Concept explainers
a. Which compounds are Bronsted-Lowry acids:
b. Which compounds are Bronsted-Lowry bases:
c. Classify each compound as an acid, a base, or both:
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Chapter 2 Solutions
Organic Chemistry (6th Edition)
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- The butylammonium ion, C4H9NH3+, has a Ka of 2.3 1011. C4H9NH3+(aq) + H2O() H3O+(aq) + C4H9NH2(aq) a) Calculate Kb for the conjugate base, C4H9NH2 (butyl amine). b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C4H9NH3+ and a base stronger than C4H9NH3. c) What is the pH of a 0.015M solution of butylammonium chloride?arrow_forwardWhich is the stronger of the following two acids? (a) acetic acid, CH3CO2H, Ka = 1.8 105 (b) chloroacetic acid, ClCH2CO2H, pKa = 2.85arrow_forwardOffer an explanation for the following observations. (a) H3O+ is a stronger acid than NH4+. (b) Nitric acid, HNO3, is a stronger acid than nitrous acid, HNO2. (c) Ethanol and water have approximately the same acidity. (d) Trifluoroacetic acid, CF3COOH, is a stronger acid than trichloroacetic acid, CCl3COOH.arrow_forward
- 1. A. The conjugate base of HCO3− is CO32− HCO3− H2CO3 B. The conjugate acid of HCO3- is CO32− HCO3− H2CO3 C. The conjugate base of H2O is OH− H2O H3O+ D. The conjugate acid of H2O is OH− H2O H3O+ E. What is the conjugated base of each of the following acids in water: HClO4; H2S; HCO3-; H2PO-4F. What is the conjugated acid of each of the following bases in water: SO4-2; H2O; HCO3-; HPO4-2arrow_forward45. HC2H3O2 (aq) + CN¯ (aq) <===> HCN (aq) + C2H3O2¯ (aq) The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information? A) CN¯ (aq) is a stronger base than C2H3O2¯ (aq) B) HCN (aq) is a stronger acid than HC2H3O2 (aq) C) The conjugate base of CN¯(aq) is C2H3O2¯ (aq) D) The equilibrium constant will increase with an increase in temperature. E) The pH of a solution containing equimolar amounts of CN¯(aq) and HC2H3O2 (aq) is 7.0.arrow_forwardCH3OH + H2O = ? Si(OH)4 + H2O = ? HS- + H2O =? What is the conjugate base and acid of the ff?arrow_forward
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