(a) The pH at which average net glycine is +0.5. (b) The pH that is equal to the pKa of the protonated amino group. (c) The pH at which the predominant glycine species is "NH3-CH2-COOH
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Q: For the following hexapeptide shown below, answer the following questions. E-N-D-Y-K-L Draw the…
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Q: Which amino acid has the greatest amount of negative charge at pH = 6.20?
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- 3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 1243. 40.00 mL of 0.0900 M NaOH is diluted to 100mL and titrated with 0.1000M HCI. Calculate the pH after the addition of the following volumes of titrant (mL); (a) 0.00; (b) 10.00 ; (c) 18.00: (d) 30.00 ; (e) 35.95 ; (f) 36.00 (g) 36.05 ; (h) 40.00.UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
- I made some titrations and the calculated molarity of HCI was 0.096, 0.097 and 0.098. The nomical concentrsrion of HCl is 0.1. How can I explain my results by comparing it to the nominal concentration if my confidence intervals don't include the nominal concentration?A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2 to reach an end point with bromocresol green indicator. The molar concentration of the HCl is calculated using the equation below (attached image): a.) Calculate the uncertainty of the result (absolute error). M=0.02333(±?????) M b.) Calculate the coefficient of variation for the result. CV= (Sy/y) x 100%Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K, = 5.2 x 10), with 0.1000 M HCl solution after the following additions of titrant. %3D (a) 10.00 mL: pH =9.72 (b) 20.70 mL: pH =|8.25 (c) 28.00 mL: pH =|10.17 %3D
- Q2) Q2) How much mole of NH3 to be added to 500 ml of the solution with pH=8.9 to dissolve 5x10 * of AgSCN? PKSP(AGSCN)=12, PKa(NH.') =9.2 , PKDA9(NH3)*/Ag+=7.2The titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? Given that the chemical reaction is 2MnO4- + 5C2O42- + 16H+ -----> 2Mn2+ + 10CO2 + 8H2O Provide a detailed solution.Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (к. = 1.54 x 105), with 0.1000 M NaOH solution after the following additions of titrant. (а) 10.00 mL: pH = (b) 20.10 mL: pH = (c) 29.00 mL: I. pH =
- Formulate a hypothesis regarding the solubility of aspirin at different pH.The experimentA) Three teaspoons of water (approx. 15 ml) were added to one tablet said to contain 300 mg of aspirin. Fizzingwas observed. Most of the tablet dissolved, but there were some solid particles. By heating the mug in amicrowave for 10 second increments until the water came to the boil (approx. 3x), all of the solid particlesdissolved. The solution was left to cool to room temperature and then placed in a fridge and NOTHINGHAPPENED. Try this yourself if you can spare two aspirin tablets, your results might look different.• Questions to ask:1. What might the fizzing bubbles be?2. Can you give a chemical explanation?3. Can you write a chemical reaction equation with aspirin reacting with something to give a gas and aspirinin another form?4. What might be the formulation (what the manufacturer mixes with aspirin in making the tablet) “trick”for aspirin to improve solubility?5. How does this compare with…b) Prepare 1000 of pH 5.50 acetate buffer solution from 0.1000 M CH;COOH and 0.1000 M NaCH;CO0 (solve for the volume of CH;COOH and NaCH;COO required)A professor prepares a buffer solution that they need for the purification of protein from human cell lysates. They did mix weak acid and conjugate base and obtained the initial solution, which is characterised by these parameters. Final volume: 200mltotal buffer compound concentration: 150mMIntitial concentration weak acid: 0.03MInitial concentration conjugate base: 0.12MInitial pH 6.9buffer compound pka 6.3