65mL of a 0.2M solution of the tetrapeptide Arg-His-Ile-Glu is adjusted to pH=7.8. The solution is then titrated with 65mL of a 0.5M solution of HCl. Sketch the titration curve, labelling the pH and volume axes. Indicate clearly the volume of HCl needed to reach each relevant pKa value and equivalence point for the titration given. (Relevant pKa values are 2.2, 4.3, 6.0, 9.6 and 12.5)
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- 3 Sketch a titration curve for the amino acid lysine and indicate the pKa values for all titratable groups. Also indicate the pH at which this amino acid has no net charge.Consider the titration of 50.00 ml of a solution of 0.2574 M of the fully protonated form of the diprotic amino acid glycine (pKa1 = 2.34, pKa2 = 9.60) with 0.3786 M KOH. What is the pH after the addition of 33.99 mL of the KOH solution?You are supplied with the following: NaCl (Mr = 58.443 g/mol) 2.5 M Tris-Cl, pH 8 oplossing / solution (1 Litre) EDTA, sodium salt (Mr = 380.2 g/mol) 10 % Sodium dodecyl sulfate solution Proteinase K solution (50 mg dissolved in 1 ml ddH2O) You need a digestion buffer consisting of the following: 15 mM NaCl 75 mM Tris-Cl, pH 8 16 mM EDTA, pH 8 0.8 % Sodium dodecyl sulfate 0.75 mg/ml proteinase K Calculate: How will you prepare 500 ml of the digestion buffer? Show all your steps and calculations and remember to explain how exactly you will make it up.
- After removing the membranes from an eggshell, the shell is dried and its mass recorded as 5.613 g. The eggshell is transferred to a 250-mL beaker and dissolved in 25 mL of 6M HCl. After filtering, the solution containing the dissolved eggshell is diluted to 250 mL in a volumetric flask. A 10.00-mL aliquot is placed in a 125-mL Erlenmeyer flask and buffered to a pH of 10. Titrating with 0.04988 M EDTA requires 44.11 mL to reach the end point. Determine the amount of calcium in the eggshells as % w/w CaCO3.After removing the membranes from an eggshell, the shell is dried and its mass recorded as 5.613 g. The eggshell is transferred to a 250–mL beaker and dissolved in 25 mL of 6 N hydrochloric acid solution. After filtering, the solution containing the dissolved eggshell is diluted to 250 mL in a volumetric flask. A 10.00–mL aliquot is placed in a 125–mL Erlenmeyer flask and buffered to a pH of 10. Titrating with 0.04988 M EDTA requires 44.11 mL to reach the end point. Determine the amount of calcium in the eggshell as % w/w calcium carbonate.For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. The amount of calcium in the sample is in terms of% CaCO3.
- Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer for maintaining intracellular pH (pH 6.9-7.3)? Justify your answer using your titration curve from part A.After removing the membranes from an eggshell, the shell is dried and its mass recorded as 5.613 g. The eggshell is transferred to a 250-mL beaker and dissolved in 25 mL of 6 M HCl. After filtering, the solution containing the dissolved eggshell is diluted to 250 mL in a volumetric flask. A 10.00-mL aliquot is placed in a 125-mL Erlenmeyer flask and buffered to a pH of 10. Titrating with 0.04988 M EDTA requires 44.11 mL to reach the end point. Determine the amount of calcium in the eggshell as %w/w CaCO3.1) Using the measured pH, calculate the concentration of H3O+ and OH- at the equivalence point. 2) If the theoretical pKa of KHP is 5.4, calculate the percent error using your experimental pKa value.
- A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0418 M EDTA. The endpoint volume was 44.36 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0418 M EDTA and the endpoint volume was found to be 30.02 ml. Calculate the molar concentration of Mg.Calculate the pH at each of the following points for the titration of 100 mL of 0. 6 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide. H3His ↔ H+ + H2His- Ka1 = 3.98x10-3 H2His- ↔ H+ + HHis2- Ka2 = 9.12x10-7 HHis2- ↔ H+ + His3- Ka3 = 4.67x10-10 Vol. of NaOH Calculated pH 0 mL 30 mL 50 mL 75 mL 100 mL 125 mL 135 mL 150 mL 175 mL Please provide a sketch of the titration curve and label both the x & y axis and applicable equations used at each data point (e.g., pH = - log[H+] or pH = pKa or pH = pKa + log )I would need help with these problems, please show step by step: 1. A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4 To this solution was added 50.0 mL of 0.15 M hydrochloric acid (HCl). What was the change in pH of the ammonia, ammonium ion solution? 2. Calculate the isoelectric and isoionic pH of 0.010 M threonine? pK1 = 2.15, pK2 = 9.12 3. Find the pH of a 1.00 L aqueous solution containing 12.43 g of tris (FM 121.14) plus 4.67 g of tris hydrochloride ( FM 157.60) ? What would be the new pH after adding 12.0 mL of 1.00 M NaOH to this buffer?