Problem Set #8 – The Nature of Acids and Bases 1. Write the formulas for the conjugate acids of (a) CH 3 NH 2 , methylamine (b) NH 2 NH 2 , hydrazine, (c) HCO 3-and the formulas for the conjugate bases of (d) HCO 3-, (e) C 6 H 5 OH, phenol, (f) CH 3 COOH 2. Write the proton transfer equilibria for the following acids in aqueous solution and identify the conjugate acid-base pairs in each one: (a) H 2 SO 4 , (b) C 6 H 5 NH 3 + , (c) H 2 PO 4-, (d) HCOOH, (e) NH 2 NH 3 + . 3. Identify the Brønsted acid and base and the conjugate base and acid formed in the following reaction: HNO 3 (aq) + HPO 4 2-(aq) ↔ NO 3-(aq) + H 2 PO 4-(aq) 4. Write the two proton transfer equilibria that demonstrate the amphiprotic character of (a) HCO 3-, (b) HPO 4 2-. Identify the conjugate acid-base pairs in each equilibrium. 5. Calculate the molarity of OH-in solutions with the following H 3 O + concentrations: (a) 0.020 mol·L-1 (b) 1.0 x 10-5 mol·L-1 (c) 3.1 x 10-3 mol·L-1 6. Calculate the pH and pOH of each of the following aqueous solutions of a strong acid
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This note was uploaded on 03/01/2011 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas.