Draw the major chemical species (excluding solvent) that exist at pH=11.85 for a solution containing tyrosine. No credit will be awarded for using shorthand notation or abbreviation to represent the amino acid.
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- Deduce expressions for the fractions of each type of species present in an aqueous solution of lysine as a function of pH and plot the appropriate speciation diagram. Use the following values of the acidity constants: pKa (H3Lys2+) = 2.18. pKa (H2Lys+) = 8.95, pKa(Hlys) = 10.53.1. What are the scientifically proven bioactivity of VCO that is beneficial to human health? 2. Discuss the advantage and disadvantage of Wijs method of iodine value determination. What non-titrimetric method can be used to determine the iodine value of edible oil? Discuss its basic principles and general methods involved.A test tube contains the following chemical equilibrium: N2O4(g) + 59 kJ ⇌ 2NO2(g). You notice that the colourless contents of the test tube turn brown. Provide two realistic reasons as to why this change would occur in a laboratory setting. Support claims with evidence from course concepts
- The pKa values of the conjugate acids of 2-aminopyridine (6.71) and 4- aminopyridine (9.11) are as shown. Which nitrogen is the more basic in these structures and why?Give reasons to support the ansrAssume that for the reaction XTP <> XDP + Pi, the Keq =272024 (dimensionless). Calculate the standard free energy change (delta Go) for the synthesis of XTP from XDP and Pi at 41.4oC in J/mol to six significant figures. Thank you for your assistance
- The pKa values of the conjugate acids of 2-aminopyridine (6.71) and 4- aminopyridine (9.11) are as shown. Why are the acidities of the conjugate acids of these structures different by about two and a half orders of magnitude?Acetic acid (CH3COOH, abbrev HA) is a very common weak acid with pKa = 4.75 (at 25oC and low ionic strength) A] Write down the dissociation equation of the weak acid HA in aqueous solution, derive the respective formulae for the dissociation constant Ka and pKa. B] Calculate pH of the diluted solution of acetic acid with concentration, c = 0.05 mol/dm3 C] What is the approximate pH of the aqueous acetate buffer solution composed of dissolved mixture of acetic acid (HA) and sodium acetate (NaA) in the same respective concentrations? What is the working pH range of acetate buffers? D] How can you prepare exactly 1 dm3 of acetate buffer solution with required pH 5.0 and the total concentration [HA + NaA], c = 0.01 mol/dm3 if the stock solution of acetic acid (HA) with concentration, cHA = 0.1 mol/dm3, anhydrous sodium acetate (NaA, MT = 82.03 g/mol) and purified water are available? E] Acetate buffer solution may be also prepared by the partial neutralization of HA with NaOH: 20 cm3 of…Outline the dissociation reactions for carbonic acid and list the electrical charges of protonated and deprotonated forms. Attach a plot for the portions of molecules possessing each of the outlined charges as function of pH.
- Use data from CRC_Std_Thermodyn_Substances and CRC_Std_Thermodyn_Aqueous-Ions to calculate ΔrH∘ΔrH∘ (in kj/mol) for the following at 25 ∘∘C. 2CaC2O4(s)⟶4CO(g)+O2(g)+2CaO(s)Give clear handwritten answer on the white paper please!If you use 1.00 mole of a monoprotic weak acid (pKa = 5.00) and 0.90 mole of its conjugate base, What is the pH of that solution. Show your work step by step