A researcher is preparing a reaction mixture to test the activity of a protein. They combine the required reaction components, which contained in a final 100ml reaction volume 200mM NaCl, unknown concentrations of acetic acid and acetate anions and a total [H^+] concentration of 64 nanomolar. Can you determine the pH of the solution. Provide your answer to once decimal place. Note: you may need to round the numbers to get the required answer.
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A researcher is preparing a reaction mixture to test the activity of a protein. They combine the required reaction components, which contained in a final 100ml reaction volume 200mM NaCl, unknown concentrations of acetic acid and acetate anions and a total [H^+] concentration of 64 nanomolar. Can you determine the pH of the solution. Provide your answer to once decimal place. Note: you may need to round the numbers to get the required answer.
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- Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answer2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he 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 KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey 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 sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Kb Ammonia NH3 NH4+ 1.8 x 10-5 Methylamine CH3NH2 CH3NH3 + 4.38 x 10-4 Ethylamine C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Aniline C6H5NH3 + 3.8 x 10-10 CH;NH, C,H,N Pyridine CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)
- You have a 12 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.14. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.55. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 12 mL sample. Acetycholine in original sample:________ nmolYou have a 11 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.22. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.62. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 11 mL sample. CH,—C−O−CH,—CH,—*N-CH, Acetylcholine CH3 acetycholine in original sample: I CH₂ H₂O CH₂ HO–CH,—CH,—*N–CH, + CH,-C−O + H* CH₂-8-0 Choline | CH3 Acetate nmolUsing the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Name Formula Kb 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, 4.38 x 10-4 C₂H5NH₂ 5.6 x 10-4 Ethylamine Aniline CHẠNH, 3.8 x 10-10 Pyridine CsHsN 1.7 x 10-⁹ 2. Compute for pKb Conjugate Acid NH4+ CH;NH * C₂H5NH3+ CH,NH,* CH,NH*
- This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 3.08 Calculated pH Answer these questions. 1. As the H+ Molarity increases, what happens to the pH ? 2.15This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100 % ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.001 M Experimental pH (given) 1.20 Calculated pH Answer these questions. 1. As the H+ Molarity increases, what happens to the pH ? 2. As the H+ Molarity increases does the solution become more acidic or more basic? 0.01 M 2.15 3.08This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCl pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 Calculated pH Answer these questions. 2.15 3.08 As the H+ Molarity increases, what to the pH ? As the H+ Molarity increases does the solution become more acidic or more basic? 3. Give a specific reason(other than general human error) why the calculated pH…
- This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.001 M Experimental pH (given) 1.20 Calculated pH Answer these questions. 1. As the H+ Molarity increases what happens to the pH2 2. AST + Molarity in basic? alues are a pH meter. 0.01 M 2.15 3.08 ore AYWhich solution is more acidic and how do you know that, based on the pH easurements)? 4. Given…This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 2.15 3.08 Calculated pH Answer these questions. what happens to the pH ? As the HF Molarity increases does the solution become more acidic or more basic? calculated pr not exactly the same as the experimental values obtained by measuring with a primeter.…You have a 15 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.06. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 5.91. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 15 mL sample. O= CH3 Acetylcholine H₂O CH,—C−O−CH,—CH,—*N-CH, → HO−CH,—CH,—*N–CH, + CH,—C−O + H* CH3 CH 3 Choline CH3 Acetate