Identify the sets that contain acid-base conjugate pairs.1. HNO2, NO,"2. Н.СО, СО, 2-3. HCI, ClO,-4. HS-, H,S5. NH3, NH,"Cr14:34/20:32

If a species loses a proton then it is considered as Bronsted-Lowry acid. If a species receives one…

Answered: Identify the sets that contain…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 34CTQ

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Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
The dihydrogen phosphate ion has the ability to act as an acid in the presence of a base and as a base in the presence of an acid. What is this property called? Illustrate this behavior with water by writing BrnstedLowry acidbase reactions. Also illustrate this property by selecting a common acid and base to react with the dihydrogen phosphate ion.
2. The molecule whose structure is illustrated here is amphetamine, a stimulant Which description best fits this molecule? (Note: There may be more than one answer.) Brønsted acid Lewis acid Brønsted base Lewis base
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. CaO b. SO2 c. Cl2O
Use Table 14.3 to help order the following acids from strongest to weakest HNO3,H2O,NH4+,C5H5NH+
Calculate the ionization constant for each of the following acids or bases form the ionization constant of its conjugate base or conjugate acid: (a) F- (b) NH4+ (c) AsO43- (d) (CH3)2 NH2+ (e) NO2- (f) HC2O4- (as a base)
Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.
. Consider 0.25 M solutions of the following salts: NaCl. RbOC1, KI, Ba(ClO4),, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.
Calculate H+ and OH- and in solutions with the following pH. (a) 9.0(b) 3.20 (c) -1.05 (d) 7.46
Acids and bases can be thought of as chemical opposites (acids are proton donors, and bases are proton acceptors). Therefore, one might think that Ka = 1/Kb. Why isnt this the case? What is the relationship between Ka and Kb? Prove it with a derivation.

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Identify the sets that contain acid-base conjugate pairs. 1. HNO2, NO," 2. Н.СО, СО, 2- 3. HCI, ClO,- 4. HS-, H,S 5. NH3, NH," Cr 14:34/20:32