Draw the titration curve below and the structure(s) of the major ionic form(s) of glutamic acid that exist in solution at the noted parts of the titration curve. Refer to the lecture slides for fully protonated glutamic acid and the pka. 14 PH 12 10 8 6 4 2 0 0 PK, B A pK₂=9.7 PK, Isoelectric point 1.0 2.0 Equivalents of OH™ added C Glutamic Acid (Hint: this structure is fully protonated) H H-N H O CH₂ I CH₂ I C O-H₂ PK, -H₂ pk₁ = 2.2 pK₂=4.3 3.0

Draw the titration curve below and the structure(s) of the major ionic form(s) of glutamic acid that exist in solution at the noted parts of the titration curve. Refer to the lecture slides for fully protonated glutamic acid and the pka. 14 PH 12 10 8 6 4 2 0 0 PK, B A pK₂=9.7 PK, Isoelectric point 1.0 2.0 Equivalents of OH™ added C Glutamic Acid (Hint: this structure is fully protonated) H H-N H O CH₂ I CH₂ I C O-H₂ PK, -H₂ pk₁ = 2.2 pK₂=4.3 3.0

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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A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Mass of KHP + Vial Mass of 'Empty' Vial Final Burette Reading Initial Burette Reading Determination #1 Determination #2 Determination #3 14.1992 g 14.0219 g 14.0982 g 13.3149 g 13.2301 g 13.2779 g 39.21 mL 0.49 mL 35.46 mL 0.86 mL 37.42 mL 1.59 mL How many moles of NaOH did they use in their third titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).
An unknown sample containing mixed alkali (naoh, nahco3, or na2co3) was analyzed using the double flask method. a 250 mg sample was dissolved in 250 ml co2 free water. a 20.0 ml aliquot of this sample required 11.3 ml of 0.009125 m hcl solution to reach the phenolphthalein end point. another 29.0 ml aliquot of the sample was titrated to the bromocresol green endpoint using 31.1 ml of the standard acid. how many millimoles of the components are there in the original solid sample
Determine the quantity of sodium acetate (CHCOONa) needed to create buffer solution at a particular pH. Do this by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the mass of starting material required. The value of Ka for CH,COOH is 1.8 x 10°. Complete Parts 1-3 before submitting your answer. NEXT > Sodium acetate (CHCOONa) is added to an existing 500.0 mL solution of 0.200 M CH₂COOH to form a buffer with a pH equal to 5.000. Let x represent the concentration of CH,COO in the water after the addition of CH,COONa. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. CH,COOH(aq) Initial (M) Change (M) Equilibrium (M) + x 0.200 Н.О(1) 1.0 × 10 -1.0 × 10° 1.8 x 10° x x+1.0×10-x-1.0 10-18 10-x-18 10-1 -1.8 x 10 5.00 x + 5.00 -5.00 HO(aq) 1.0*10* + CH,COO (aq) RESET -1.0 x 10° x-5.00 x+ 10×10-x-1.0×10-* Determine the quantity of sodium acetate…
For the titration of 10.0 mL 0.10 M glycine (Ka1 = 4.5x10-3; Ka2 = 1.7x10-10) with 0.10 M NaOH, calculate the pH at the following added volumes of NaOH: 1) 0.0 mL 2) 3.0 mL 3) 5.0 mL 4) 10.0 mL 5) 15.0 mL 6) 18.0 mL 7) 20.0 mL 8) 24.0 mL Submit an image of all your answers and their accompanying solutions.
MISSED THIS? Read Section 18.4 (Page); Watch KCV 18.4B. Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. Hd 14 12 10 8 6420 80 120 160 40 Volume of base added (mL) The figure shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 160 milliliters on the x-axis. The curve of the plot goes up gradually from pH 2.3 at 0 milliliters to pH 5.8 at 49 milliliters, next the plot goes up steeply to pH 11.8 at 51 milliliters, and finally the plot goes up gradually to pH 12.2 at 160 milliliters. ✓ Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in way. Part D At what volume of added base does pH =…
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
Y Do you predict that this salt bridge will become stronger, become weaker, or be unaffected as pH increases from pH-7.2 to pH=7.97 The salt bridge will become stronger. The salt bridge will become weaker. The salt bridge will be unaffected. Previous Answers Correct At pH=7.2 the glutamic acid (Glu) side chain will carry a charge of -1 (at 3 pH units above the pK, for Glu, the side chain will be almost fully ionized whereas the histidine (His) side chain will carry a charge of < 0.5 (at pH pK, the charge on His would be +0.5; since pH 7.2 is above its pK, it will carry less (+) charge as it becomes more deprotonated). As the pH increase to 7.9, the charge on Glu will remain-1 and the charge on His will decrease; thus, this salt bridge is predicted to become weaker as pH is raised from 72 to 7.9. Part B Justify your answer with calculations of partial charges on these amino acid side chains at pH 7.2. (Hint: Consider lessons from Coulomb's law, and the Henderson Hasselbalch equation)…
Time to purify biochemisfunase! To do this, you’ll need to make MORE buffers. One of the buffers that you need to make requires 150 mM Tris (pH 8), 250 mM sodium chloride (NaCl) and 2 mM dithiothreitol (DTT, a reducing agent that prevents the formation of disulfide bonds in proteins). Your jolly postdoc friend wants you first to make 500 ml of a1.0M Tris stock solution before making the buffer. Describe how you would make this stock solution, and show all calculations.
In the experiment, when phenolphthalein indicator was added to NH4OH solution, the solution changes color from colorless to pink. True False Eutrophication in lakes depletes the oxygen in water. Moreover, the presence of excess phosphate ions on the lake does not lead to fish kill. true false
Titration is the addition of a chemically equivalent volume of a solution of known concentration called analyte titrant fluent None of them
Calculate the isoionic and isoelectric pH of 0.01111 M methionine. Enter your answers to the hundredths place. isoionic pH = 1 X100 TOOLS x10⁰ isoelectric pH = 2.089 x10-6 Amino Acid Asparagine Glutamine Isoleucine Leucine Methionine Phenylalanine Proline Serine Tryptophan Valine. pKal 2.16 2.19 2.318 2.328 2.18 2.20 1.952 2.187 2.37 2.286 pK₂2 8.73 9.00 9.758 9.744 9.08 9.31 10.640 9.209 9.33 9.719
Choose the buffer with the greatest buffering capacity: d. 0.25M formic acid/formate buffer at pH 3, pKa 3.75 b. 0.25M HEPESH+/HEPES buffer at pH 10, pKa = 8.08 c. 0.75M acetic acid/acetate buffer at pH 4.76, pKa = 4.76 a. 1M acetic acid/acetate buffer at pH 4.76, pKa = 4.76 Next Page