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Unformatted text preview: Chapter 10 1. Select the equilibrium expression for the reaction: P4(s) + 3KOH(aq) + 3 H2O(l) PH3(aq) + 3KH2PO2 (aq) ANS: E A) K = 1 [P4 ][H 2O]3 [KOH]3 B) K = [PH 3 ][KH 2PO 2 ]3 [PH 3 ][KH 2PO 2 ]3 C) K = [P4 ][KOH]3 [H 2O]3 [PH 3 ][KH 2PO 2 ]3 D) K = [KOH]3 [H 2O]3 E) K = [PH 3 ][KH 2PO 2 ]3 [KOH]3 2. The value of K for the reaction N2O4(g) 2NO2(g) at a given temperature is 0.211. If the equilibrium partial pressure of NO2 at the same temperature is 0.0172 bar, then what is the equilibrium concentration of N2O4? € A) 0.0815 B) 0.00664 C) 0.00140 D) 6.24×10–5 E) 0.0602 3. For which reaction does K = Kc (at the same temperatures)? A) C(s) + CO2(g) 2 CO(g) B) 2 SO2(g) + O2(g) 2 SO3(g) C) 2 BrCl(g) Br2(g) + Cl2(g) D) N2(g) + 3H2(g) 2 NH3(g) E) N2O4(g) 2NO2(g) 1 4. Calculate K for the reaction 2 SO2(g) + O2(g) 2 SO3(g) given the information below. SO3(g) ½ O2(g) + SO2(g) K = 4.0×10–13 A) 4.0 x 1024 B) 5.0 x 1012 C) 2.5 x 1012 D) 1.6 x 106 E) 6.3 x 1024 5. A mixture of 19.8 bar H2 and 12.8 bar Br2 was placed in a vessel at 700. K. At equilibrium, the vessel is found to contain 8.2 bar H2. What is K for the reaction? H2(g) + Br2(g) 2 HBr(g) A) 55 B) 14 C) 12 D) 1.2 E) 0.018 6. If ΔGrxn° = 27.1 kJ/mol at 25°C for the dissociation of acetic acid (CH3COOH) in aqueous solution, then which statement is true? CH3COOΗ(aq) + H2O(l) CH3COO–(aq) + H3O+(aq) A) At equilibrium, the concentration of products and reactants will be the same. B) At equilibrium, the concentration of products will be greater than that of reactants. C) At equilibrium, the concentration of products will be less than that of reactants. D) The reaction can never be in equilibrium. E) Because acetic acid is a weak acid, it doesn't generate H3O+ in water. 2 7. What is the equilibrium partial pressure of CO(g) if 4.50 g of C(s) and 0.500 bar of CO2(g) are placed in a reaction vessel and allowed to reach equilibrium at 1.00×103 °C, where K = 167.5. C(s) + CO2(g) 2 CO(g) A) 1.01 bar B) 0.998 bar C) 0.994 bar D) 0.988 bar E) 0.494 bar 8. Which changes to the system will cause the following reaction to shift right (toward products as written) to re-­‐attain equilibrium? N2O4(g) 2 NO2(g) ΔH° = 58.0 kJ/mol I) addition of NO2 II) addition of N2O4 gas III) increase in temperature A) I only B) II only C) III only D) I and III E) II and III 9. Which statement is false? A) The rate of the forward reaction is equal to the rate of the reverse reaction when Q = K . B) The rate of the forward reaction is greater than that of the reverse reaction when Q < K. C) When Q = K, ΔGrxn° = 0. D) When Q = K, no macroscopic change in reaction composition can be observed. E) All of these statements are true. 3 10. Which statement is true? A) When the value of Q is large, the equilibrium must lie on the product side of the equilibrium reaction. B) When the value of K is large, the equilibrium lies on the reactant side of the equilibrium reaction. C) A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products. D) A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. E) When the value of K is small, the value of Q for the same reaction will also be small. 11. The equilibrium constant, Kc for the reaction 2 NOCl(g) 2 NO(g) + Cl2(g) is 0.51 at a certain temperature. A mixture of the three gases with the following composition was introduced into a container at this temperature. Which statement is true? [NOCl] = 1.3 M [NO] = 1.2 M [Cl2] = 0.60 M A) B) C) D) E) Cl2(g) is produced until equilibrium is reached. [NOCl] = [NO] = [Cl2] at equilibrium. NOCl(g) is produced until equilibrium is reached. [Cl2] = 0.30 M at equilibrium. No apparent reaction takes place. 12. For the following reaction, when the volume of the container is reduced: 3 Fe(s) + 4 H2O(g) 4 H2(g) + Fe3O4(s) A) the equilibrium constant increases B) more H2(g) is produced C) no change occurs D) more H2O(g) is produced E) more Fe(s) is produced 4 13.The equilibrium constant K for the synthesis of ammonia gas from nitrogen and hydrogen gas is 6.8 x 105 at 298 K. Predict its value at 400. K using any of the pertinent information below. ΔGorxn = -­‐ 16.45 kJ/mol ΔHorxn = -­‐ 92.22 kJ/mol A) 1.0 B) 140 C) 7.6 x 10-­‐5 D) 6.7 x 105 E) 51 14. Which statement properly identifies and labels the conjugate acid-­‐base pairs in the reaction: NO2–(aq) + H2PO4-­‐(aq). HNO2(aq) + HPO42-­‐(aq) Acid 1 Base1 Acid 2 Base 2 A) HNO2 HPO42– NO2– H2PO4– B) H2PO4– NO2– HPO42– HNO2 C) NO2– HNO2 HPO42– H PO – 2 4 D) HNO2 NO2– H2PO4– HPO42– E) HPO42– H2PO4– HNO2 NO2-­‐ 15. The equilibrium constant, Kc , is unitless because: A) Solids and pure liquids are not included in the equilibrium expression. B) At equilibrium, all reagents are at standard state (1M or 1 bar). C) In equilibrium reactions, the number of reactant atoms/molecules always equals the number of product atom/molecules. D) Equilibrium expression are written in terms of activities, not concentrations. E) None of these is true. 5 16. A mixture of N2, H2, and NH3 with partial pressures of 0.22 bar, 0.44 bar, and 0.18 bar, respectively, was prepared and heated to 500. K at which temperature K = 0.036. Which statement is true? N2(g) + 3 H2(g) 2 NH3(g) A) NH3 tends to decompose under these conditions. B) NH3 tends to form under these conditions. C) The partial pressure of NH3 remains constant. D) Q = 1.86 under these conditions. E) NH3 forms regardless of conditions. 17. Which equation best matches the equilibrium constant expression below? 2+ [Cu ] Kc = + 2 [Ag ] A) Cu(aq) + 2Ag2+(aq) Cu2+(aq) + Ag(aq) B) 2Ag(aq) + Cu2+(aq) Cu(aq) + 2Ag2+(aq) C) 2Ag(s) + Cu2+(aq) Cu(s) + 2Ag2+(aq) D) Cu(s) + 2Ag+(aq) 2Ag(s) + Cu2+(aq) E) 2Cu(s) + Ag+(aq) Cu2+(aq) + 2Ag(s) 18. What is the value of K for the reaction N2O(g) + ½ O2(g) 2NO(g) given the information below? N2(g) + ½ O2(g) N2O(g) K = 2.7x10-­‐18 N2(g) + O2(g) 2NO(g) K = 4.7x10-­‐31 A) 5.9 x 1012 B) 2.7 x 10-­‐18 C) 1.7 x 10-­13 D) 1.3 x 10-­‐48 E) 3.7 x 1017 € 6 19. The following were placed in a 1.00 L reaction vessel: 1.00 mol CO 1.00 mol H2O 2.00 mol CO2 2.00 mol H2 If Kc = 1.00 at 1100 K for the reaction below, then which statement is true? CO(g) + H2O(g) CO2(g) + H2(g) A) The concentration of CO at equilibrium is less than the initial concentration. B) The concentration of CO2 at equilibrium is greater than the initial concentration. C) K for the reaction is greater than Kc (at the same temperature). D) The equilibrium concentration of H2 can be represented as 2.00 – x. E) All of these statements are true. 20. A 1.00 bar sample of H2S is allowed to decompose at 1405 K until equilibrium is achieved. At equilibrium, the partial pressure of S2 is 0.037 bar. What is the value of K for this reaction? 2H2S(g) S2(g) + 2H2(g) A) 2.36x10-­‐4 B) 2.96x10-­‐3 C) 1.42x10-­‐3 D) 4.24x103 E) 7.04x102 21. Which statement is true? 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g) ΔHo = -­‐150 kJ A) Reducing the volume of the system causes equilibrium to shift to the right toward products. B) Decreasing the pressure of the system causes the equilibrium to shift to the left toward reactants. C) Decreasing the temperature shifts the reaction right toward products. D) Increasing the partial pressure of H2O shifts the reaction left toward reactants. E) The addition of O2 to the systems shifts the reaction to the right toward products. 7 22. At a particular temperature, Kc = 2.5 x 1010 for the reaction 2SO2(g) + O2(g) 2SO3(g) What is Kc for the reaction SO3(g) SO2(g) + ½ O2(g) A) 4.0 x 10-­‐11 B) 1.6 x 10-­‐21 C) 6.3 x 10-­‐6 D 6.3 x 1020 E)1.6 x 105 23. The value of K at 308 K is 6.5x104 for the reaction of NO(g) with chlorine gas to form NOCl(g). If PNO = 0.35 bar and PNOCl = 0.10 bar at equilibrium, then what is the equilibrium partial pressure of the chlorine gas? A) 2.3 x 105 B) 4.3 x 10-­‐6 C) 1.9 x 103 D) 5.4 x 10-­‐4 E) 1.3 x 10-­‐6 24. Which statement is true? A) All reaction quotients are equilibrium constants. B) If K > Q, then the reaction must shift to the reactants (left) to re-­‐attain equilibrium. C) If Q < K, then the reaction is nonspontaneous. D) Not all equilibrium constants are reaction quotients. E) If Q > K, the reaction must proceed in a direction to reduce the amount of products present or increase the amount of reactants. 25. What is the expression for the reaction quotient for the reaction: 4NO2(g) + O2(g) 2N2O5(s) ANS: E (PN 2 O 5 ) 2 A) Q = (PNO 2 ) 4 (PO 2 ) (PN 2 O 5 ) B) Q = 4 (P ) (P ) NO O 2 2 € C) Q = (PNO 2 ) 4 (PO 2 ) € € 8 D) Q = E) Q = 1 (PN 2 O 5 ) 2 1 (PNO 2 ) 4 (PO 2 ) € 27. At 425oC, K = 4.18 x 10-­‐9 for the reaction 2HBr(g) H2(g) + Br2(g). If 0.20 bar of HBr(g), and 0.010 bar of both H2(g) and Br2(g) are introduced into a container, € which expression best represents the equilibrium pressure of HBr? then A) 0.20 – x B) 0.20 – 2x C) 0.20 + x D) 0.20 + 2x E) 0.010 + x 28. An evacuated 2.00 L flask was filled with 0.200 mol HI gas which decomposed according to the following equation at 453oC. At equilibrium, the concentration of HI was 0.078 M. What is Kc for this reaction at 453oC? 2HI(g) ⇌ H2(g) + I2(g) A) 0.020 B) 0.011 C) 0.0016 D) 1.8 E) 0.14 29. Which equation correlates with the equilibrium constant expression: A) 3D(g) + 2E(g) ⇌ 2C(g) B) 2C(g) ⇌ D(g) + E(g) C) A(s) + B(l) + 2C(g) ⇌ 3D(g) + 2E(g) D) 3D(g) + 2E(g) ⇌ 2C(g) + 2B(s) E) None of these equations correlate to the equilibrium constant expression given. 9 30. Molecular iodine decomposes according to the following reaction, for which Kc = 3.76 x 10-­‐3 at 1000oC. If 0.45 mol of I2 is placed in a 3.0 L container, what is the equilibrium concentration of I(g) at 1000oC? I2(g) ⇌ 2I(g) A) 0.011 M B) 0.023 M C) 0.00028 M D) 0.00056 M E) 0.15 M 32. The value of ΔGo for the reaction below is -­‐141.6 kJ/mol at 298 K. What is the value of K for the reaction at 298K? O2(g) + 2SO2(g) ⇌ 2SO3(g) A) 0.944 B) 1.51 x 10-­‐25 C) 6.62 x 1024 D) 1.06 E) 1.42 x 1057 33. Which statement is true? A) A reaction with Q greater than 1 must be product favored. B) At equilibrium, the concentration of reactants is equal to the concentration of products. C) If K is less than 1, then the pressure of reactant is greater than that of product and the system is not at equilibrium. D) Q cannot be negative. E) K can have a value anywhere from negative infinity to positive infinity. 34. Which statement is true? A) All Q are K. B) The values of K and Kc for a given reaction can never be the same. C) For a reaction to be at equilibrium, K must equal 1. D) If Q = 64 and K = 5.7 for a given reaction, then the reaction must proceed to the left to re-­‐attain equilibrium. E) None of these statements are true. 10 35. Use the information given below to find Kc for the reaction CO2(g) + H2(g) ⇌ H2O(g) + CO(g) 2H2O(g) ⇌ 2 H2(g) + O2(g) Kc = 1.6 x 10-­‐11 2CO2(g) ⇌ 2CO(g) + O2(g) A) B) C) D) E) Kc = 1.3 x 10-­‐10 8.1 0.12 0.35 7.1 x 105 2.9 Chapter 11 1. What is the conjugate base of CH3NH3+ in H2O? A) CH3NH42+ B) CH3NH2 C) H3O+ D) OH– E) None of these 2. Which of these species is most likely to be completely deprotonated in aqueous solution? A) HNO2 B) HF C) CH3COOH D) HCN E) HClO4 3. Which statement(s) correctly pairs the definition with the acid/base theory? A) Bronsted-­‐Lowry bases are proton donors. B) Arrhenius bases produce hydronium ions in aqueous solution. C) Lewis bases are electron pair donors. D) Bronsted-­‐Lowry acids are proton acceptors. E) All of these are true. 11 4. Which of the following is the weakest acid? A) HCN (pKa = 9.31) B) HIO3 (pKa = 0.77) C) HF (pKa = 3.45) D) CH3COOH (pKa = 4.75) E) HNO2 (pKa = 3.37) 5. Which oxoacid is strongest? A) HIO B) HClO3 C) HClO D) HBrO E) HClO4 6. The pH of 0.800 M aqueous benzenesulfonic acid (a monoprotic acid) is 0.51. What is the value of Ka for benzenesulfonic acid? A) 0.19 B) 0.12 C) 0.90 D) 0.44 E) 0.51 7. What is the pH of a 0.25 M HBrO(aq) solution? (pKa = 8.69) A) 5.90 B) 0.60 C) 8.10 D) 4.65 E) 9.30 8. The equation that represents Ka2 for phosphoric acid is A) HPO42–(aq) + H2O(l) ↔ PO43–(aq) + H3O+(aq) B) H2PO4–(aq) + H2O(l) ↔ HPO42–(aq) + H3O+(aq). C) H3PO4(aq) + 2H2O(l) ↔ HPO42–(aq) + 2H3O+(aq). D) HPO42–(aq) + H2O(l) ↔ H2PO4–(aq) + OH–(aq). E) H3PO4(aq) + H2O(l) ↔ H2PO4–(aq) + H3O+(aq). 9. What is the pH of a 0.026 M solution of NaOH? A) 1.59 B) 0.026 C) 12.41 D) 13.97 E) The pH cannot be calculated without the Kb of NaOH. 12 10. Which of the following salts are acidic in H2O? I) NaBr II) NH4Br III) NaF IV) FeCl3 A) I and III B) III and IV C) I and II D) IV only E) II and IV 11. All of the following can act as Lewis bases except A) OH B) H2O C) Al2O3 D) Br– Ε) All of these may act as Lewis bases − 12. All of the following acids have the same strength in water except A) HNO3 B) HClO3 C) HBr D) HF E) They all have the same strength 13. What is the [OH-­‐] concentration in a cup of coffee with pH = 4.27? A) 9.7 M B) 2.0x10-­‐5 M C) 1.9x10-­‐10 M D) 5.5x10-­‐5 M E) 5.4x109 M 14. What is the pH of a 0.013 M solution of HBr? A) 1.89 B) 1.59 C) 12.41 D) 12.11 E) 3.78 13 15. The pH of a 0.042 M solution of a weak acid, HA, is 2.79. What is the Ka for this acid? A) 6.3x10-­‐5 B) 5.2x10-­‐5 C) 1.6x10-­‐3 D) 0.040 E) 0.45 16. What is the pH of a 0.167 M solution of C6H5NH2? The Kb of C6H5NH2 is 7.4x10-­‐10 and the Ka of C6H5NH3+ is 1.4x10-­‐5. A) 11.184 B) 13.227 C) 0.777 D) 4.954 E) 9.046 17. Which acid is strongest? A) HCN, pKa 9.21 B) HN3, pKa = 4.72 C) HNO2, pKa = 3.14 D) HBrO, pKa = 8.60 E) H2O2, pKa = 11.66 18. Identify the two conjugate acid – base pairs in the reaction below. Acids are listed first in each pair, followed by that acid's conjugate base. HIO2(aq) + (CH3)2NH(aq) IO2-­‐(aq) + (CH3)2NH2+(aq) Pair One Pair Two A) HIO2 and (CH3)2NH IO2-­‐ and (CH3)2NH2+ B) HIO2 and (CH3)2NH2+ IO2-­‐ and (CH3)2NH + C) (CH3)2NH2 and HIO2 (CH3)2NH and IO2-­‐ D) HIO2 and IO2-­‐ (CH3)2NH2+ and (CH3)2NH -­‐ E) IO2 and HIO2 (CH3)2NH and (CH3)2NH2+ 19. Which statement is true? A) NH3 is a Bronsted-­‐Lowry base because it is a proton donor. B) The bromide ion is a Lewis base, but not a Bronsted-­‐Lowry base. C) Water can be a Bronsted-­‐Lowry acid OR a Lewis base. D) Metal cations tend to be Lewis acids due to their ability to donate electron pairs. E) HSO4-­‐ is neither an acid nor a base under any theory. 14 20. Which statement regarding a solution of 0.0100 M NaNO2 is true? A) The pH of the solution is acidic because HNO2 is a weak acid that + undergoes acid hydrolysis to produce H3O in solution. B) The pH of the solution is neutral because it was made from a strong base and a weak acid. C) The pH of the solution is basic because NaOH is a strong base that -­‐ undergoes base hydrolysis to produce OH in solution. D) The pH of the solution is acidic because the conjugate acid of NaOH + undergoes acid hydrolysis to produce H3O in solution. E) The pH of the solution is basic because the conjugate base of HNO2 -­‐ undergoes base hydrolysis to produce OH in solution. 21. At 50.0oC, pKw = 13.262. What is the pH of pure water at this temperature? A) 7.00 B) 7.37 C) 6.63 D)13.30 E) 0.70 22. The hydrogen sulfate or bisulfate ion HSO4– can act as either an acid or a base in water solution. In which of the following equations does HSO4– act as an acid? A) HSO4– (aq) + H2O(l) → H2SO4 (aq) + OH– (aq) B) HSO4– (aq) + H3O+ (aq) → SO3 (aq) + 2 H2O (l) C) HSO4– (aq) + OH– (aq) → H2SO4 (aq) + O2–(aq) D) HSO4– (aq) + H2O (l) → SO42– (aq) + H3O+ (aq) E) none of these 23. Which species is least likely to be completely deprotonated in aqueous solution? A) HNO3 B) HF C) HCl D) HBr E) HClO4 24. Which statement is true? A) NH3 is a Bronsted-­‐Lowry base because it is a proton donor. B) The bromide ion is a Lewis base, but not a Bronsted-­‐Lowry base. C) Water can be a Bronsted-­‐Lowry acid AND a Lewis base. D) Metal cations tend to be Lewis acids due to their ability to donate electron pairs. E) HSO4-­‐ is neither an acid nor a base under any theory. 15 25. What is the conjugate base of HPO42-­‐ ? A) PO43-­‐ B) H3PO4 C) H2PO4-­‐ D) HPO4 E) H2PO4 26. What is the pH of a 0.0147 M solution of KOH at room temperature? A) 1.83 B) 12.17 C) 13.98 D) 12.47 E) 1.53 27. Which base is weakest? A) BrO4-­‐ B) BrO3-­‐ C) IO4-­‐ D) BrO-­‐ E) IO-­‐ 28. Which statement regarding a solution of 0.0100 M NaNO2 is true? A) The pH of the solution is acid because HNO2 is a weak acid that + undergoes acid hydrolysis to produce H3O in solution. B) The pH of the solution is neutral because it was made from a strong base and a weak acid. C) The pH of the solution is basic because NaOH is a strong base that undergoes base hydrolysis to produce OH-­‐ in solution. D) The pH of the solution is acidic because the conjugate acid of NaOH undergoes acid hydrolysis to produce H3O+ in solution. E) The pH of the solution is basic because the conjugate base of HNO2 undergoes base hydrolysis to produce OH-­‐ in solution. 29. Which of the following species would be found in a 1.0M aqueous solution of HCl at 298K? I. H2O III. Cl-­‐ V. H+ + II. H3O IV. HCl A) I, II, and III B) II, III, and IV C) III, IV, and V D) All of the species E) Not enough information is provided 16 30. If pKa for a known acid HA is 1.39, what is the value of pKw at 25°C? A) 2.45 x 10-­‐13 B) 14 C) 1.39 D) 12.6 E) 0.041 31. An aqueous solution of which substance could have pH = 5.95? A) KNO3 B) Ca(CN)2 C) NaF D) CH3NHCl E) Li2SO4 32. What is the pH a 0.0237 M solution of NaOH? A) 12.375 B) 1.625 C) 0.00237 D) -­‐1.625 E) There is not enough information. 33. What is the pH of a 0.244 M solution of H3BO3? A) 0.610 B) 13.4 C) 0.914 D) 13.1 E) There is not enough information. 34. Which statement is true? A) NH3 is a Bronsted-­‐Lowry base because it is a proton donor. B) The fluoride ion is a Lewis base, but not a Bronsted-­‐Lowry base. C) Water can be a Bronsted-­‐Lowry acid AND a Lewis base. D) Metal cations tend to be Lewis acids due to their ability to donate electron pairs. E) HSO4-­‐ is neither an acid nor a base under any theory. 17 35. Which of the following statements is true? A) Ka values are the same for all 3 protons in H3PO4. B) Ka1 > Ka2 > Ka3 for any triprotic acid. C) pKa1 + pKa2 + pKa3 = 14 for a triprotic acid. D) Ka1 < Ka2 < Ka3 for any triprotic acid. E) Two of these statements are true. 36. Sodium bicarbonate undergoes thermal decomposition according to the reaction below. Which of the following would cause the equilibrium to shift to produce more CO2(g)? 2NaHCO3(s) ⇌ NaCO3(s) + CO2(g) + H2O(g) I. Addition of 0.20 atm of argon gas II. Removal of NaHCO3(s) III. Removal of H2O(g) A) I only B) II only C) III only D) I and II E) II and III 37. Which base is weakest? A) BrO4-­‐ B) BrO3-­‐ C) IO4-­‐ D) BrO-­‐ E) IO-­‐ 38. What is the conjugate base of H3AsO4? A) AsO43-­‐ B) H4AsO4 C) HAsO42-­‐ D) H2AsO4-­‐ E) H3AsO3-­‐ 18 39. What concentration of NH3 is required to have the same pH as a 0.010 M solution of LiOH? The Kb for NH3 is 1.8 x 10-­‐5. A) 0.010 M B) 2.4 M C) 560 M D) 5.6 M E) There is not enough information. Chapter 12 1. 100 mL of each of the following solutions is mixed. Which one of the mixed solutions is a buffer? A) 1.0 M NH3(aq) + 0.6 M KOH(aq) B) 1.0 M NH4Cl(aq) + 1.0 M KOH(aq) C) 1.0 M NH3(aq) + 0.4 M HCl(aq) D) 1.0 M NH4Cl(aq) + 0.4 M HCl(aq) E) 1.0 M NH3(aq) + 1.0 M HCl(aq) 2. Choose the effective pH range of an aniline/anilinium chloride buffer. The value of the Kb for aniline is 4.3 × 10–10. A) 3.6–5.6 B) 8.4–10.4 C) 1.1–3.1 D) 5.1–7.1 E) 10.1–12.1 3. A buffer solution made of NH3 and NH4NO3 (Kb for NH3 = 1.8x10–5). If the pH of the buffer is 9.26 and the concentration of NH4NO3 is 0.175 M, then what is the concentration of NH3? A) 0.0387 M B) 0.175 M C) 0.757 M D) 0.831 M E) 0.452 M 4. If a small amount of a strong base is added to buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solu...
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