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.

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.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 110AE: The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica...

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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 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*
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)
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 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 pH ? 2. As the H+ Molarity increases does the solution become more acidic or more basic? 0.01 M 2.15 3.08
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.…
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 ? 2.15
a) Acetic acid is a weak acid that dissociates into acetate ion and hydronium ions in solutions: CH3COOH(aq) + H2O(l) ⇌ H3O+(aq) + CH3COO-(aq) The value of the dissociation constant (Ka) for acetic acid is 1.78×10-5. If you require a buffer of pH 5.25, what would be the ratio of [CH3COO-]/[CH3COOH] that you would use? A 0.316 B 3.16 C 4.15 D 0.415 b) If you need to prepare a buffer with a pH of 8.8, which one of the following acid/conjugate base pairs would you choose? A HCN / KCN B HF / KF C CH3COOH / NaCH3COO D HClO / NaClO
Please round to 2 decimal places - my original answer was 4.29 which was marked incorrect.
Using the table of the weak base below, you have chosen Methylamine 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 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CH;NH, CH3NH3 + 4.38 x 10-4 C₂H5NH₂ C₂H5NH3 + 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3 + 3.8 x 10-10 Pyridine C,H,N CşH;NH+ 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (answer in 2 decimal places)
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 車 Conjugate Acid Name Formula 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 Ammonia NH3 CH;NH2 CH§NH2 CH;NH2 C;H;N NH,+ Methylamine Ethylamine Aniline Pyridine CH;NH;* CH$NH;* CH;NH;* C;H;NH 1.7 x 10-9 1. Compute the pOH of the buffer solution. (Write your answer in 1 decimal place).
Kal Ascorbic acid (H₂CH₂O) is a diprotic acid. The acid dissocation constants for H₂CH₂O are K₁1 = 8.00 × 10-5 and K₁2 = 1.60 x 10-12. Determine the pH of a 0.136 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. H₂C₂H₂O] = [HC₂H₂OT] = [C₂H₂O²] = M M M