CHE 226 ANALYTICAL CHEMISTRY Fall 2004 EXAM III – December 2, 2004 Name ______________________________ WRITE YOUR NAME ON EACH EXAM PAGE NOW. THERE ARE 8 QUESTIONS AND 103 PERCENT TOTAL IN THIS EXAM. Show clearly all work on these pages. Use the proper number of significant figures and the correct units in all final answers. You must show your calculations and/or reasoning, including equations, on a question to obtain any credit; no credit for answers appearing out of the blue. Your work must be understandable at the time it is being graded to obtain any partial credit. You do not have to do the final arithmetic on a question unless you need to have a numerical value for the next part of a question, as long as the answer is expressed in its final form and all algebraic manipulations have been made. Very little will be subtracted for routine arithmetic errors, but all numerical answers must be shown to the proper number of significant figures. Programmable calculators must have all memory erased. A calculator may be used, but not shared with anyone else. Tables of data and other information that may be useful are appended to the back of the exam. Use the backs of the pages as scrap paper. Anything written on the backs will be ignored unless you add an explanatory note on the front of the page. Unless otherwise stated, assume all solutions are aqueous, density = 1.0000 g/mL; activity coefficients are unity (i.e., activity = concentration); temperature, T = 298 K; Kw = 1.008 x 10-14. QUESTION 1 ___________ /6 QUESTION 7 ___________ /14 QUESTION 2 ___________ /8 QUESTION 8 ___________ /34 QUESTION 3 ___________ /6 QUESTION 9 ___________ / QUESTION 4 ___________ /10 QUESTION 10 __________ / QUESTION 5 ___________ /10 QUESTION 11 __________ / QUESTION 6 ___________ /15 TOTAL __________ /103Name __________________________________ Phosphoric acid, H3PO4, is very important in biological systems, even though it is a relatively simple inorganic acid. Often referred to as “inorganic phosphate” or “monophosphate”, Pi, it is involved in a myriad of enzymatic and other biological reactions. Phosphate is a vital constituent of nucleotides and nucleic acids and a major component of calcium hydroxyapatite, Ca10(PO4)6(OH)2, which forms teeth and bones. Although the carbonate buffer primarily controls physiological pH in most mammals, phosphate also contributes to the buffering action. The pKa’s for phosphoric acid, H3PO4, are 2.15, 7.20, and 12.15. Questions #1-6 following immediately below deal directly with phosphoric acid and its acid-base properties. 1. (6 Points) Calculate the values of the Ka’s for phosphoric acid. 2. (8 Points) The pH of blood is normally about 7.40 in healthy humans. Identify the two predominant chemical forms of phosphoric acid (or, “the phosphate system”) at this pH, and calculate the concentration ratio of the basic to the acidic form. CHE 226 Exam III Fall 2004 2Name __________________________________ 3. (6 Points) Calculate the theoretical pH of a 0.0500 M solution of Na2HPO4. Assume that all the simplifying assumptions that are typically used to reduce an acid-base system to one controlling equilibrium when calculating pHs are valid. 4. (10 Points) Now, calculate the theoretical pH of 0.0500 M Na2HPO4 using the full equation derived when none of the simplifying assumptions is made. [See the last page.] 5. (10 Points) Using the hydrogen ion concentrations obtained from Questions 3 and 4 above, calculate the relative error in the hydrogen ion concentration obtained in Question 3. [This assumes that the more extensive equation provides the “true value”, or at least a better estimate of it.] Does the simple approach provide an acceptable level of error? CHE 226 Exam III Fall 2004 3Name __________________________________ 6. (15 Points) Calculate the theoretical pH of a solution formed by mixing 50.0 mL of 0.200 M NaH2PO4 with 50.0 mL of 0.120 M HCl? 7. (14 Points) Calculate the pH of a solution that is 0.100 M in 2-(2-aminoethyl)pyridine -- H2NCH2CH2-C5H5N, AEP. This is a dibasic compound – the amino group and the ring nitrogen. A handbook table of pKa values for the protonated forms indicates that the pKa1 = 4.24 for the diprotonated (+2) form, H2AEP2+, and pKa2 = 9.78 for the monoprotonated (+1) form, H2AEP2+. CHE 226 Exam III Fall 2004 4Name __________________________________ 8. (34 Points) Barium iodate, Ba(IO3)2, is relatively insoluble [Ksp = 1.57 x 10-9]. Iodic acid is a fairly strong “weak acid” [Ka = 1.7 x 10-1]. You wish to calculate the theoretical solubility S of barium iodate in a solution that is also 0.10 M in iodic acid. Because of its acid strength you must use the full systematic approach to solving this problem. (a) (12 Points) Accurately write all the equilibrium reactions for this system. Next to each equation write its associated equilibrium constant. (b) (5 Points) List all the chemical species that exist in this solution whose concentrations are not known and must therefore be calculated. (c) (10 Points) Write the mass-balance equations for this system. Let S stand for the equilibrium solubility of barium iodate. (d) (7 Points) Write the charge-balance equation for this solution. CHE 226 Exam III Fall 2004 5Name __________________________________ SELECTED CONSTANTS, UNITS, AND CONVERSION FACTORS [The uncertainty in the last digit(s) is shown italicized in parentheses] Atomic mass constant: mu = 1.660 538 73 x 10-27 kg Avogadro’s number: N = 6.022 141 99 (47) x 1023 mol-1 Boltzmann constant: k = 1.380 6503 (24) x 10-23 J/K Elementary charge: e = 1.602 176 462 (63) x 10-19 C Faraday constant: F = 96 485.3415 (39) C/mol Molar gas constant: R = 8.314 472 (15) J/K-mol = 1.9872 cal/K-mol = 0.082 057 L-atm/K-mol = 0.022 414 m3/mol at STP Pi: π = 3.141 592 653 6 Planck’s constant: h = 6.626 068 76 (52) x 10-34 J-s Speed of light (in a vacuum): c = 2.999 792 458 (exact) x 108 m/s Stefan-Boltzmann constant: σ = 5.670 400 (40) x 10-8 W/m2-K4 Standard acceleration of gravity: gn = 9.806