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Unit Seven Worksheet – 2 WS – C – U7C20S3-4 Name_________________________________________________ Period__________________ Section 20.3 Part I: Matching. Match the definition with the term that best correlates to it. No definition will be used more than once. _____1. Amphoteric _____7. Hydrogen-ion donor _____2. Conjugate acid _____8. Lewis acid _____3. Conjugate base _____9. Lewis base _____4. Conjugate acid-base pair _____10. Monoprotic acid _____5. Diprotic acid _____11. Triprotic acid _____6. Hydrogen-ion acceptor A) B) C) D) E) F) G) H) I) J) K) A Bronsted-Lowry acid A Bronsted-Lowry base Description of a substance that can act both as an acid and a base Acid that contains three ionizable hydrogens Acid that contains two ionizaable hydrogens Acid that contains one ionizaable hydrogen Particle that remains when an acid has donated a hydrogen ion An electron-pair acceptor An electron-pair donor Particle formed when a base gains a hydrogen ion Two substances that are related by the loss or gain of a single hydrogen ion Part III: Short Answer. Answer the following questions. Classify each of the following acids as monoprotic, diprotic, or triprotic. 12. HCOOH: _____________________________________________________________ 13. HBr: ________________________________________________________________ 14. H2SO3: ______________________________________________________________ 15. H3ClO4: _____________________________________________________________ 16. What would you expect to happen when lithium metal is added to water? Show the chemical reaction. page 1 – WS – C – U7C20S3-4 17. Identify the hydrogen ion donor(s) and hydrogen ion acceptor(s) for ionization of sulfuric acid in water. Label the conjugate acid-base pairs. 18. Identify all of the ions that may be formed when H3PO4 ionizes in water. 19. In the following chemical reaction, identify the Lewis acid and base. BF3 + F– ↔ BF4– Section 20.4 Part I: Matching I. Match the definition with the term that best correlates to it. No definition will be used more than once. _____20. Acid dissociation constant _____23. Strong base _____21. Base dissociation constant _____24. Weak acid _____22. Strong acid _____25. Weak base A) B) C) D) E) F) Ratio of the concentration of the dissociated (or ionized) form of an acid to the concentration of the undissociated acid; symbolized Ka Base that dissociates completely into metal ions and hydroxide ions in aqueous solution Acid that completely ionizes in aqueous solution Base that does not dissociate completely in aqueous solution Acid that only partially ionizes in aqueous solution Ratio of concentration of conjugate acid times concentration of hydroxide ion to the concentration of conjugate base; symbolized Kb page 2 – WS – C – U7C20S3-4 Part II: Matching I. Match each solution with its correct description. _____26. dilute, weak acid A) B) C) D) E) _____27. dilute, strong base _____28. concentrated, strong acid 18M H2SO4(aq) 0.5M NaOH(aq) 15M NH3(aq) 0.1M HC2H3O2(aq) 0.1M HCl(aq) _____29. dilute, strong acid _____30. concentrated, weak base Part III: Short Answer. Answer the following questions. 31. Write the expression for the base dissociation constant for hydrazine, N2H4, a weak base. Hydrazine react with water to form the N2H5+ ion. 32. Write the base dissociation constant expression for the weak base analine, C6H5NH2. C6H5NH2(aq) + H2O(l) ↔ C6H5NH3+(aq) + OH–(aq) Part IV: Calculations. 33. Solve the following problems. Show work or receive no credit. Include proper units. A 0.10M solution of formic acid has an equilibrium [H+] = 4.2 x 10-3 M. HCOOH(aq) → H+(aq) + HCOO–(aq) What is the Ka of formic acid (HCOOH)? page 3 – WS – C – U7C20S3-4 34. The Ka of benzoic acid, C6H5COOH, is 6.3 x 10-5. What is the equilibrium [H+] in a 0.20 M solution of benzoic acid? 35. A 0.10M solution of hydrocyanic acid, HCN, has an equilibrium hydrogen ion concentration of 6.3 x 10-6M. What is the Ka of hydrocyanic acid? page 4 – WS – C – U7C20S3-4