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- 16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?5. a) The Kw value that we normally use is for room temperature (25°C). Calculate the equilibrium H+ concentration and pH of pure, neutral water at 0.0°C (Kw= 1.14 x 10-15at 0.0°C) b) Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution.(Kb= 4.37 x 10-4at 25°C)NTH assign one of the Trials to pe iment. Upon completion of your exper Volume (mL) 7.0 NICI₂6 H₂O mass of Nicl₂ •64₂0= 2.80 volume of 4.0 M C₂ 48 W₂ = 7.5 1 7.5 mass of witch glass 29.7189 mass of prodiect & watch ghasi 31.9739 mass of the product: 2.269. the pH is a light green & a 7 on the scale. Tria (3) shade. 0 the beaker until you obtai ation of the solid. filtrate in filter blask is pick- Lavener so C₂ 48 No is the excers reasent opwise to the solid unti mL. Record your obses 10 mL graduated cyli 7. Pour tion beaker, dropwise to the bea all of the solution, ges observed dur Ni Cl₂ · 6 Fl₂0 was the lumiting vergent. sti da second 5 mL aliquot RECOVE AL beaker th the ace ted cyli the be 5 mL aliquot of acetone to the
- The equilibrium constant, K, for a neutralization reaction can be symbolized as Kn- Determine K, at 25 °C for the reaction NH, (aq) + HB1O(aq) = NH†(aq) + BrO¯(aq) using Kw, and the K, and K, values from the ionization constant tables. Kn ||Calculate the pH at 25 °C of a 0.13M solution of trimethylammonium chloride ((CH;) NHCI 3 CH;),NHC!) Note that trimethylamine ((CH3),N) i is a weak base with a pK, of 4.19. b. Round your answer to 1 decimal place.Calculate the pH at 25 °C of a 0.60M solution of anilinium chloride (C,H, NH, CI). Note that aniline (C,H, NH,) is a weak base with a pK, of 4.87. Round your answer to 1 decimal place. PH-0
- Disable nd Bases 13 of 21 I Review | Constants | Periodic Table Part A H of nd the As a technician in a large pharmaceutical research firm, you need to produce 150. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.98. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. at ses How much 1.00 M KH,PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. • View Available Hint(s) Volume of KH2PO4 needed = Value UnitsConsider the following data on some weak acids and weak bases: acid base K. Kp name formula name formula 10 4.9 x 10 -4 hydrocyanic acid HCN ethylamine C2H5NH2 | 6.4 × 10 HCH;CO2 1.8 × 10 C,H;NH2 |4.3 × 10 5 - 10 аcetic acid aniline Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C6H5NH3CI choose one v 0.1 М CzHsNHзBr choose one v 0.1 M NaCH3CO2 choose one v 0.1 M Naci choose one vTh C 1. The V C What Cc A My Home Alabama Activity O Dashbo keAssignment/takeCovalentActivity.do?locator=assignment -take 身 口 IReview Topics) (References) M Use the References to access important values if needed for this question. ereg The pH of an aqueous solution at 25°C was found to be 4.30. Creq The pOH of this solution is The hydronium ion concentration is M. req The hydroxide ion concentration is M. req Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next ENG 令 US Home End Ansert F11 F12 F8 F9 F10 & 7 P R T Y U * CO
- Arrange the following solution from lowest pH to highest pH: 0.20 М СН,СООН (К, — 1.8 х 10-5) 0.06 М СH,COОН (К, — 1.8 х 10-5) 0.75 М CH,СООН (К, 3 1.8 х 10-) %3D %3D Section а. 0.20 М СH3СООН < 0.06 M CH-COОH <0.75 М СH,COОН b. 0.75 М СH,CООН < 0.06 М CH;COOH CH;COOH 0.20 М С. 0.06 М СH,СООН < 0.20 М CH-COОH <0.75 М СH,COОН d. p.75 M CН,СООН < 0.20 м CH-COОH <0.06 М СH,COОНH,AsO a triprotic acid with K, = 10-22, K2 = 10-7.0 and Kg = 10-11.5 Now, write the dissociation reactions and the corresponding equilibrium constant expressions. Show a dominant arsenic species graph: pH (use the given K values) vs. a total concentration of arsenic species of 0.01m. What is the mass balance equation of arsenic species, the total concentration is 0.01m.C 1. The V C What Cc A My Home A Activity 1Alabama O Dashbo ginent/takeCovalentActivity.do?locator=assignment-take 身 口 [Review Topics) (References) Use the References to access important values if needed for this question. The pH of an aqueous solution of 9.81x102 M carbonic acid, H„CO3 (aq), is Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next ENG US End Insert Home F9 F10 F7 8. T Y U
