Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula HNO2 4.5 x 10 NH3 1.8 x 10 -5 nitrous acid ammonia acetic acid HCH;CO2|1.8 × 10 -5 -4 ethylamine C2H, NH, 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'i' 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 KCH3CO2 choose one O 0.1 M NaNO2 choose one O 0.1 M NH4Br choose one O 0.1 M Naci choose one O

Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula HNO2 4.5 x 10 NH3 1.8 x 10 -5 nitrous acid ammonia acetic acid HCH;CO2|1.8 × 10 -5 -4 ethylamine C2H, NH, 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'i' 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 KCH3CO2 choose one O 0.1 M NaNO2 choose one O 0.1 M NH4Br choose one O 0.1 M Naci choose one O

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 191MP

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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?
Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 M
Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
The acid ionization constants for species that are listed below can be found by using data given in the following tables: Acid Ka1 Ka2 Ka3 H3PO4 7.5 x 10–3 6.2 x 10–8 4.2 x 10–13 H2CO3 4.3 x 10–7 5.6 x 10–11 HNO2 4.5 x 10–4 HIO3 1.7 x 10–1 Base Kb NH3 1.8 x 10–5 Which of the following is the weakest acid? HCO3– HNO2 NH4+ HIO3 H2PO4–
Hello, i am provided the pH levels and volumes for Bromocresol Green weak acid by strong base and strong base by weak acid. I am also provided the pH levels and volumes for Phenolphthalein weak acid by strong base and strong base by weak acid. How can we set up a table with all these information to make a graph for each. Heres the data Bromocresol Green: - weak acid by strong base: 12.80 pH; 20.3 mL - strong base by weak acid: 1.49 pH; 20.1 mL Phenolphthalein: - weak acid by strong base: 12.83 pH; 20.1 mL - strong base by weak acid:1.49 pH; 20.1 mL
Consider the molecule, pentanoic acid which has a pKa of 4.81: H3C OH Calculate the conjugate base to acid ratio at each of the following pH values. i. 11.75 ii. 4.81 iii. 2.95
Consider the following list when answering the questions that follow: C6H5CO2H , Ka = 6.3 x 10-5 C6H5CO2 - , Kb = 1.6 x 10-10 CN- , Kb = 2.5 x 10-5 HCN , Ka = 4.0 x 10-10 For the reaction between benzoic acid (C6H5CO2H ) and a solution containing cyanide ions (CN- ): (a) The name of the conjugate base produced is --- (b) The name of the conjugate acid produced is --- (c) The reaction is ----- favoured (type 'reactant' or 'product'), because the reactants are the ----- (type 'weaker' or 'stronger') set of acid and base.