HOMEWORK 1A 1. Write the correct equilibriumconstant expressions for the following reactions. (a) 4NH 3 (g) + 7O 2 (g) 4NO 2 (g) + 6H 2 O (g) (b) 2NO 2 (g) + 7H 2 (g) 2NH 3 (g) + 4H 2 O (g) (c) NH 4 Cl (s) NH 3 (g) + HCl (g) (d) 2ZnS (s) + 3O 2 (g) 2ZnO (s) + 2SO 2 (g) (e) Cl 2 (g) + H 2 O (g) 2HCl (g) + ½O 2 (g) 2. In a 2.50 L flask at 298 K, 0.125 mol SO 2, 0.145 mol O 2, and 0.465 mol SO 3 are at equilibrium. Calculate the equilibrium constant for the reaction: 2SO 2 (g) + O 2 (g) 2SO 3 (g) 3. At 450 K the equilibrium constant for the reaction: NO (g) + ½O 2 (g) NO 2 (g) is given by: K eq = 1.25 x 10 2 (a) At equilibrium are the products or reactants favored for this reaction? (b) What is the numerical value of K eq for the reaction: 2NO (g) + O 2 (g) 2NO 2 (g) (c) What is the numerical value of K eq for the reaction: 2NO 2 (g) 2NO (g) + O 2 (g) 4. The equilibrium constant for the reaction: N 2 (g) + O 2 (g) 2NO (g) at 2,130ºC is 2.0 x 10 1. For the following conditions, determine whether the reaction is spontaneous forward or in reverse, or whether it is at equilibrium. (a) A 1.0 L box contains 0.02 mole of N 2, 0.01 mole of O 2, and 0.02 mole of NO at 2,130ºC. (b) A 1.0 L box contains 0.2 mole of N 2, 0.01 mole of O 2, and 0.02 mole of NO at 2,130ºC. (c) A 1.0 L box contains 0.2 mole of N 2, 0.01 mole of O 2, and 0.2 mole of NO at 2,130ºC.
HOMEWORK 1B 1. At 1,476 K the equilibrium constant for the reaction: CO (g) + ½O 2 (g) CO 2 (g) is given by: K c = 2.50 x 10 5 (a) Determine the numerical value of K p for the above reaction. (b) What would be the numerical value of the K p for the reaction: 2CO (g) + O 2 (g) 2CO 2 (g) 2. When sulfur trioxide is produced from the combustion of sulfur dioxide at 1,000. K, a sample of the equilibrium gas mixture showed 0.562 atm of SO 2, 0.101 atm of O 2, and 0.332 atm of SO 3. (a) Calculate the equilibrium constant, K p, for the reaction: 2SO 3 (g) 2SO 2 (g) + O 2 (g) (b) Determine the numerical value of K c for the above reaction. (c) Calculate the numerical value of the K c for the reaction: SO 2 (g) + ½O 2 (g) SO 3 (g) 3. At 298 K, K c = 2.25 x 10 2 for the reaction: 2NO (g) N 2 (g) + O 2 (g) (a) If a container is initially charged with 7.50 M NO, calculate the equilibrium concentration of NO. (b) What is the percent dissociation of NO? 4. A solution is prepared by dissolving 0.125 moles of calcium chloride in enough water to make 500.0 ml of solution. (a) Calculate the molarity of the calcium chloride in the solution. (b) A 100.0 ml sample of the calcium chloride solution is mixed with 10.0 ml of water. Calculate the molarity of the calcium chloride in the new solution. (c) Calculate the molarities of the calcium ions and the chloride ions in the new solution.
HOMEWORK 1C 1. K p is 0.225 at 350ºC for the reaction: 2NO (g) N 2 (g) + O 2 (g) The tank is initially charged with 0.200 atm NO, 0.100 atm N 2, and 0.100 atm O 2 at 350ºC. (a) Is the forward or reverse reaction spontaneous? (b) Calculate the pressure of NO once equilibrium has been established. 2. For the reaction: 2ClF (g) Cl 2 (g) + F 2 (g) A 2.50 L flask at equilibrium contains 0.400 moles of ClF, 0.300 moles of Cl 2, and 0.100 moles of F 2. (a) Calculate the numerical value of the K c for the above reaction. (b) If 0.200 moles of F 2 is added to the flask at equilibrium, calculate the new concentration of ClF when equilibrium is reestablished. 3. Complete each of the following ICE tables, and tell if the x in the ICE table will be large or small. (a) A + 2B C K eq = 1 x 10 9 I 1.0 1.0 0 C E (b) A + 2B C K eq = 1 x 10 9 I 0 0 1.0 C E (c) 2D + E 2F K eq = 1 x 10 9 I 1.0 1.0 0 C E (d) 2D + E 2F K eq = 1 x 10 9 I 0 0 1.0 C E 4. The equilibrium constant for the reaction: 2HCl (g) H 2 (g) + Cl 2 (g) at 25ºC is 6.2 x 10 54. (a) Why was it unnecessary to be told whether the value is for K p or K c? (b) Without any calculations, what does the numerical value of this constant tell you about the decomopition of HCl? (c) If 0.010 mole of HCl is placed in a 1.0 liter tank and allowed to come to equilibrium at 25ºC, will the x in the ICE table be large or small? What will be the final concentration of the hydrogen gas, in moles per liter? (d) If 0.0050 mole of Cl 2 and 0.0050 mole of H 2 are placed together in a 1.0 liter tank and allowed to come to equilibrium at 25ºC, will the x in the ICE table be large or small? What will be the final concentration of the hydrogen gas, in moles per liter?
HOMEWORK 1D 1. 3.00 moles of NO, 5.00 moles of ClNO, and 2.00 moles of Cl 2 are placed in a 25.0 liter tank at a temperature of 503 K. After the reaction has come to equilibrium, there are 6.12 moles of ClNO in the tank. (a) Write a balanced equation for the reaction producing 1 mole of ClNO from the other two substances. (b) Calculate K c for this reaction at 503 K, with proper units. (c) Calculate K p for this reaction at 503 K, with proper units. 2. Ammonia decomposes according to the reaction: 2NH 3 (g) N 2 (g) + 3H 2 (g) A 2.00 liter tank is originally charged with 0.500 moles of ammonia, and at equilibrium it is found that the ammonia is 16.5% decomposed. Calculate the numerical value of the K c for the above reaction. 3. A tank of O 2 has an initial pressure of 2.00 atm. The O 2 undergoes the reaction: 3O 2 (g) 2O 3 (g) and at equilibrium the total pressure is 1.75 atm. Find K p for the reaction 4. At 350 K, a 14.0 g sample of N 2 O gas is placed in an evacuated 10.0 liter container. (a) What is the pressure of N 2 O in the container, measured in atmospheres? (b) The N 2 O gas decomposes, as shown by the following equation: 2N 2 O (g) 2N 2 (g) + O 2 (g) If the N 2 O from (a) is 20.0% decomposed when equilibrium is established at 350 K, calculate the value of the K p for this decomposition reaction. (c) If the temperature is raised to 400 K, the N 2 O from (a) is 25.0% decomposed when equilibrium is reestablished. Calculate the value of the K c for this decomposition reaction at 400 K. (d) If the temperature is raised to 450 K, the K c for this decomposition reaction is 2.7 x 10 2 M. How many moles of O 2 must be added to the container to reduce the quantity of N 2 O to 0.200 moles at equilibrium. 5. The following reaction is exothermic: PCl 3 (g) + Cl 2 (g) PCl 5 (g) For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2) whether the new equilibrium pressure of PCl 5 will be higher, lower, or remain the same. (a) The addition of a catalyst (b) A decrease in the volume of the reaction container (c) Addition of chlorine gas at constant volume (d) An increase in temperature (e) Adding argon gas to the reaction container (f) Addition of PCl 5 gas at constant volume. (continued on next page)
6. The following reaction is endothermic: CaCO 3 (s) CaO (s) + CO 2 (g) For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2) whether the new equilibrium pressure of CO 2 will be higher, lower, or remain the same. (a) A decrease in the volume of the reaction container (b) Addition of carbon dioxide gas at constant volume (c) An increase in temperature (d) Addition of solid CaCO 3 at constant volume. 7. For the same reaction in problem 6, indicate whether the new equilibrium mass of CaCO 3 will be higher, lower, or remain the same. (a) An decrease in the volume of the reaction container (b) Addition of carbon dioxide gas at constant volume 8. The following reaction is exothermic: N 2 (g) + 3H 2 (g) 2NH 3 (g) For each of the following properties, indicate how it must change to force the equilibrium to shift to the right. (a) Pressure (b) Temperature (c) Concentration of N 2 (d) Concentration of NH 3
HOMEWORK 1E 1. Rank the following acids from weakest to strongest: H 4 SiO 4, H 3 PO 4, H 2 SO 4, HClO 4. 2. For the following reaction: C 3 H 7 NH 2 + CH 3 OH C 3 H 7 NH 3 + + CH 3 O (a) Identify the acid, base, conjugate acid and conjugarte base (b) If the reverse reaction is favored, identify the strongest ascid and strongedt base in the reaction 3. Identify the conjugate base for each of the following: (a) HF (b) H 2 O (c) NH 3 (d) HSO 4 4. Identify the conjugate acid for each of the following: (a) F (b) H 2 O (c) NH 3 (d) HSO 4 5. Give the missing information for each: Acid Base Reaction of the acid in water Solution 0 H 2 SO 4 HSO 4 (a) Solution 1 H 3 PO 4 (b) Solution 2 NO 3 (c) Solution 3 NH 4 + (d) Solution 4 CO 3 2 (e) Solution 5 HSO 4 (f) Solution 6 H 2 O 6. Give the missing information for each solution at 25ºC: (a) Solution 1 1.25 x 10 3 (b) Solution 2 5.00 x 10 5 H 2 SO 4 + H 2 O H 3 O + + HSO 4 [H 3 O + ] [OH ] ph poh (c) Solution 3 4.50 (d) Solution 4 6.40 7. A detergent box must bear a warning label if its contents will form a solution of ph greater than 11, because a strong base degrades protein structure. Should a box bear such a label if the H 3 O + concentration of a solution of its contents is 2.5 x 10 12 moles per liter? 8. A solution of ammonia has a hydronium ion concentration of 8.0 x 10 9 moles per liter. What is the poh of the solution? 9. The K w for pure water at 60ºC is 9.5 x 10 14. (a) Calculate the ph of pure water at 60ºC. (b) Is pure water at 60ºC acidic, basic, or neutral?
HOMEWORK 1F 1. For the following acids, write (1) the reaction for their ionization in water, and (2) their acid ionization constant expression. (a) HClO 2 (b) HCN (c) HCO 2 H 2. Rank the following acids from weakest to strongest: HOC 6 H 5, HClO 2, H 2 O, NH 4 +. 3. For the following bases, write (1) the reaction for their ionization in water, and (2) their base dissociation constant expression. (a) CH 3 NH 2 (b) F (c) NO 2 4. For the following acids, predict the numerical values for their acid ionizations constants. (a) HBrO 3 (b) HBrO 2 (c) HBrO 5. Calcualte the ph of each of the following strong acid and strong base solutions. (a) 0.001 M HCl (b) 0.02 M HNO 3 (c) 0.001 M NaOH (d) 0.001 M Ba(OH) 2 6. The acid ionization constant for arsenious acid, HAsO 2, is 6.0 x 10 10. (a) Calculate the ph of a 0.10 M solution of arsenious acid. (b) Calculate the poh of a 0.10 M solution of arsenious acid. 7. A 0.10 M solution of trichloroacetic acid, CCl 3 CO 2 H, is 1.3% ionized. (a) Calculate the K a for the acid. (b) Calculate the ph of the solution. 8. A solution is 0.25 M in nitrous acid. (a) Calculate the equilibrium concentration of NO 2 in the solution. (b) Calculate the ph of the solution. (c) Calculate the percent ionization of HNO 2. 9. The base dissociation constant for the organic base pyridine, C 5 H 5 N, is 1.58 x 10 8. (a) Calculate the concentration of C 5 H 5 NH + in a solution that was originally 0.10 M in pyridine. (b) Calculate the ph of the solution. 10. The base dissociation constant for the weak base hydrazine, N 2 H 4, is 2.0 x 10 6. Calcualte the molar concentration of hydrazine would yield a poh of 3.52.
HOMEWORK 1G 1. When sulfur dioxide gas is dissolved in water, it produces a 0.050 M sulfurous acid solution. (a) Calcualte the concentrations of H +, HSO 3, SO 2 3, and H 2 SO 3 in the sulfurous acid solution. (b) Calcualte the ph of the solution? 2. A solution is 0.30 M in sulfuric acid. (a) Calculate the concentrations of H +, HSO 4, SO 2 4, and H 2 SO 4 in the sulfuric acid solution. (b) Calcualte the ph of the solution? 3. A solution is 0.18 M in ammonium chloride. (a) Which ion is reacting with water? (c) What constant is used to calculate the ph? 4. A solution is 0.025 M in sodium acetate. (a) Which ion is reacting with water? (c) What constant is used to calculate the ph? (b) Is the solution acidic or basic? (d) Calculate the ph of the solution. (b) Is the solution acidic or basic? (d) Calculate the ph of the solution. 5. A 0.100 M solution of sodium iodite, NaIO 2, has a ph of 10.85. (a) Write the equation for the hydrolysis of NaIO 2. (b) Write the equilibrium constant expression for the hydrolysis reaction. Is it a K a or K b expression? (c) Calculate the value for the equilibrium constant in (b). (d) Calculate the acid ionization constant for HIO 2. HOMEWORK 1R 1. Write the K c and K p expressions for the following reactions. (a) 2CO 2 (g) 2CO (g) + O 2 (g) (b) PCl 3 (g) + 3NH 3 (g) 3HCl (g) + P(NH 2 ) 3 (g) (c) H 2 O (g) + C (s) CO (g) + H 2 (g) 2. At 298 K the equilibrium constant for the reaction: N 2 O 4 (g) 2NO 2 (g) is given by: K c = 4.63 x 10 3 (a) What is the numerical value of K c for the reaction: 2NO 2 (g) N 2 O 4 (g) (b) What is the numerical value of K c for the reaction: ½N 2 O 4 (g) NO 2 (g) (continued on next page)
3. The equilibrium constants for the following reactions are given: H 2 CO 3 (aq) HCO 3 (aq) + H + (aq) K c = 4.2 x 10 7 HCO 3 (aq) CO 3 2 (aq) + H + (aq) K c = 4.8 x 10 11 Calculate the equilibrium constant for the reaction: H 2 CO 3 (aq) CO 3 2 (aq) + 2H + (aq) 4. The equilibrium constant for the reaction: H 2 (g) + I 2 (g) 2HI (g) At 430ºC is 1.6 x 10 2. The reaction absorbs heat. Determine whether the reaction is spontaneous forward or in reverse, or whether it is at equilibrium. (a) A 1.0 L box contains 0.010 mole of H 2, 0.010 mole of I 2, and 0.40 mole of HI at 430ºC. (a) A 1.0 L box contains 0.10 mole of H 2, 0.10 mole of I 2, and 0.40 mole of HI at 430ºC. (a) A 1.0 L box contains 0.010 mole of H 2, 0.10 mole of I 2, and 0.40 mole of HI at 430ºC. 5. At 350.ºC, the equilibrium constant for the reaction: 2SO 3 (g) 2SO 2 (g) + O 2 (g) is given by: K p = 1.8 x 10 5 (a) What are the proper units (in atmospheres) for the given K p value? (b) What is the numerical value of K c for the reaction? (c) What would be the proper units for the K c? 6. Ammonium carbamate, NH 4 CO 2 NH 2, decomposes as follows: NH 4 CO 2 NH 2 (s) 2NH 3 (g) + CO 2 (g) Starting with only the solid, it is found that at 40 C the total gas pressure at equilibrium is 0.363 atm. Calculate the numerical value of K p with proper units. 7. Phosgene gas, COCl 2, can be prepared from carbon monoxide gas and chlorine gas as follows: CO (g) + Cl 2 (g) COCl 2 (g) 3.00 x 10 2 moles of pure phosgene gas was placed in a 1.50 L container, heated to 800. K, and at equilibrium the pressure of CO was found to be 0.497 atm. Calculate the numerical value of K p with proper units. 8. The equilibrium constant for the reaction: 2HF (g) H 2 (g) + F 2 (g) at a particular temperature is 3.6 x 10 35. A 0.500 L container is originally charged with 0.025 moles of H 2 and 0.025 moles of F 2, and allowed to reach equilibrium. Calculate the equilibrium concentrations, in moles per liter, of H 2 and F 2 in the container. (continued on next page)
9. Nitrosyl chloride, NOCl, decomposes as follows: 2NOCl (g) 2NO (g) + Cl 2 (g) When a 2.50 mole sample of NOCl was placed in a 1.50 L chamber at 400. C, and allowed to reach equilibrium, it was found to be 28.0% decomposed. Calculate the K p and K c for the reaction, with proper units for each. 10. At 500 K, the equilibrium constant for the reaction: SF 6 (g) SF 4 (g) + F 2 (g) is given by: K p = 2.50 x 10 1 A flask is originally charged with 0.500 atm of SF 6 and an unknown amount of F 2. At equilibrium the pressure of SF 6 was found to be 0.365 atm. Find the initial pressure of the F 2. 11. The following reaction produces the deep blue tetraamminecopper(ii) complex ion: Cu 2+ (aq) + 4NH 3 (aq) Cu(NH 3 ) 4 2+ (aq) To determine the equilibrium constant for the reaction above, an equilibrium solution was prepared by mixing together 10.00 ml of a 0.0750 M Cu(NO 3 ) 2 solution with 5.00 ml of a 0.600 M NH 3 solution. The absorbance of the equilibrium solution was measured at a wavelength of 546 nm in a 1.00 cm cuvet, and found to be 0.356. (a) Determine the initial concentrations of Cu 2+ and NH 3 in the equilibrium solution. (b) Using the calibration line to the right, determine the equilibrium concentration of Cu(NH 3 ) 4 2+ in the equilibrium solution. (c) Determine the equilibrium concentrations of Cu 2+ and NH 3 in the equilibrium solution (d) Determine the equilibrium constant for the given reaction. 12. The following reaction is exothermic: SO 2 (g) + Cl 2 (g) SO 2 Cl 2 (g) For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2) whether the new equilibrium moles of SO 2 Cl 2 will be higher, lower, or remain the same. (a) The addition of a catalyst (b) A decrease in the volume of the reaction container (c) Addition of SO 2 gas at constant volume (d) The removal of SO 2 Cl 2 gas at constant volume (e) An increase in temperature (f) Adding helium gas to the reaction container (continued on next page)
13. The following reaction is endothermic: 2Fe(OH) 3 (s) 2Fe 2 O 3 (s) + 3H 2 O (g) For each of the following disturbances, indicate (1) the direction the equilibrium will shift, and (2) whether the new equilibrium pressure of water vapor will be higher, lower, or remain the same. (a) The addition of a catalyst (b) A decrease in the volume of the reaction container (c) Addition of water vapor at constant volume (d) An increase in temperature (e) Adding argon gas to the reaction container (f) Addition of solid Fe(OH) 3 at constant volume. 14. For the following equilibrium reaction: Ag 2 CO 3 (s) 2Ag + (aq) + CO 3 2 (aq) write the net ionic equation for each of the following shifts, and underline the added substance that caused the shift. (a) The addition of AgNO 3 (aq) (b) The addition of NaCl (aq) (c) The addition of HCl (aq) 15. For the following acids, write (1) the reaction for their ionization in water, and (2) their acid ionization constant expression. (a) HClO 2 (b) NH 4 + 16. Rank the following acids from weakest to strongest: H 2 SO 4, H 2 SO 3, HSO 3, H 2 S, HS 17. Rank the following acids from weakest to strongest: HC 3 H 5 O 2, HNO 2, HBr, H 2 O, C 5 H 5 NH + 18. For the following bases, write (1) the reaction for their ionization in water, and (2) their base dissociation constant expression. (a) (CH 3 ) 3 N (b) C 6 H 5 O 19. Rank the following bases from weakest to strongest: NH 3, H 2 NNH 2, CH 3 NH 2 20. Rank the following bases from weakest to strongest: F, H 2 O, HCO 2 3, CO 3 21. What is the ph of each of the following strong acid or strong base solutions? (a) 0.015 M HClO 4 (b) 0.015 M Ca(OH) 2 (continued on next page)
22. Formic acid, HCO 2 H, is a weak acid. (a) Write the equation for the ionization of formic acid. (b) Write the equilibrium constant expression for the reaction. (c) If a 0.10 M formic acid solution has a ph of 2.39, what is formic acid s acid ionization constant? (d) If a 0.25 M formic acid solution is 2.7% ionized, what is the ph of the solution? 23. The acid ionization constant for benzoic acid, C 6 H 5 CO 2 H, is 6.5 x 10 5. (a) Write the equation for the ionization of benzoic acid. (b) Write the equilibrium constant expression for the reaction. (c) What is the ph of a 0.10 M solution of benzoic acid? (d) What is percent ionization of benzoic acid in a 0.10 M solution? 24. Propylamine is a weak base that reacts with water as follows: C 3 H 7 NH 2 + H 2 O C 3 H 7 NH 3 + + OH The base dissociation constant for this reaction, K b, is 4.8 x 10 6. (a) What is the concentration of C 3 H 7 NH 3 + in a solution that was originally 0.050 M in propylamine? (b) What is ph of the solution? 25. A solution is 0.250 M in ascorbic acid. (a) What are the concentrations of H 3 O +, HC 6 H 6 O 6, C 6 H 6 O 6 2, and H 2 C 6 H 6 O 6 in the solution? (b) What is the ph of the solution? 26. Predict whether the solutions of each of the following salts will be acidic, basic, or neutral. (a) KClO 3 (b) NH 4 NO 3 (c) NaC 2 H 3 O 2 (d) NH 4 CN 27. A solution is 0.035 M in ammonium bromide, NH 4 Br. (a) Write the equation for the hydrolysis of NH 4 Br. (b) Write the equilibrium constant expression for the reaction. (c) Calculate the ph of the solution. 28. A solution 0.035 M in sodium hypochlorite, NaClO, has a ph of 10.00. (a) Write the equation for the hydrolysis of NaClO. (b) Write the equilibrium constant expression for the reaction. (c) Calculate the value for the hydrolysis constant. (d) Calculate the acid ionization constant for HClO. Compare your answer with the value from Handout 3.
HOMEWORK 1R ANSWERS 1. (a) K c = [CO] 2 [O 2 ] K p = p 2 CO p O2 [CO 2 ] 2 2 p CO2 (b) K c = [HCl] 3 [P(NH 2 ) 3 ] K p = p 3 HCl p P(NH2)3 [PCl 3 ][NH 3 ] 3 3 p PCl3 p NH3 (e) K c = [CO][H 2 ] K p = p CO p H2 [H 2 O] p H2O 2. (a) 216 (b) 0.0680 3. 2.0 x 10 17 4. (a) reverse (b) forward (c) equilibrium 5. (a) atm (b) 3.5 x 10 7 (c) M 6. 7.09 x 10 3 atm 3 7. 3.3 atm 1 8. 6.0 x 10 19 M each 9. 1.95 atm, 3.53 x 10 2 M 10. 0.541 atm 11. (a) 0.0500 M Cu 2+, 0.200 M NH 3 (b) 0.0383 M Cu(NH 3 ) 4 2+ (c) 0.0117 M Cu 2+, 0.047 M NH 3 (d) 6.7 x 10 5 12. (a) none, none (b) right, higher (c) right, higher (d) right, lower (e) left, lower (f) none, none 13. (a) none, same (b) left, same (c) left, same (d) right, higher (e) none, same (f) none, same 14. (a) Ag 2 CO 3 (s) 2Ag + (aq) + CO 3 2 (aq) (b) Ag 2 CO 3 (s) + 2Cl (aq) 2AgCl (s) + CO 3 2 (aq) (c) Ag 2 CO 3 (s) + 2H + (aq) 2Ag + (aq) + H 2 O (l) + CO 2 (g) 15. (a) HClO 2 + H 2 O H 3 O + + ClO 2 K a = [H 3 O + ][ClO 2 ] [HClO 2 ] (b) NH + 4 + H 2 O H 3 O + + NH 3 K a = [H 3 O + ][NH 3 ] [NH + 4 ] (continued on next page)
16. HS, H 2 S and HSO 3 (tie), H 2 SO 3, H 2 SO 4 17. H 2 O, C 5 H 5 NH +, HC 3 H 5 O 2, HNO 2, HBr 18. (a) (CH 3 ) 3 N + H 2 O (CH 3 ) 3 NH + + OH K b = [(CH 3 ) 3 NH + ][OH ] [(CH 3 ) 3 N] (b) C 6 H 5 O + H 2 O C 6 H 5 OH + OH K b = [C 6 H 5 OH][OH ] [C 6 H 5 O ] 19. H 2 NNH 2, NH 3, CH 3 NH 2, 20. H 2 O, F, HCO 3, CO 3 2 21. (a) 1.82 (b) 12.48 22. (a) HCO 2 H + H 2 O H 3 O + + HCO 2 (b) K a = [H 3 O + ][HCO 2 ] [HCO 2 H] (c) 1.7 x 10 4 (d) 2.17 23. (a) C 6 H 5 CO 2 H + H 2 O H 3 O + + C 6 H 5 CO 2 (b) K a = [H 3 O + ][C 6 H 5 CO 2 ] [C 6 H 5 CO 2 H] (c) 2.59 (d) 2.5% 24. (a) 4.9 x 10 4 M (b) 10.69 25. (a) 0.0044 M H 3 O +, 0.0044 M HC 6 H 6 O 6, 1.6 x 10 12 M C 6 H 6 O 6 2, 0.246 M H 2 C 6 H 6 O 6 (b) 2.36 26. (a) neutral (b) acidic (c) basic (d) basic 27. (a) NH 4 + + H 2 O H 3 O + + NH 3 (b) K a = [H 3 O + ][NH 3 ] [NH + 4 ] (c) 5.36 28. (a) ClO + H 2 O HClO + OH (b) K b = [HClO][OH ] [ClO ] (c) 2.9 x 10 7 (d) 3.5 x 10 8