Skim the intro paragraph of Reference 4. Which buffer system from the previous question would be most appropriate for growingcells? Note: this is based only on pH ranges, not if one of the ions is hazardous to cells too.(A hypochlorous acid + sodium hypochloritenone of themC propionic acid + sodium propionateD formic acid + potassium formate Match each buffer system with the correct pH range the buffer maintains.PromptsSubmitted Answershypochlorous acid + sodium hypochlorite2.77-4.77formic acid + potassium formateO 2.77-4.77propionic acid + sodium propionate6.46-8.764.76-6.76Question 23.89-5.89

The formula for buffer ranges is Pka - 1 to pka +1 For hypochlorous acid the pka value is nearly…

Match each buffer system with the correct pH range the buffer maintains. Prompts Submitted Answers hypochlorous acid + sodium hypochlorite 2.77-4.77 I formic acid + potassium formate 2.77-4.77 propionic acid + sodium propionate 6.46-8.76 4.76-6.76 Question 2 3.89-5.89

Match each buffer system with the correct pH range the buffer maintains. Prompts Submitted Answers hypochlorous acid + sodium hypochlorite 2.77-4.77 I formic acid + potassium formate 2.77-4.77 propionic acid + sodium propionate 6.46-8.76 4.76-6.76 Question 2 3.89-5.89

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...

See similar textbooks

Similar questions

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.
QUESTION 4 Kb (NH3)-1.8 x 10-5 If we mix 20.0 ml of 0.40 M NH3 with 40.0 ml of 0.20 M HCL, the solution pH will be equal to notations) QUESTION S at equilibrium. (type your answer, do not use scientific Ka (HF) 7.2 x 104 Now we mix 15.0 ml of 0.24 M HF and 15.0 ml of 0.24 M NaOH. At equilibrium, the pH of the mixture will be equal to (type your answer, do not use scientific notations)
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%…
Moving to another question will save this response. Question 10 A esc A Moving to another question will save this response. P buffer is frequently used in biochemical experiments 0 F1 Q 2 0: F2 W 20 #3 F3 E 000 000 $ 4 F4 1: % R 5
Only typed solution
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.
Please solve! Thank you for your help!
Biology Match each weak acid with the pH value at which it would buffer. You are currently in a sorting module. Turn off browse mode or quick nav, Tab to items, Space or Enter to pick up, Tab to move, Space or Enter to drop. pH 33 pH 55 pH 99 Answer Bank hydrazoic acid (pKapKa of 4.64.6) formic acid (pKapKa of 3.83.8) acetic acid (pKapKa of 4.764.76) boric acid (pKapKa of 9.249.24) chloroacetic acid (pKapka of 2.872.87) ammonium (pKapKa of 9.259.25)
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…
Some soluble compounds are listed in the table below. Classify each compound using the checkboxes. compound H₂SO HCH₂ CO₂ NH₂ NaOH type of compound (check all that apply) strong weak strong base acid acid ionic molecular 0 0 0 weak base 0
Question 14 "A buffer solution is prepared by adding 8.80 mL of 1.47 M HBr to 199.0 mL of 0.12 M methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong base is added. What is the pH? Round your answer to 2 decimal places. Your Answer: Answer
for pH titration lab! please help