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1) Identify a good buffer.
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2) Which of the following solutions is a good buffer system?
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Chemistry Ch.16

QuestionAnswer
1) Identify a good buffer. E) significant amounts of both a weak acid and its conjugate base
2) Which of the following solutions is a good buffer system? A) A solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2
3) Which of the following solutions is a good buffer system? B) A solution that is 0.10 M HCN and 0.10 M LiCN
4) Which one of the following statements is TRUE? C) A buffer resists pH change by neutralizing added acids and bases.
5) If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE? D) [HCHO2] > [NaCHO2]
6) If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89, which of the following is TRUE? A) [HCHO2] < [NaCHO2]
7) If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74, which of the following is TRUE? B) [HCHO2] = [NaCHO2]
10) A buffer solution is 0.100 M in both HC7H5O2 and LiC7H5O2 and has a pH of 4.19. Which of the following pH values would you expect from the addition of a small amount of a dilute solution of a strong base? D) 4.49
28) Which of the following is TRUE? B) A buffer is most resistant to pH change when [acid] = [conjugate base]
29) Define buffer capacity. A) Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness.
30) The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid? C) 10
31) Which of the following acids (listed with pKa values) and their conjugate base would form a buffer with a pH of 8.10? C) HClO, pKa = 7.54
32) Which of the following acids (listed with Ka values) and their conjugate base would form a buffer with a pH of 2.34? E) HClO2, Ka = 1.1 x 10-2
33) A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer? C) adding 0.050 moles of HCl
34) A 1.0 L buffer solution is 0.050 M HC2H3O2 and 0.250 M LiC2H3O2. Which of the following actions will destroy the buffer? A) adding 0.050 moles of NaOH
35) Identify the pH of normal blood. C) 7.4
65) Which of the following compounds will have the highest molar solubility in pure water? B) MgCO3, Ksp = 6.82 × 10-6
66) Which of the following compounds will be more soluble in acidic solution than in pure water? B) FeS
67) Identify the salts that are in hard water. A) CaCO3 and MgCO3
68) Which of the following compounds solubility will not be affected by a low pH in solution? A) AgCl
79) Which of the following compounds will have the highest molar solubility in pure water? C) Al(OH)3, Ksp = 3 × 10-34
The Ka of hydrazoic acid is 1.9 × 10-5. D) hydrazoic acid
The Ka of chloroacetic acid is 1.36 × 10-3. C) chloroacetate ion
In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C? C) 0.1 M CaBr2
What is the molar solubility of AgCl in 0. 30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1.7 × 107. B) 1.6 × 10- 2 M
41) What is the molar solubility of AgCl in 0. 10 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021. A) 0. 050 M
36) Which of the following is TRUE? A) The equivalence point is where the amount of acid equals the amount of base during any acid-base titration.
37) When titrating a strong monoprotic acid and KOH at 25°C, the D) pH will be equal to 7 at the equivalence point.
38) When titrating a weak monoprotic acid with NaOH at 25°C, the C) pH will be greater than 7 at the equivalence point.
39) When titrating a monoprotic strong acid with a weak base at 25°C, the E) pH will be less than 7 at the equivalence point.
40) Identify the most common indicator. D) phenolphthalein
41) Identify the indicator that can be used at the lowest pH. C) crystal violet
42) Identify the indicator that has two endpoints. B) thymol blue
43) Identify the indicator that can be used at the highest pH. E) alizarin yellow R
86) Give the equation for an unsaturated solution in comparing Q with Ksp. B) Q < Ksp
87) Give the equation for a saturated solution in comparing Q with Ksp. C) Q = Ksp
88) Give the equation for a supersaturated solution in comparing Q with Ksp. A) Q > Ksp
89) A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10-10. C) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution.
90) A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9. D) Nothing will happen since Ksp > Q for all possible precipitants.
91) A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9. D) A precipitate will form since Q > Ksp for calcium oxalate.
94) Identify the compound that is acid-insoluble. B) As2S
95) Identify the compound that is base-insoluble. C) CoS
96) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl. C) AgCl
97) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl, then H2S and 0.2 M HCl. B) CdS
98) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; and OH- to a pH of 8. E) ZnS
99) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. A) Ba3(PO4)2
100) A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the soluble ions D) NH4Cl
101) A ligand is a molecule or ion that acts as a D) Lewis base
102) Describe the solubility of Al(OH)3 with respect to pH. A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
103) Gives what happens at low pH for aluminum hydroxide. A) Al(H2O)63+ dissolves
104) Gives what happens at neutral pH for aluminum hydroxide. C) Al(OH)3 precipitates
105) Gives what happens at high pH for aluminum hydroxide. B) Al(H2O)2(OH)4- dissolves
106) A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the Kf for Cu(CN)42- is 1.0 × 1025, how much copper ion remains at equilibrium? B) 1.9 x 10-26 M
107) A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF. If the Kf for AlF63- is 7 × 1019, how much aluminum ion remains at equilibrium? C) 9.1 × 10-19 M
37) In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C? C) 0.1 M CaBr2
A) 3/4 of the way to second equivalence point of a diprotic acid/strong base titration 5) pH = pKa2
B) equivalence point of a strong acid/strong base titration 1)pH = 7
C) half-way to equivalence point of a weak acid/strong base titration 2) pH = pKa
D) equivalence point of a weak base/strong acid titration 4)pH < 7
E) equivalence point of a weak acid/strong base titration 3)pH > 7
40) What is the molar solubility of AgCl in 0. 30 M NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3)2+ is 1. B) 1.6 × 10- 2 M7 × 107.
41) What is the molar solubility of AgCl in 0. 10 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021. A) 0. 050 M
42) 0.10 M potassium chromate is slowly added to a solution containing 0. 50 M AgNO3 and 0. 50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively. D) 6.8 × 10-2 M
43) A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds __________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6. B) 1.1 × 10-2
Created by: isha2326
 

 



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