Primary Topics in Equilibrium
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1 Primary Topics in Equilibrium Outline 1. Equilibrium Expression 2. Calculating Concentration Given K 3. Calculating K Given Concentration Review 1. Equilibrium Expression (only gas and aqueous do not include solids or liquids) Kc: 2 SO 3 (g) 2 SO 2 (g) + O 2 (g) Kp: 2 NOCl (g) 2 NO (g) + Cl 2 (g) Ka: Weak acids like HF Kb: Weak bases like NH 3 Ksp: PbI 2 (s) Pb 2+ (aq) + 2 I - (aq) 2. Calculating Concentration Given K Kc: Given 0.10 M COCl 2, what are the equilibrium concentrations of CO and Cl 2 given the Kc = 2.19 x COCl 2 (g) CO (g) + Cl 2 (g) Solve for x when we assume 0.10 x x is the concentration of 1 mole of CO and 1 mole of Cl 2. Ka: Calculate the ph of a 0.30 M solution of acetic acid, HC 2 H 3 O 2, at 25 C. HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) K a for acetic acid at 25 C is Solve for x when we assume 0.30 x x = [H 3 O + ] so to find ph = - log [x] Kb: Same as Ka except x = [OH - ] so to find poh = - log [x], then ph = 14 - (poh) Ksp: Calculate the equilibrium solubility for the following equation given Ksp = 1.4 x 10-7 : Cu(IO 4 ) 2 (s) Cu 2+ (aq) + 2 IO - 4 (aq) Solve for x which is the concentration of 1 mole of Cu 2+. [IO - 4 ] = 2x.
2
3 3. Calculating K Given Concentration (Perform ICE) Kc: 0.35M of H 2 (g) and 0.22M of Br 2 (g) are initially placed in a container according the reaction below. At equilibrium the [H 2 ] = 0.14M. Calculate the Kc. H 2 (g) +Br 2 (g) 2HBr (g) I 0.35M 0.22M 0 M C -x -x +2x E 0.14M 0.22-x 2x E x = 0.14 x = 0.21 Ka: Calculate the Ka when 0.1M solution of a weak acid that has a ph of HA (aq) + H 2 O (l) H 3 O + (aq) + A - (aq) I 0.1 M 0 M 0 M C -x +x +x E = 0.09M 0.01 M 0.01 M Kb: Same as Ka, except may be given ph which must be converted to poh to calculate [OH - ] at equilibrium. Ksp: The molar solubility for PbBr 2 (s) is 0.01 mol L -1. Calculate the Ksp for this reaction. PbBr 2 (s) Pb +2 (aq) + 2Br - (aq) I 0 M 0 M C + x +2x E 0.01 M 2x E x = 0.01 (0.01) (0.02)
4 Equilibrium Expression 1. Write the expression of Kc for the following reactions. In each case, indicate whether the reaction is homogeneous or heterogeneous. a. 3 NO (g) N 2 O (g) + NO 2 (g) b. CH 4 (g) + 2 H 2 S (g) CS 2 (g) + 4 H 2 (g) c. Ni(CO) 4 (g) Ni (s) + 4 CO (g) d. HF (aq) H + (aq) + F - (aq) e. 2 Ag (s) + Zn 2+ (aq) 2 Ag + (aq) + Zn (s) 2. Write the expression for Kc for the following reactions. a. N 2 (g) + O 2 (g) 2 NO (g) b. Ti (s) + 2 Cl 2 (g) TiCl 4 (l) c. 2 C 2 H 4 (g) + 2 H 2 O (g) 2 C 2 H 6 (g) + O 2 (g) d. FeO (s) + H 2 (g) Fe (s) + H 2 O (g) e. 4 HCl (aq) + O 2 (g) 2 H 2 O (l) + 2 Cl 2 (g) 3. Write the expression for Kp for the following reactions. a. 2 NO (g) + O 2 (g) 2 NO 2 (g) b. 2 NO 2 (g) N 2 O 4 (g) c. 2 Cl 2 (g) + 2 H 2 O (g) 4 HCl (g) + O 2 (g) d. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) 4. Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solution. a. HBrO 2 b. HC 3 H 5 O 2 c. HC 6 H 5 O d. HCO 3 - e. HC 2 H 3 O 2 5. Write the chemical equation and the Kb expression for the ionization of each of the following bases in aqueous solution. a. (CH 3 ) 2 NH b. CO 3 2- c. CHO 2 - d. C 3 H 7 NH 2 e. C 6 H 5 CO 2-6. Write the expression for the solubility-product constant for each of the following strong electrolytes: a. AgI b. SrSO 4 c. Fe(OH) 2 d. PbI 2 e. Cu 3 (PO 4 ) 2
5 f. MnCO 3 Questions 7-10 (A) Kc (B) Kp (C) Ka (D) Kw (E) Ksp 7. The equilibrium constant uses partial pressures of gases as units. 8. This equilibrium constant always has a value of 1 x at 25 C. 9. This equilibrium constant is used for the dissociation of an acid. 10. The equilibrium expression for this equilibrium constant does not contain a denominator. Calculating Concentration Given K 11. At 2000 C, the equilibrium constant for the reaction below is Kc = 2.4 x NO (g) N 2 (g) + O 2 (g) If the initial concentration of NO is M, determine: a. The equilibrium constant expression. b. The equilibrium concentrations of NO, N 2, and O At 400 K, the equilibrium constant for the reaction below is Kc = 7.0 x Br 2 (g) + Cl 2 (g) 2 BrCl (g) If 0.30 mol of Br 2 and 0.30 mol of Cl 2 are introduced into a 1.0 L container, determine: a. The equilibrium constant expression. b. The equilibrium concentrations of Br 2, Cl 2, and BrCl. 13. At 373 K, Kp = for the equilibrium reaction below: 2 IBr (g) I 2 (g) + Br 2 (g) If the initial pressure of IBr is atm, determine: a. The equilibrium constant expression. b. The equilibrium pressures of IBr, I 2, and Br 2. (Hint: Do not assume x = 0.025) 14. At 298 K, Ka = 1.3 x 10-5 for a solution of 0.10 M propionic acid, HC 3 H 5 O 2. a. Develop the chemical equation for propionic acid. c. Calculate the ph when the solution comes to equilibrium. d. Calculate the percent ionization. 15. At 298 K, Ka = 6.8 x 10-4 for a solution of 0.05 M hydrofluoric acid, HF. a. Develop the chemical equation for hydrofluoric acid.
6 c. Calculate the ph when the solution comes to equilibrium. d. Calculate the percent ionization.
7 16. At 298 K, Kb = 1.7 x 10-9 for a solution of M pyridine, C 5 H 5 N. a. Develop the chemical equation for pyridine. c. Calculate the ph when the solution comes to equilibrium. d. Calculate the percent ionization. 17. At 298 K, Kb = 1.8 x 10-5 for a solution of M ammonia, NH 3. a. Develop the chemical equation for ammonia. c. Calculate the ph when the solution comes to equilibrium. d. Calculate the percent ionization. 18. At 25 C, the reaction below has an equilibrium constant Ksp = 7.1 x 10-4 : CaCrO 4 (s) Ca 2+ (aq) + CrO 4 2- (aq) b. Calculate the equilibrium concentrations of Ca 2+ and CrO 4 2- in a saturated solution of CaCrO At 25 C, the reaction below has an equilibrium constant Ksp =1.7 x 10-5 : PbCl 2 (s) Pb 2+ (aq) + 2 Cl - (aq) b. Calculate the equilibrium concentrations of Pb 2+ and Cl - in a saturated solution of PbCl 2. Calculating K Given Concentration 20. A mixture of 0.10 M NO, M H 2, and 0.10 M H 2 O is placed in a vessel at 300 K. The following equilibrium is established 2 NO (g) + 2 H 2 (g) N 2 (g) + 2 H 2 O (g) At equilibrium [NO] = M. b. Calculate the equilibrium concentrations of H 2, N 2, and H 2 O. c. Calculate Kc. 21. A mixture of 1.5 g of H 2 and 70.0 g of Br 2 is heated in a 2 L vessel at 700 K. These substances react as follows: H 2 (g) + Br 2 (g) 2 HBr (g) At equilibrium the vessel is found to contain 0.8 g of H 2. a. Calculate the initial concentrations of H 2, Br 2, and HBr. c. Calculate the equilibrium concentrations of H 2, Br 2, and HBr. d. Calculate Kc. 22. A flask contains 4.1 atm of CO 2, 2.1 atm of H 2, and 3.3 atm of H 2 O initially at 500 K according to the following reaction: CO 2 (g) + H 2 (g) CO (g) + H 2 O (g) At equilibrium the pressure of H 2 O is found to be 3.5 atm.
8 b. Calculate the equilibrium pressures of all substances. c. Calculate Kp. 23. A flask is charged with 1.50 atm of N 2 O 4 and 1.00 atm NO 2 at 298 K, and the following equilibrium is achieved: N 2 O 4 (g) 2 NO 2 (g) After equilibrium is reached, the partial pressures of NO 2 is 0.50 atm. b. Calculate the equilibrium partial pressures of N 2 O 4. c. Calculate the value of Kp for the reaction. 24. A solution of 0.10 M lactic acid, HC 3 H 5 O 3, has a ph of b. Calculate the Ka for lactic acid. 25. A M solution of phenylacetic acid, HC 8 H 7 O 2, is found to have a ph of b. Calculate the Ka for phenylacetic acid. 26. A M solution of ephedrine, C 10 H 15 ON, is found to have a ph of b. Calculate the Kb for ephedrine. 27. The molar solubility of PbBr 2 at 298 K is M. b. Calculate the Ksp for PbBr The ph of a solution of Fe(OH) 2 is found to be b. Calculate the equilibrium concentration of OH - (aq). c. Calculate the molar solubility. d. Calculate the Ksp for Fe(OH) X (g) + Y (g) 3 Z (g) The reaction mixture represented above is at equilibrium at 298 K, and the molar concentrations are [X] = 2.0 M, [Y] = 0.5 M, and [Z] = 4.0 M. What is the value of the equilibrium constant for the reaction at 298 K? (A) 0.50 (B) 2.0 (C) 4.0 (D) 16 (E) In a saturated solution of Zn(OH) 2 at 298 K, the value of [OH - ] is 2.0 x 10-6 M. What is the value of the solubility-product constant, Ksp, for Zn(OH) 2 at 298 K? (A) 4.0 x 10-18
9 (B) 8.0 x (C) 1.6 x (D) 4.0 x (E) 2.0 x 10-6
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