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The velocity v with which a protein moves through water under the influence of an electric field varied with values of pH in the range 3.0<pH<7.0 according to the expression v/( ųms-1)=a+b(pH)+c(pH)^2+ d(pH)^3 with a=0.50, b=-0.10, c=-3.0*10^-3, and d=5.0*10^-4. Identify the isoelectric point of the protein.
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- 5A.3(a) Suppose that na = 0.10ng and a small change in composition results in HA changing by dµ =+12Jmol-!, by how much will µz change?b) Conductivity measurements were one of the first methods used to determine the ionization constant of water (Kw). The ionization constant of water is given by the following equation: Kw = (aµ+)(aoH-) = M ) Given that: т a = Y+ X m° = 1 mol kg. Quantities a, V+ and m denote activity, mean activity coefficient and concentration. log y+ = -|Z+Z_|A/Im, A = 0.509 for aqueous solution at 25 °C. Assume that Y+ × 1 and water is a weak electrolyte with degree of dissociation of a. Using the expression provided, show that the molar conductivity of pure water (A) can be -1/2 written as A(H20) = (1 M)K²[^.(H*)+ A,(OH¯)]. Quantity 1, denotes molar ionic conductivity at infinite dilution. [A(H20) = 5.5 × 10-6 S m¬1 and Kw = 10-14] %3D Kohlrausch and Heydweiller measured the conductivity of water in 1894 and determined that A(H20) = 5.5 × 10-6 S m-1 at 298 K. Using the information provided in Table 1, determine Kw. Table 1 Cation A. (01 cm? mol) Anion Ao ( cm? mol-1) H3O* or H* 350.0 OH 199.2 NH4+…At 298 K, the electrolytic conductivity of a 0.2 M KC1 solution is 2.50 X 10-2S cm-1. Calculate its molar conductivity.
- What is the strength of the ionic interactions between an ion with 1 positive charges and an ion with 2 negative charges, when the distance between them is 19.4 nanometers and the solvent is water, at 25 oC with a dielectric constant of 78.5?Differentiate acidimetry from alkalimetryAt 25 °C the molar ionic conductivities of F−, Cl−, and Br− are 5.54 mS m2 mol−1, 7.635 mS m2 mol−1, and 7.81 mS m2 mol−1, respectively. What are their mobilities?
- 4.(a) Aqueous 50.5 % (w/w) sodium hydroxide has a density of 1.53 g cm–3. Calculate the concentration of this solution in mol dm–3. (b) What volume of 50.5 % (w/w) aqueous sodium hydroxide is required to prepare 500 cm3 of 0.100 mol dm–3 stock NaOH? [Start with your answer to 4(a)](b) The critical packing parameter for a surfactant is defined as: CPP = agle where v is the hydrocarbon volume, a, is the head group area, and l, is the chain length. (1) Using the critical packing parameter, give conditions for the formation of spherical micelles, cylindrical micelles, and bilayers in solution. (ii) A particular surfactant has a hydrophobic volume of 459.4 A', head group area of 71 A, and tail length of 21.8 A. What structure is this likely to form in solution? If a surfactant has hydrophobic volume of 520 A' and tail length of 24 A between which values of head group area would it form cylindrical micelles? (ii) 18 tv MacBook Air 000 Edality al, g. on te ew led ed in X= A solution was prepared by dissolving 140.0 g of KCl in 315 g of water. Calculate the mole fraction of KC1. (The formula weight of KCl is 74.6 g/mol. The formula weight of water is 18.0 g/mol.) Express the mole fraction of KCl to two decimal places. View Available Hint(s) Submit 5 ΑΣΦ Part B - Use the definition of molality 001 mol/ka 12 of 33 ? P Pearson Review I Constants I Periodic Table A solution was prepared by dissolving 140.0 g of KCl in 315 g of water. Calculate the molality of KC1. (The formula weight of KCl is 74.6 g/mol. The formula weight of water is 18.0 g/mol.) Express the concentration of KCl in molality to two decimal places. ▸ View Available Hint(s) >
- Calculate the Debye length (1/k) of the double electric layer near the charged surface in KCl solutions of two concentrations c1 =0.01 M and c2= 0.1 M.Calculate the ionization constant of propanoic acid (CH3CH2COOH) using the following data: Parameter Value pH 4.51 1.18 x 105 µS-cm1·M-1 3.866 x 105 uS-cm-1·M-1 Molar conductivity of HZ, Am Conductivity at infinite dilution, Ao To calculate the ionization constant, calculate the following: (report all answers in 3 SF) 1. fraction of propanoic acid ionized: 2. equilibrium concentrations of the conjugate base of propanoic acid and hydronium ion: M 3. initial concentration of the acid: M 4. ionization constant:Calculate the ionic strength (in mmoldm^-3) of 0.05moldm^-3 K3PO4