A Question 13 (1 point) Retake question *A buffer solution is prepared by adding 6.02 mL of 1.11 M HI to 192.0 mL of 0.11 M methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong acid is added. What is the pH? Round your answer to 2 decimal places. Your Answer: Answer

A Question 13 (1 point) Retake question *A buffer solution is prepared by adding 6.02 mL of 1.11 M HI to 192.0 mL of 0.11 M methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong acid is added. What is the pH? Round your answer to 2 decimal places. Your Answer: Answer

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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Answer the questions by writing the correct letter of your answer. Explain your answer briefly in 1 or 2 When a strong acid is added to a non-buffered solution with a pH of 8, the pH of the solution decreases to a pH of 3. When the same strong acid is added to a buffered solution with a pH of 8, the pH of the solution will most likely a. increase b. decrease to pH 7 c. decrease to pH 3 d. remain at pH 8
A Moving to another question will save this response. Question 17 What is the pH when 0.09 L of 0.148 M HCI is added to 0.148L of 0.09 M C6H5NH2? (Kb = 3.8* 10 10) Report your answer to two decimal places A Moving to another question will save this response.
In the spooky chemistry lab, you spot a 50mL solution of 6.0M hydrochloric acid. What is the pH of this acid? Yeouch...that sure would hurt if it spilled on you! You remember from when we learned about dilutions that adding water reduces the concentration of a solution. Sweet. You decide to add 950mL of water to the solution. What is the new pH of the hydrochloric acid solution? Ok, weird one here, but this is Honors Chem, so challenges are always welcome. Yippee. So, let’s rewind back to the 50mL solution of 6.0M HCl. Let’s say that you want to dilute this solution so that it has a pH equal to exactly 7. How much water would you need to add to it in order to achieve this goal? (HINT: This is so unrealistic...which is why no chemist would ever do it...but it’s still fun to do the math & determine why it’s so crazy!)
Box 1 and 2. box 1 answer choices: higher, lower, or unchanged. box 2 answer choices: higher, lower, or unchanged.
QUESTION 2 10 points Save Answer Calculate the pH of a solution prepared by mixing 20.5 mL of a 0.500 M sodium flouride solution with 32.5 mL of a 0.750 M hydrofluoric acid solution. Use the pka calculated from question 1.
Hoping for complete solutions since I’m having a hard time with this. Pls skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced What is the pH when:a. 0.15 mL of 1 M NaOH has been added to 30.0 mL of 0.10 M NH3? b.0.15 mL of 1 M HCl has been added to of 30.0 mL 0.10 M NH3? c. 0.15 mL of 1 M NaOH has been added to 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl buffer soln d. 0.15 mL of 1 M HCl has been added to 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl buffer soln with Ka or Kb of 1.8*10-5
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. 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%…
We used 0.001M of HCl
Change the top option to a Base and repeat the table for 0.001, 0.01, 0.1 and 1 for the base filling in the table below. Acid Base Initial pH Initial pH Concentration Concentration 0.001M 3.00 0.001M 11.00 0.01M 2.00 0.01M 12.03 0.1M 1.00 0.1M 13.00 1M 0.00 1M 14.00 If you were to use a calculator to do these calculations would you get the same answers? Try at least one on the acid side and one on the base side to confirm your answer.
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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…