Derive the ionization fraction, a2, where (HPO?-), in terms of and the acidity constants, Ka1, Kaz, and Kaz for the phosphoric acid system. Plot the pa-pH diagram for this system. Note: Pr = [H3PO,) + [H2PO,]+ [HPO;-]+ [PO?-] %3D
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- Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.Given that the equivalence point volume from the second derivative plot is 7.3429, how many grams of salicylic acid (138.121 g/mol) was synthesized? To determine the yield of the hydrolysis reaction, potentiometric titration was done. NaOH was used as the titrant, and three trials of standardization with KHP yields a titrant concentration of 0.0427 M.Calculate the mole fractions of SO2•H2O, HSO3- and SO3 2- in solution at a pH of 3.0, characteristic of many fogs, as well as the total concentration of S(IV) in solution for 20 ppb SO2 in the gas phase. Constants attached in table
- Determine the pH and concentration of all species at equilibrium for the basic 5-fluorouracil species (C4HFN2O22-). Justify the use of approximations if necessary.Provide the equation for the mass balance of this solution. C4HFN2O22-= 0.30 MGive the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.
- ) A truck driver carrying a load of lead nitrate (Pb(NO3)2) lost control of his semi- truck after hitting a patch of ice and crashed the truck into Blue Lake, which was right next to the highway. Despite the best efforts of the emergency workers, several of the crates containing lead nitrate were damaged, and the highly soluble compound dissolved immediately. Assuming the lake is initially at circumneutral pH (7), and that the spill resulted the in a total lead concentration of 10-3 M within the lake. Based on the following information, will PbO(s) precipitate out of Blue Lake. Assume all lead nitrate dissociates into Pb+2 and NO3-, no other sources of lead exist in the lake and that no other reactions besides the equations shown below occur. PbO(s) + 2H+ ⇌ PbO(s) + H+ ⇌ PbO(s) + H2O ⇌ PbO(s) + 2H2O ⇌ Pb2+ + H2O PbOH+ + H2O Pb(OH)2o Pb(OH)3- + H+ logKs0/ksp =14 logK1=3.4 logK2=-0.5 logK3=-12The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.044 M solution of HClO isThe Henderson-Hasselbalch equation: a. relates the pH of a solution to the pKa and the concentration of acid and salt. b. allows the graphical determination of the molecular weight of a weak acid from its pH alone. c. is equally useful with solutions of acetic acid and of hydrochloric acid. d. employs the same value for pKa for all weak acids.
- A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationIf an Ecell of 0.495V was noted when your cell was set-up. What is thesolution pH?What is the pH of a solution which is equimolar with respect to both ethanoic acid and sodium ethanoate? (Ka for ethanoic acid is 1.8 x 10-5 moldm-3) What special property does this solution have?