 1.142. The only remaining NaOH in the lab is 100 mL of 1.0 M NaOH solution. Given this amount, howmany moles of acetic acid must be used to prepare 1 L of the buffer.A. 0.088 molB. 0.175 molC. 0.275 molD. 0.350 mol3. If the lab has an available stock of 5.0 M acetic acid solution, how many mL of this solution must beused to obtain the calculated moles of acetic acid?A. 17.6 mL B. 35.0 mLC. 55.0 mLD. 70.0 mL4. Using the Van Slyke equation, calculate the buffer capacity, B, of the buffer to be prepared.A. 0.100B. 0.146 C. 0.200 D. 0.2355. The Ka of NaH2PO4 6.2 x 10-8. Using the Henderson-Hasselbalch equation, calculate the molarratio of [conjugate base]/[weak acid] that must be used in preparing the buffer.Α. 0.39В. О.78С. 1.56D. 2.346. There is an available 50 mL of 0.2M NaH2PO4 in the laboratory. Convert this first to the moles ofNaH2PO4. The molar mass of NaH2PO4 is 119.98 g/mol.A. 0.005 molB. 0.010 molC. 0.025 molD. 0.045 mol7. Given the number of moles of NaH2PO4 available as computed above and the molar ratio calculated,which of the following moles of NaOH when added to NaH2PO4 will produce the required bufferA. 0.0061 molB. 0.0078 molC. 0.0156 molD. 0.0390 mol8. If a readily available 0.2 M NaOH is present in the lab, how many mL of this solution will you use tosupply the calculated moles from above?А. 30.5 mL B. 39.0 mLC. 78.0 mLD. 195.0 mL

Answered: Image /qna-images/answer/20884524-c64b-4108-bd02-cb14e9da8155.jpg

1. For the pH 4.5 buffer, you must use acetic acid and sodium hydroxide: СНЗСООН + NaОН — NaCH3CO0 + H20 The Ka of acetic acid is 1.8 x 10-5. Using the Henderson-Hasselbalch equation, calculate the molar ratio of [conjugate base]/[weak acid] that must be used in preparing the buffer. A. 0.29 B. 0.57 C. 0.87 D. 1.14

1. For the pH 4.5 buffer, you must use acetic acid and sodium hydroxide: СНЗСООН + NaОН — NaCH3CO0 + H20 The Ka of acetic acid is 1.8 x 10-5. Using the Henderson-Hasselbalch equation, calculate the molar ratio of [conjugate base]/[weak acid] that must be used in preparing the buffer. A. 0.29 B. 0.57 C. 0.87 D. 1.14

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter37: Qualitative Analysis Of Group Ii Cations

Section: Chapter Questions

Problem 3ASA

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A generic version for Drug X is applying registration to the FDA. For the generic drug to be approved, it must prove bioequivalence with an innovator/originator drug. However, the company registering Drug X is applying for an exemption for in vivo bioequivalence testing. To qualify for this exemption, one of the requirements is to prove that it can be highly soluble in an aqueous buffer of pH 1.2, 4.5, 6.8. As the drug formulator, you need to prepare these buffers to test your sample. 1. For the pH 4.5 buffer, you must use acetic acid and sodium hydroxide: CH3COOH + NaOH → NaCH3COO + H2O The Ka of acetic acid is 1.8 x 10-5. Using the Henderson-Hasselbalch equation, calculate the molar ratio of [conjugate base]/[weak acid] that must be used in preparing the buffer. 0.29 B. 0.57 C. 0.87 D. 1.14 2. The only remaining NaOH in the lab is 100 mL of 1.0 M NaOH solution. Given this amount, how many moles of acetic acid must be used to prepare 1 L of the buffer. 0.088 mol B. 0.175…
The following text may be found at the ThermoFisher website: "PBS (phosphate buffered saline) is a pH-adjusted blend of ultrapure-grade phosphate buffers and saline solutions which, when diluted to a 1X working concentration, contains 137 mM NaCl, 2.7 mM KCl, 8 mM Na2HPO4, and 2 mM KH2PO4. Each 10X PBS solution is ready to use upon dilution to the desired concentration." This means that the product that you purchase has a concentration 10 times the concentration at which it is used. 1. Look up the pKa values for phosphoric acid and list them as a part of your response. 2. Based on the description of the contents of the PBS buffer, calculate the pH of the 1X solution. 3. Assume that you wish to use a pH = 7.00 buffer. If your answer to 2 was more acidic than pH 7.00, calculate how much 1.00 M NaOH you would need to add to get to pH = 7.00. If your answer to 2 was more basic than pH 7.00, calculate how much 1.00 M HCl you would need to add to get to pH = 7.00.
) A truck driver carrying a load of lead nitrate (Pb(NO3)2) lost control of his semi- truck after hitting a patch of ice and crashed the truck into Blue Lake, which was right next to the highway. Despite the best efforts of the emergency workers, several of the crates containing lead nitrate were damaged, and the highly soluble compound dissolved immediately. Assuming the lake is initially at circumneutral pH (7), and that the spill resulted the in a total lead concentration of 10-3 M within the lake. Based on the following information, will PbO(s) precipitate out of Blue Lake. Assume all lead nitrate dissociates into Pb+2 and NO3-, no other sources of lead exist in the lake and that no other reactions besides the equations shown below occur. PbO(s) + 2H+ ⇌ PbO(s) + H+ ⇌ PbO(s) + H2O ⇌ PbO(s) + 2H2O ⇌ Pb2+ + H2O PbOH+ + H2O Pb(OH)2o Pb(OH)3- + H+ logKs0/ksp =14 logK1=3.4 logK2=-0.5 logK3=-12
0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.
Part b As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the potential to kill weeds effectively. A sparingly soluble salt, Herbigon is dissolved in 1 M acetic acid for technical reasons having to do with its production. You have determined that the solubility product Ksp of Herbigon is 9.00×10-6 Although the formula of this new chemical is a trade secret, it can be revealed that the formula for Herbigon is X-acetate (XCH COO, where "X" represents the top-secret cation of the salt). It is this cation that kills weeds. Since it is critical to have Herbigon dissolved (it won't kill weeds as a suspension), you are working on adjusting the pH so Herbigon will be soluble at the concentration needed to kill weeds. What pH must the solution have to yield a solution in which the concentration of X* is 4.00×10-3 M? The pKa of acetic acid is 4.76.
A 1L buffer solution needs to be prepared. The buffer will be composed of the following, 200mM tris, 400mM glycine, and 0.5% (w/v) glycerol. The stock reagents for tris (124.14g/mol) and glycine (75.07g/mol) are stored as separate lyophilized powders. Glycerol is stored as a liquid at 20% (w/v). Approximately how many mL of glycerol should be measured for this buffer?
Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)
A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts): Assume that Calcium Iodideand Sodium Oxalate are the starting substances (reactants) in the reaction: a. Write a balanced chemical equation describing the formation of kidney stones, using the information in the case study. b. State the names of the products that are produced from this reaction. c.…
A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts): Assume that Calcium Iodideand Sodium Oxalate are the starting substances (reactants) in the reaction: a. Write a balanced chemical equation describing the formation of kidney stones, using the information in the case study. b. State the names of the products that are produced from this reaction. c.…
A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts): Assume that Calcium Iodideand Sodium Oxalate are the starting substances (reactants) in the reaction: a. Write a balanced chemical equation describing the formation of kidney stones, using the information in the case study. b. State the names of the products that are produced from this reaction. c.…
A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts):
A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts): Assume that Calcium Iodideand Sodium Oxalate are the starting substances (reactants) in the reaction: a. Write a balanced chemical equation describing the formation of kidney stones, using the information in the case study. b. State the names of the products that are produced from this reaction. c.…