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Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following:
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- The conjugate base of hydrofluoric acid dissolved in water is: a F b OH c H3O d HF e F2arrow_forwardUse Table 14.3 to help answer the following questions. a. Which is the stronger base, ClO4 or C6H5NH2? b. Which is the stronger base, H2O or C6H5NH2? c. Which is the stronger base, OH or C6H5NH2? d. Which is the stronger base, C6H5NH2 or CH3NH2?arrow_forwardUse this list of important industrial compounds (and Figure 14.8) to answer the following questions regarding: CaO, Ca(OH)2, CH3CO2H, CO2, HCl, H2CO3, HF, HNO2, HNO3, H3PO4, H2SO4, NH3, NaOH, Na2CO3. (a) Identify the strong Bronsted-Lowry acids and strong Bronsted-Lowry bases. (b) List those compounds in (a) that can behave as Bronsted-Lowry acids with strengths lying between those of H3O+ and H2O. (c) List those compounds in (a) that can behave as Bronsted-Lowry bases with strengths lying between those of H2O and OH-.arrow_forward
- 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.arrow_forwardShow how methylamine, CH3NH2, is a BrnstedLowry base. Is methylamine also a Lewis base? Explain.arrow_forwardAccording to the Brønsted-Lowry theory, which of the following would you expect to act as an acid? Which as a base? (a) CH3O- (b) CO32- (c) HAsO42-arrow_forward
- Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid in each of the following equations: (a) NO2+H2OHNO2+OH (b) HBR+H2OH3O++Br (c) HS-+H2OH2S+OH (d) H2PO4+OHHPO42+H2O (e) H2PO4+HClH3PO4+Cl (f) [Fe( H 2 O)5(OH)]2++[Al( H 2 O)6]3+[Fe( H 2 O)6]3++[Al( H 2 O)5(OH)]2+ (g) CH3OH+HCH3O+H2arrow_forwardTrimethylamine, (CH3)3N, is a common reagent. It interacts readily with diborane gas, B2H6. The latter dissociates to BH3, and this forms a complex with the amine; (CH3)3N BH3. Is the BH3 fragment a Lewis acid or a Lewis base?arrow_forwardA hydrogen atom in the organic base pyridine, C5H5N, can be substituted by various atoms or groups to give XC5H4N, where X is an atom such as Cl or a group such as CH3. The following table gives Ka values for the conjugate acids of a variety of substituted pyridines. (a) Suppose each conjugate acid is dissolved in sufficient water to give a 0.050 M solution. Which solution would have the highest pH? The lowest pH? (b) Which of the substituted pyridines is the strongest Brnsted base? Which is the weakest Brnsted base?arrow_forward
- 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)arrow_forwardFor solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Kaarrow_forward
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