Answered: 3. Fill in the missing reagents in the…

Science

Chemistry

3. Fill in the missing reagents in the following flowchart. Ph Ph CHO Ph Br. Br Ph Ph- Ph Ph Ph- Ph Ph Ph Ph Ph -Ph

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.17QAP

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Chem. R1) In real life situation, titrations are used everyday , specially in the medical world and laboratories. In our daily living if we experienced stomach pain and bloating why is it that we need to take a drug that contains Famotidine Calcium Carbonate Magnesium Hydroxide?
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. Under normal conditions this system functions to: Maintain blood pH near physiological pH. Remove excessive H+ generated during…
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. Question 9: What would be the consequence(s) of lower than normal blood pH? Cause proteins to denature Decrease in enzyme activities Limit…
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. Question 1: What percent of the ingested aspirin is in the active form in the stomach (remember that gastric juice has a pH of ~1.5)? 0.01%…
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. Question 7: What is the purpose of the activated charcoal? Absorb the residual aspirin to prevent it from entering her bloodstream. Increase…
1.What reagent is used as the indicator for the neutralization? a)citric acid b)sodium hydroxide c)sodium citrate d)phenolphthalein 2. What is the mole ratio of NaOH to citric acid for this neutralization reaction? a)2 mole NaOH/1 mole citric acid b)1 mole NaOH/1 mole citric acid c)1 mole NaOH/2 mole citric acid d)1 mole NaOH/3 mole citric acid e)3 mole NaOH/1 mole citric acid 3.If 35.00 mL of 0.1104 M NaOH were used to reach the neutralization point, how many moles of NaOH were dispensed? a)3.154 x 10-3 mol NaOH b)1.104 x 10-4 mol NaOH c)258.8 mol NaOH d)3.864 x 10-3 mol NaOH 4. Using the above mole ratio, convert the moles of NaOH in the previous question to moles of citric acid. a)1.288 x 10-3 mol citric acid b)1.159 x 10-2 mol citric acid c)3.864 x 10-3 mol citric acid d)1.932 x 10-3 mol citric acid 5. How many grams of citric acid were neutralized in the question above? (MM = 192.12 g/mol) a)0.7425 g…
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. Question 10: Bicarbonate was an effective buffer in Molly’s situation, what else could/does serve as buffers in the body? Free amino acids…
Questions: 1. Why sodium carbonate is used to standardize HCL? 2. What happens when you add hydrochloric acid to sodium carbonate? 3. What happens if we use phenolphthalein for the standardization of HCI with sodium carbonate? 4. How do I standardize 2.5N HCI? 5.What is Sodium Carbonate?
Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science) The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets. When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic. She was rushed to the nearest Emergency Room. When she reached the hospital she was unarousable and was breathing rapidly and deeply. She was examined and lab samples were obtained. Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5. The active, and toxic at high doses, form is the protonated form. What percent of ingested and absorbed aspirin is in the active form in the blood (average pH of 7.4) under normal conditions? 0.00013% 0.13%…
1.What reagent is used as the indicator for the neutralization? a)citric acid b)sodium hydroxide c)sodium citrate d)phenolphthalein 2. What is the mole ratio of NaOH to citric acid for this neutralization reaction? a)2 mole NaOH/1 mole citric acid b)1 mole NaOH/1 mole citric acid c)1 mole NaOH/2 mole citric acid d)1 mole NaOH/3 mole citric acid e)3 mole NaOH/1 mole citric acid 3.If 35.00 mL of 0.1104 M NaOH were used to reach the neutralization point, how many moles of NaOH were dispensed? a)3.154 x 10-3 mol NaOH b)1.104 x 10-4 mol NaOH c)258.8 mol NaOH d)3.864 x 10-3 mol NaOH 4. Using the above mole ratio, convert the moles of NaOH in the previous question to moles of citric acid. a)1.288 x 10-3 mol citric acid b)1.159 x 10-2 mol citric acid c)3.864 x 10-3 mol citric acid d)1.932 x 10-3 mol citric acid 5. How many grams of citric acid were neutralized in the question above? (MM = 192.12 g/mol) a)0.7425 g…
gnment Score: 43.8% tion 16 of 16 > O Macmillan Learning molar mass: assessments.macmillanlearning.com 4.5-4.6 Homework formula: Resources Question 16 of 16-45-46 Homework Hint The identity of an unknown monoprotic organic acid is determined by titration. A 0.509 g sample of the acid is titrated with 0.194 M NaOH. What is the molar mass of the compound if 21.5 mL of the NaOH solution is required to neutralize the sample? The compound is 68.8% C, 4.95% H, and 26.2% O. What is the molecular formula of the organic acid? Check Answer 8 mol
3. Write the reaction that happens when you add HCl into a NaH2PO4/Na2HPO4 buffer solution. lution