3. The ph of 0.40 M aqueous CH 3 COOH will be. A) 2.57 B) 3.45 C) 4.12 D) 5.17

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1 1. Addition of the common ion, CH 3 COO, to a CH 3 COOH solution. A) decreases the ph of the solution B) increases the ph of the solution C) increases the concentration of H + D) has no effect on the ph of the solution 2. The following salts were added to aqueous solution of their respective acids or bases. Which addition causes no change in ph? A) Potassium acetate to acetic acid B) HCOO Na to HCOOH C) KCl to HCl D) NH 4 NO 3 to NH 3 (aq) 3. The ph of 0.40 M aqueous CH 3 COOH will be. A) 2.57 B) 3.45 C) 4.12 D) The ph of a solution containing 0.40 M CH 3 COOH and 0.20 M CH 3 COONa is. A) 3.33 B) 2.22 C) 5.55 D) The ph of a 0.20 M aqueous NH 3 solution is. A) 8.92 B) C) 9.82 D) The ph of a solution containing 0.20 M NH 3 and 0.30 M NH 4 Cl is. A) 8.09 B) C) 9.07 D) Page 1

2 7. A buffer solution can be prepared by mixing a in required proportions A) weak acid and its salt with a strong base B) weak acid and its salt with a weak base C) weak base and its salt with a weak acid D) strong acid and its salt with a strong base 8. Which of the following represents the pk a of an acid? A) 1/log K a B) log 1/K a C) log K a D) log 1/K a 9. The pk a values of acids A, B, C and D are 5.9, 8.1, 4.7 and 6.9, respectively. The strongest acid is. A) C B) B C) A D) D 10. Which of the following would be a buffer solution? A) KCl / HCl B) NH 3 / NH 4 Cl C) Na 2 SO 4 / H 2 SO 4 D) KNO 3 / HNO Which of the following would not be a buffer solution? A) CH 3 COOK / CH 3 COOH B) HCN / NaCN C) NaClO 4 / HClO 4 D) NaHCO 3 / H 2 CO The ph of a buffer solution containing 0.15 M NH 3 and 0.35 M NH 4 Cl is. A) 8.88 B) 10.8 C) 9.77 D) Page 2

3 13. The ph of a buffer containing 0.20 M CH 3 COOH and 0.20 M CH 3 COONa is. A) 3.72 B) 5.45 C) 5.01 D) The ph of a bicarbonate (HCO 3 )-carbonic acid (H 2 CO 3 ) buffer is The ratio of the concentration of H 2 CO 3 to HCO 3 is. A) 2.4 B) C) 0.24 D) The ph of a buffer solution containing 0.10 M Na 2 HPO 4 and 0.15 M KH 2 PO 4 is. A) 7.03 B) 3.51 C) D) The ph of a CH 3 COONa / CH 3 COOH buffer is The ratio of [CH 3 COO - ] / [CH 3 COOH] is. A) 0.33 B) 0.45 C) 0.25 D) The ph of blood plasma is Assuming that the buffer action is due to HCO 3 /H 2 CO 3 the ratio of [HCO 3 ] / [H 2 CO 3 ] is. A) 2.0 B) 10. C) 4.0 D) The ph of a buffer containing 0.20 M NH 3 and 0.20 M NH 4 Cl is. A) 8.25 B) 9.25 C) D) Page 3

4 19. What is the ph of the 0.20 M NH 3 / 0.20 M NH 4 Cl buffer after the addition of 10.0 ml of 0.10 M HCl to 65.0 ml of the buffer. A) 8.05 B) 9.58 C) D) The ph of 1.00L of the buffer containing 1.0 M CH 3 COONa and 1.0 M CH 3 COOH is. A) 2.37 B) 4.74 C) 3.74 D) The ph of 1.00L of the buffer containing 1.00 M CH 3 COONa and 1.00 M CH 3 COOH after the addition of mole NaOH is. A) 3.82 B) 6.12 C) 4.81 D) The ph of 1.00L of the buffer 1.00 M CH 3 COONa / 1.00 M CH 3 COOH after the addition of 0.12 mol HCl is. A) 4.64 B) 4.96 C) 3.86 D) The ionization constants of a diprotic acid, H 2 A, are and To obtain a buffer of ph 5.8 you would use. A) NaHA + H 2 A B) Na 2 A + NaHA C) Na 2 A + H 2 A D) NaHA + Na 2 A + H 2 A Page 4

5 24. Which of the following weak acids is suitable for preparing a buffer of ph 8.6? HA (K a = ), HB (K a = ), HC (K a = ), HD (K a = ) A) HD B) HA C) HB D) HC g of a monoprotic acid neutralizes 16.4 ml of M KOH. The molar mass of the acid is g/mol. A) 105 B) 304 C) 154 D) g of a diprotic acid was dissolved in water to make ml of solution. If 25.0 ml of this solution required 11.1 ml of 1.00 M KOH for complete neutralization, the molar mass of the acid is. A) 180 g mol 1 B) 90.1 g mol 1 C) 45.5 g mol 1 D) 270 g mol In a titration experiment 12.5 ml of M H 2 SO 4 neutralized 50.0 ml of NaOH. The concentration of the NaOH solution is. A) M B) M C) M D) M 28. In a titration experiment, 20.4 ml of M HCOOH neutralized 19.3 ml of Ba(OH) 2. The concentration of Ba(OH) 2 solution is. A) M B) M C) M D) M Page 5

6 29. A g sample of a monoprotic acid was dissolved in 25.0 ml water and titrated with M NaOH. The acid required 18.4 ml of the base to reach the equivalence point. The molar mass of the acid is g mol 1 A) 54.8 B) 95 C) 110 D) g of a monoprotic acid (molar mass 110 g/mol) was dissolved in 25.0 ml of water. The ph of the solution was found to be 5.87 after the addition of 10.0 ml of M NaOH. The K a of the acid is. A) B) C) D) Exactly 500 ml of M NaOH was mixed with exactly 500 ml M CH 3 COOH. The equilibrium concentration of OH is. A) M B) M C) M D) M 32. The ph at the equivalence point of the titration of 0.20 M HCl vs M methylamine is. A) 8.42 B) C) 9.18 D) The ph at the equivalence point in the titration of 0.10 M HCOOH versus 0.10 M NaOH is. A) 4.61 B) 8.23 C) 5.75 D) Page 6

7 34. The ionization constant K a of an indicator is The color of the non-ionized form is red and that of the ionized form is yellow. The color of the indicator at ph 4 is. A) green B) red C) yellow D) orange 35. The K a of an indicator is It is green in the nonionized form and red in the ionized form. The indicator will change its color at a ph of. A) 2.7 B) 8.3 C) 6.3 D) The solubility product of silver chromate (Ag 2 CrO 4 ) is given by. A) [Ag + ] [CrO 4 2 ] B) [Ag + ] 2 [CrO 4 2 ] C) [Ag + ][CrO 4 2 ] 2 D) [CrO 4 2 ] / [Ag + ] 37. The solubility product of mercury(i) chloride (Hg 2 Cl 2 ) is given by. A) [Hg + ] [Cl ] B) [Hg + ] 2 [Cl ] 2 C) [Hg 2 2+ ] [Cl ] D) [Hg 2 2+ ] [Cl ] The solubility product of manganese(ii) phosphate, Mn 3 (PO 4 ) 2 is given by. A) [Mn 2+ ] 2 [PO 4 3 ] 3 B) [Mn 2+ ] [PO 4 3 ] C) [Mn 2+ ] 3 [PO 4 3 ] 2 D) [Mn 2+ ] [PO 4 3 ] For precipitation to occur from a solution: A) ph > poh B) ion product > solubility product C) ion product < solubility product D) ion product = solubility product Page 7

8 40. The concentration of I in a saturated AgI solution with [Ag + ]= M is. A) M B) M C) M D) M 41. The concentration of Al 3+ in a saturated Al(OH) 3 solution with [OH ] = M is. A) M B) M C) M D) M 42. The solubility of SrF 2 is g/l. The solubility product for SrF 2 is. A) M B) M C) M D) M 43. The solubility of silver phosphate, Ag 3 PO 4, is g/l. Its solubility product is. A) B) C) D) The molar solubility of MnCO 3 is M. The K sp of the compound is. A) B) C) D) The solubility of an ionic compound MX (molar mass = 346 g) is g/l. Its K sp is. A) B) C) D) Page 8

9 46. The solubility of an ionic compound M 2 X 3 (mw = 288) is g/l. Its K sp is. A) B) C) D) The solubility product of calcium fluoride, CaF 2, is Its solubility is M. A) B) C) D) The ph of a saturated solution of Zn(OH) 2 is. A) 8.53 B) 9.53 C) D) The ph of a saturated solution of MOH is Its K sp will be. A) B) C) D) ml of M NaF is mixed with 25 ml of 0.15 Sr(NO 3 ) 2. The concentration of F in the final solution is. (K sp of SrF 2 is ) A) M B) C) D) Page 9

10 51. Solid NaI is added to a solution containing 0.01 M each of Cu +, Ag +, K + and Mg 2+. The ion that gets precipitated first is. A) Ag + B) Mg 2+ C) K + D) Cu A ph that is suitable for the separation by precipitation of Fe(OH) 3 from a solution that is initially M in both Fe 3+ and Zn 2+ is. A) 3.5 B) 8.5 C) 1.5 D) The solubility of CaCO 3 decreases in the presence of. A) CO 2 B) Na 2 CO 3 C) HCl D) NaCl 54. Which of the following statements is true with respect to AgCl? A) K sp is same as its solubility. B) K sp of AgCl is the same in M AgNO 3 as in water. C) The solubility of AgCl is independent of the concentration of AgNO 3. D) [Ag + ] in solution changes significantly after the addition of AgCl to M AgNO How many grams of CaCO 3 will dissolve in ml of M Ca(NO 3 ) 2? A) g B) g C) g D) g 56. The solubility product of PbBr 2 is Its solubility in 0.20 M KBr solution is. A) M B) M C) M D) M Page 10

11 57. Lead bromide will have the greatest molar solubility in 0.10 M. A) KBr B) MgBr 2 C) Pb(NO 3 ) 2 D) NaBr. 58. The molar solubility of AgCl in a solution made by dissolving 10.0g of CaCl 2 in 1.00 L of solution is. A) M B) M C) M D) M 59. The molar solubility of BaSO 4 in a solution containing 1.0 M SO 4 2 ions is. A) M B) M C) M D) M 60. Which of the following compounds is not more soluble in acid than in water? A) BaSO 4 B) PbCl 2 C) Fe(OH) 3 D) HgS 61. A compound that is more soluble in HCl (aq) than in water is. A) CaCO 3 B) BaI 2 C) AgCl D) Hg 2 Cl The compound below whose solubility is unaffected by ph changes is. A) BaC 2 O 4 B) Ca 3 (PO 4 ) 2 C) Ag 2 CrO 4 D) CuI Page 11

12 63. Mg(OH) 2 is most soluble at ph. A) 7 B) 11 C) 8 D) The molar solubility of Fe(OH) 2 at ph 8.00 is. A) M B) 1.6 M C) 0.16 M D) M 65. Fe(OH) 2 is least soluble at a ph of. A) 10 B) 4 C) 0 D) The solubility product of Mg(OH) 2 is The minimum concentration of NaOH required to decrease the concentration of Mg 2+ in 0.01 M Mg(NO 3 ) 2 to M is. A) M B) M C) 0.35 M D) M 67. If 2.50 g of CuSO 4 are dissolved in ml of 0.30 M NH 3, the concentration of [Cu(NH 3 ) 4 ] 2+ at equilibrium in the solution is. A) M B) M C) M D) M 68. The concentration of Cd 2+ at equilibrium when 0.50 g of Cd(NO 3 ) 2 is dissolved in 500 ml of 0.50 M NaCN is. (The formation constant of Cd(CN) 4 2 is ) A) M B) M C) M D) M Page 12

13 69. Sodium hydroxide is added to M Al 3+ until the ph becomes 14. The predominant species at equilibrium is. (K f for Al(OH) 4 is ). A) Al 3+ B) Al(OH) 4 C) Al(OH) 3 D) Al 2 O The molar solubility of AgI in a 1.0 M NH 3 solution is. A) M B) M C) M D) M 71. AgOH is not soluble in. A) NaOH B) HNO 3 C) NH Which of the following statements is not correct? A) CuI 2 dissolves in NH 3. B) AgBr dissolves in NaCN. C) HgCl 2 dissolves in KCl. D) AgCl dissolves in NaCl. 73. An example of a metal ion in the second group of qualitative analysis is. A) Hg 2 2+ B) Cu 2+ C) Ca 2+ D) Mn Silver chloride can be separated from lead chloride using. A) K 2 CrO 4 B) H 2 S C) NH 3 D) KI Page 13

14 75. The concentration of Pb 2+ in a solution that is 0.15 M in Cl is. A) B) C) D) NH 4 Cl can be distinguished from KCl by the addition of. A) AgNO 3 B) Conc. HCl C) NaOH D) Pb(NO 3 ) AgNO 3 can be distinguished from Cu(NO 3 ) 2 by using. A) HNO 3 B) H 2 S C) HCl D) Br 2 /H 2 O 78. The buffer range is defined as ph= pk a ± 1. The range of conjugate base to acid that corresponds to this equation is. A) B) C) 1 10 D) The pk a of methyl orange is Over what ph range does this indicator change from 90% HIn to 90% In? A) B) C) D) Which one of the following is true for an acid base titration at the half -neutralization point (the point at which half of the acid has been neutralized)? A) ph = poh B) ph = ฝ pk a C) pk a = ฝ ph D) ph = pk a Page 14

15 ml of NaOH was mixed with 400 ml of a 2.00 M HNO 2 solution. The ph of mixed solution was 1.50 units greater than the original acid solution. The molarity of NaOH used was. A) 0.82 M B) 1.28 M C) M D) 2.15 M 82. The pk a of butyric acid is 4.7. The K b of its conjugate base is. A) B) C) D) Exactly 500 ml of M NaOH was mixed with exactly 500 ml of M CH 3 COOH. The equilibrium concentration of CH 3 COO is. A) M B) M C) M D) M ml of 1.00 M Ba(OH) 2 was mixed with 86.4 ml of M H 2 SO 4. The mass of BaSO 4 formed is. A) 2.16 g B) 7.12 g C) 3.42 g D) 9.96 g ml of 1.00M Ba(OH) was mixed with 86.4 ml of M H 2 SO 4. The ph of the resulting solution is. A) 4.56 B) C) 8.72 D) Page 15

16 86. For which of the following reactions is the equilibrium constant called the solubility product? A) B) C) D) 87. Equal volumes of 0.12 M AgNO 3 and 0.14 M ZnCl 2 were mixed. The equilibrium concentration of Cl will be. A) M B) C) M D) The solubility product of silver carbonate, Ag 2 CO 3, is Its solubility in g/l is. A) B) C) D) In a solution that is initially M in Zn 2+, the Zn 2+ can be precipitated at a ph of. A) 2.68 B) 8.11 C) 4.32 D) In a solution that is initially M Fe 3+, Fe(OH) 3 can be precipitated at a ph of. A) 2.16 B) 1.68 C) 2.68 D) 1.01 Page 16

17 ml of M HCl is titrated against M CH 3 NH 2. What will be the solution ph after the addition of 10.0 ml of CH 3 NH 2 solution? A) 1.37 B) 2.73 C) 2.37 D) The molar solubility of Pb(IO 3 ) 2 in 0.10 M NaIO 3 is M. The K sp of Pb(IO 3 ) 2 is. A) B) C) D) Mercury (II) chloride reacts with excess KI to yield. A) Hg 2 I 2 B) HgI 4 2 C) HgI 2 D) HgI 94. The pk a of phenolphthalein is Over what ph range does this indicator change from 95% HIn to 95% In? A) B) C) D) Solid NaI is added to a solution which is 0.010M is Cu + and 0.010M Ag +. The concentration of Ag + when CuI just begins to precipitate is. A) M B) M C) M D) M Page 17

18 ml of HCl as added to g of MCO 3. The excess HCl required 5.64 ml of M NaOH for neutralization. The molar mass of the metal carbonate is g mol 1. A) 137 B) 117 C) 197 D) The equilibrium constant for the reaction between aqueous HCl and aqueous NaOH is. A) B) C) D) The equilibrium constant for the reaction between CH 3 COOH and NaOH is. A) B) C) D) g of a hydrated diprotic acid was dissolved in enough water to make 250ml of solution and 25 ml of the resulting solution required 15.9 ml of M NaOH for neutralization. The number of molecules of water in the hydrate is. (The molecular weight of the anhydrous acid is 90 g/mol.) A) 2 B) 7 C) 5 D) A buffer solution of ph 4.74 can be prepared by mixing CH 3 COOH and CH 3 COONa in the proportion. A) 500 ml of 0.80 M CH 3 COOH ml 0.80 M CH 3 COONa B) 500 ml of 0.80 M CH 3 COOH ml 0.40 M CH 3 COONa C) 500 ml of 0.40 M CH 3 COOH ml 0.80 M CH 3 COONa D) 50 ml of 0.80 M CH 3 COOH + 25 ml of 0.04 M CH 3 COONa Page 18

19 101. The pk a of phenolphthalein is The ratio of non-ionized form to the ionized form of the indicator at ph 8.00 is. A) 1.26 B) 17.1 C) 1.1 D) Oil paintings containing lead compounds become dark due to the formation of. A) PbSO 4 B) PbS C) PbCl 2 D) PbO 103. Sodium ions can be separated from Ba 2+ ions by the addition of. A) HCl B) HNO 3 C) CH 3 COOH D) H 2 SO Zn 2+ ions can be separated from Hg 2+ ions by using. A) NaCl B) KI C) HCl D) H 2 S 105. The concentration of Sr 2+ is a solution saturated with both BaSO 4 and SrSO 4 is. A) M B) M C) M D) M 106. The substance having the greatest solubility among the following is. A) CaSO 4 (K sp = ) B) BaSO 4 C) Ag 2 SO 4 D) AgI Page 19

20 107. How many ml of 1.0 M NaOH must be added to 200 ml of 0.10 M NaH 2 PO 4 to obtain a buffer solution of ph 7.50? A) 23 ml B) 30 ml C) 43 ml D) 13 ml 108. Which of the following has the highest [H + ]? A) 0.10 M H F B) 0.10 M H F in 0.10 M NaF C) 0.10 M H F in 0.10 M SbF 5 (SbF 5 reacts with F - to form SbF 6 - ) D) 0.01 M H F 109. A distribution curve shows how the fractions of nonionized acid and its conjugate base vary as a function of ph. At the point of intersection of the distribution curves of [CH 3 COOH] and [CH 3 COO ]: A) ph = poh B) ph = pk a C) ph + poh = pk a D) ph = pk a + pk b 110. A distribution curve shows how the fractions of nonionized acid and its conjugate base vary as a function of ph. The curves of the plot of [CH 3 COOH] vs. ph and [CH 3 COO ] vs. ph will intersect at a ph of. A) 7.47 B) 2.83 C) 3.85 D) The addition of washing soda (Na 2 CO 3 ท10H 2 O) removes ions present in hard water. A) Mg 2+ B) SO 4 2 C) Ca 2+ D) Cl Page 20

21 112. Most of the acid base indicators change their color at ph equal to. A) pk a B) pk b C) pk a + pk b D) pk a ± 1 Page 21

22 Answer Key 1. B 2. C 3. A 4. D 5. B 6. C 7. A 8. B 9. A 10. B 11. C 12. A 13. D 14. B 15. A 16. D 17. B 18. B 19. D 20. B 21. C 22. A 23. B 24. D 25. D 26. B 27. B 28. D 29. C 30. D 31. A 32. D 33. B 34. B 35. D 36. B 37. D 38. C 39. B 40. D 41. B 42. C 43. A 44. C Page 22

23 45. A 46. B 47. C 48. B 49. D 50. A 51. A 52. A 53. B 54. B 55. C 56. B 57. C 58. A 59. A 60. B 61. A 62. D 63. A 64. A 65. A 66. C 67. B 68. C 69. B 70. D 71. A 72. D 73. B 74. C 75. B 76. C 77. C 78. D 79. A 80. D 81. B 82. D 83. B 84. D 85. B 86. D 87. C 88. A 89. B 90. C Page 23

24 91. A 92. C 93. B 94. C 95. A 96. C 97. C 98. B 99. A 100. A 101. D 102. B 103. D 104. B 105. D 106. C 107. D 108. C 109. B 110. D 111. C 112. D Page 24

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