1. Derive the theoretical binding curve for a monoprotic acid (binding fraction as a function of hydrogen ion concentration), starting with the equilibrium expression for a weak acid. 2. Consider two weak acids, with pKa values of 1.8 and 4.5. Calculate the fraction binding of each for the case when pH = pKa, and the fraction binding when pH = 6.0. 3. When we say the pH = pKa at the midpoint of a titration curve, we are assuming slight dissociation of weak acids. What does your answer to question 2 say about the validity of this assumption? 4. In class we discussed how to convert titration data to binding curve data. For a titration with the following calculate the fraction bound. [OH-] = 0.100 Endpoint volume: 15.0 ml Initial volume of acid: 25.0 ml Base added: 7.50 ml pH = 1.6, 4.45 5. For the answers in 4, use the calculated fraction bound and the pH to calculate the Kd values in each case. Submit this on the form on the home page.

1. Derive the theoretical binding curve for a monoprotic acid (binding fraction as a function of hydrogen ion concentration), starting with the equilibrium expression for a weak acid. 2. Consider two weak acids, with pKa values of 1.8 and 4.5. Calculate the fraction binding of each for the case when pH = pKa, and the fraction binding when pH = 6.0. 3. When we say the pH = pKa at the midpoint of a titration curve, we are assuming slight dissociation of weak acids. What does your answer to question 2 say about the validity of this assumption? 4. In class we discussed how to convert titration data to binding curve data. For a titration with the following calculate the fraction bound. [OH-] = 0.100 Endpoint volume: 15.0 ml Initial volume of acid: 25.0 ml Base added: 7.50 ml pH = 1.6, 4.45 5. For the answers in 4, use the calculated fraction bound and the pH to calculate the Kd values in each case. Submit this on the form on the home page.

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

What is the maximum concentration of Mg2+ that can exist in solution at pH 12 considering a solubility product for Mg(OH)2 of Ksp = 10-11.8? How much hardness does this represent, expressed as mg/L CaCO3?
To find the pH of a buffer composed of H₂PO4 (aq) and HPO2(aq), which pKą value should be used in the Henderson-Hasselbalch equation? PK₁3 = 12.32 PK₁2 = 7.21 OpKal = 2.16 Calculate the pH of a buffer solution obtained by dissolving 26.0 g of KH₂PO4(s) and 43.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH || = Incorrect
Consider the dissolution of solid Ca3(PO4)2 in an aqueous solution of 0.2 M Ca(NO3)2. Identify which ONE of the following statements is INCORRECT. a. Ca2+ is the common ion. b. The Ksp expression for calculating the solubility of Ca3(PO4)2 is Ksp = 108s5 c. The value of the Ksp for Ca3(PO4)2 remains unchanged d. After addition of Ca3(PO4)2 the Ca2+ concentration remains constant e. All nitrate anions remain in solution
In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
In this activity you will use the virtual lab to determine the concentration of a strong monoprotic acid. To do this, you can perform a titration using NaOH and phenolphthalein found in the virtual lab. (Note: The concentration of the acid is between 0.025M and 2.5M so you will need to dilute the NaOH solution so that the volume to reach the endpoint is between 10 and 50 mL). Once you have determined the concentration of the acid, please enter your answer into a form at the bottom of this page. Unknown acid: 10 ml 0.15 ml of phenolphthalein 0.60 ml of NaOH
5ml = volume acid/base used to adjust 4.76 HCL concentration = 1.0 M acetate buffer = 0.1 M
The potentiometric titration data of 2,422 mmol chloride ion with 0.1000 M AgNO3 are as follows. What should the x and y axis values be to find the turning point using the first derivative curve? AgNO3 volume (mL) Potential (Volts) 5.0 0.062 15.0 0.085 20.0 0.107 22.0 0.123 23.0 0.138 23.50 0.146 23.80 0.161 24.00 0.174 24.10 0.183 24.20 0.194 24.30 0.233
A solution of 61.01 ml of 0.003453 M A₁B2 is mixed with a solution of 14.82 ml of 0.00200 M C₁D₂. Find the value of pQ (the minus log of Q) for the formation of C₁B2. X 6.41 7.92
Part B: Molar Solubility of Ca(OH): in presence of Ca Temperature of the Experiment:24.6°C Concentration of HCI(ag): 0,05M Trial 1 Trial 2 1) Volume of Saturated Ca(OH)2 solution used 10.05 ml 10.14ml 2) Initial Buret Reading (mL) 11.45 ml 14.85 mL 3) Final Buret Reading (mL) 14.85 mL 18.81 ml 4) Volume of Added HCI (mL) 5) Mole of Added HCI 6) Mole of OH in Ca(OH)2 + Ca" solution 7) Concentration of [OH] (mol/L) 8) Concentration of [Ca) (mol/L) 9) Molar Solubility of Ca(OH): (mol/L) 10) Average Molar Solubility of Ca(OH):
2. Calculate how much agarose you need in order to make a 0.7% agarose gel with 75 mL 1X SB buffer (0.2 M NaOH, 0.75 M Boric Acid, pH 8). How much agarose Unanswered 3. Measure Answer g of agarose in a flask. Add 75 mL 1 x SB buffer,
Will Mg(OH)2() precipitate from a solution that is 0.012 M MgCI2 and also 0.15 M NH3? What is the ion product of the solution? Note: Kp = (NH4*)(OH)/(NH3) = 1.8 ×10-5 Ksp of Mg(OH)2(9)= 1.8 × 10-11 Answer: = yes or no (type "yes" if it will precipitate and "no" if it will not) %3D Qsp x 10 answer 3 is the exponent. include + or - sign
5 A biochemist wants to separate Glu, Arg, and His using a cation-exchange chromatograpy. Determine the order of elution from this column using pH=7.00 buffer mobile phase.