1022_2nd Exam_1030416
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which of the following species is amphoteric?
A) CO32- B) HPO42- C)NH4 D) HF
E) None of the above are amphoteric.
Answer: B
2)What is the conjugate base of H2PO4 ?
A)H3PO4 B) PO43- C) HPO42- D) OH E) H3O+
Answer: C
3) Identify the weak diprotic acid.
A)HClO4 B)HNO3 C)H3PO4 D)H2SO3 E)H2SO4
Answer: D
4) Which of the following statements is TRUE?
A) The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid.
B) A weak base is composed of a cation and an anion with a very weak attraction between them.
C) A strong acid is composed of a proton and an anion that have a very strong attraction for one another.
D) A strong acid has a strong conjugate base.
E) None of the above statements are true.
Answer: A
5)Determine the pH of a 0.00598 M HClO4 solution.
A) 11.777 B) 6.434 C) 3.558 D) 2.223 E) 7.566
Answer: D
6) Calculate the pOH of a solution that contains 7.8 x 10-6 M OH at 25°C.
A) 5.11 B) 9.64 C) 12.72 D) 8.89 E) 1.28
Answer: A
7) Acid rain consists primarily of ________.
A) benzoic acid
B) nitric and sulfuric acids C) nitric acid
D) sulfuric acid E) acetic acid Answer: B
8) Determine the pH of a 0.62 M NH4NO3 solution at 25°C. The Kb for NH3 is 1.76 × 10-5.
A) 9.45 B) 4.73 C) 9.27 D) 11.52 E) 2.48
Answer: B
9)Place the following in order of increasing acid strength.
HBrO2 HBrO3 HBrO HBrO4
A)HBrO2 < HBrO4 < HBrO < HBrO3 B) HBrO < HBrO4 < HBrO3 < HBrO2 C)HBrO2 < HBrO3 < HBrO4 < HBrO D)HBrO4 < HBrO2 < HBrO3 < HBrO E)HBrO < HBrO2 < HBrO3 < HBrO4 Answer: E
10)What is the Kw of pure water at 50.0°C, if the pH is 6.630?
A) 2.13 × 10-14 B) 2.34 × 10-7 C) 1.00 × 10-14 D) 5.50 × 10-14
E)There is not enough information to calculate the Kw.
Answer: D
11)Which of the following bases is the STRONGEST? The base is followed by its Kb.
A) C5H5N, 1.7 × 10-9 B) CH3NH2, 4.4 × 10-4 C) (CH3CH2)2NH, 8.6 × 10-4 D) NH3, 1.76 × 10-5
E) C6H5NH2, 4.0 × 10-10 Answer: C
12) Which one of the following will form a basic solution in water?
A) LiBrO B)NaC2H3O2 C) LiCN D)KClO2
E) All of the above will form basic solutions.
Answer: B, C
13) Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 x 10-2) and 0.15 M HClO (Ka = 2.9 × 10-8).
A) 12.55 B) 4.18 C) 1.39 D) 3.55 E) 9.82
Answer: C
14)Determine the [OH ] concentration in a 0.169 M Ca(OH)2 solution.
A) 0.338 M B) 0.298 M C) 0.169 M D) 5.92 × 10-14 M
E) 2.96 × 10-14 M
15)Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.
A) 2.7 B) 5.4 × 10-3 C) 4.9 × 10-7 D) 8.5 × 10-6 E) 1.2 × 10-5
Answer: D
16) Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 × 10-4.
A) 3.5 × 10-2 % B) 1.2 × 10-2 % C) 1.1 % D) 4.7 % E) 3.2 %
Answer: E
17) Identify a good buffer.
A) significant amounts of both a strong acid and a strong base B) significant amounts of both a weak acid and a strong acid C) small amounts of both a strong acid and a strong base D) small amounts of both a weak acid and its conjugate base
E) significant amounts of both a weak acid and its conjugate base Answer: E
18)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?
A)[HCHO2] << [NaCHO2]
B)[HCHO2] > [NaCHO2]
C)[HCHO2] = [NaCHO2]
D)[HCHO2] < [NaCHO2]
E)It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.
Answer: B
19) 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?
A) 2.9 × 10-27 M B) 3.8 × 10-24 M C) 6.7 × 10-28 M D) 4.6 × 10-25 M E) 1.9 x 10-26 M Answer: E
20) 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.
A)A precipitate will form since Q > Ksp for calcium oxalate.
B) A precipitate will form as calcium oxalate is not soluble to any extent.
C)Nothing will happen Ksp > Q for all possible precipitants.
D) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds.
E) There is not enough information to determine.
Answer: A
21) The molar solubility of Ag2S is 1.26 × 10-16 M in pure water. Calculate the Ksp for Ag2S.
A) 1.12 × 10-8 B) 3.78 × 10-12 C) 8.00 × 10-48 D) 1.59 × 10-32 E) 6.81 × 10-63 Answer: C
22) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8 × 10-5.
A) 9.26 B) 11.13 C) 4.74 D) 12.55 E) 13.00
Answer: B
23) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 100.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.
A) 10.56 B) 5.28 C) 8.72 D) 3.44 E) 6.58
Answer: B
24) Determine the molar solubility of AgBr in a solution containing 0.200 M NaBr. Ksp (AgBr) = 7.7 × 10-13.
A) 3.8 × 10-12 M B) 1.54 × 10-13 M C) 0.200 M D) 8.8 × 10-7 M
E) 5.8 × 10-5 M Answer: A
25) 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.
B) At the equivalence point, the pH is always 7.
C) A titration curve is a plot of pH vs. the [base]/[acid] ratio.
D) An indicator is not pH sensitive.
E) None of the above are true.
Answer: A
26) Determine the molar solubility of BaF2 in pure water. Ksp for BaF2 = 2.45 × 10-5.
A) 6.13 × 10-6 M B) 1.83 × 10-2 M C) 1.23 × 10-5 M D) 4.95 × 10-3 M E) 2.90 × 10-2 M Answer: B
27) When titrating a monoprotic strong acid with a weak base at 25°C, the A) pH will be greater than 7 at the equivalence point.
B) pH will be less than 7 at the equivalence point.
C) titration will require more moles of the base than acid to reach the equivalence point.
D) pH will be 7 at the equivalence point.
E) titration will require more moles of acid than base to reach the equivalence point.
Answer: B
28)Give the equation for a supersaturated solution in comparing Q with Ksp.
A)Q < Ksp B) Q Ksp C)Q = Ksp D)Q > Ksp
E) none of the above Answer: D
29)Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 300.0 mL of 0.20 M KClO. The Ka for HClO is 2.9 × 10-8.
A) 6.46 B) 8.01 C) 5.99 D) 7.54 E) 7.06
Answer: D
30) A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.
A) 3.57 B) 3.63 C) 3.46 D) 2.89 E) 3.34
Answer: A
31) Define buffer capacity.
A) Buffer capacity is the amount of acid that can be added until all of the base is used up.
B) Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness.
C) Buffer capacity is the amount of base that can be added until all of the acid is used up.
D) Buffer capacity is the amount of base that can be added until all of the base is used up.
E) Buffer capacity is the amount of acid that can be added until all of the acid is used up.
Answer: B
32) Choose the electron configuration for Fe3+.
A) [Ar]3d5 B) [Ar]4s23d3 C) [Ar]4s23d9 D) [Ar]4s23d6 E) [Ar]4s13d4
Answer: A
33)Name the following: Fe[AlF6]
A) iron (III) hexafluoroaluminate B) ironaluminumhexafluoride C) aluminumhexafluoroferrate D) iron(II) hexafluoroaluminum
E) iron(I) aluminumhexafluoride Answer: A
34) Determine the chemical formula for the compound, diamminetetraaquairon(II)chloride.
A)[Fe(NH3)2][(H2O)4Cl]
B)[Fe(NH3)2(H2O)4]Cl2 C)[Fe(NH3)2(H2O)4]Cl3 D)[Fe(NH3)2(H2O)4Cl]
E)[Fe(H2O)4][(NH3)2Cl]
Answer: B
35) Identify the isomers that have ligands which coordinates to metal in different ways.
A) geometric isomers B) coordination isomers.
C) optical isomers D) linkage isomers
E) stereoisomers.
Answer: D
36) How many unpaired electrons would you expect for the complex ion: [Cr(CN)6]4-?
A) 5 B) 3 C) 2 D) 1 E) 0
Answer: C
37)Name the following: [Pt(H2O)4F2]Br2 A) tetraaquadifluoroplatinum(IV) bromide
B) platinum(III)tetraaquadifluorobromide C) tetraaquadibromodifluoroplatinate D) platinum (II) dibromodifluorotetrahydride
E) platinum(II)bromide Answer: A
38) Which of the following compounds can exhibit fac-mer isomerism?
A) [Fe(NH3)4(H2O)2]2+
B) [Fe(CO)3(NH3)3]3+
C) [Cu(CO)5Br]+
D) [Fe(CO)5ONO]2+
E) [Cr(H2O)4Br2]+
Answer: B
39) The complex ion, [Ni(NH3)6]2+, has a maximum absorption near 580 nm. Calculate the crystal field splitting energy (in kJ/mol) for this ion.
A) 485 kJ/mol B) 114 kJ/mol C) 343 kJ/mol D) 206 kJ/mol E) 292 kJ/mol Answer: D
40) Which of the following pairs of coordination compounds or complex ions are examples of coordination isomers?
A)[Fe(NH3)2(H2O)4]Cl2 and [Fe(NH3)4(H2O)2]Cl2 B) [MnCl3Br]2- and [MnClBr3]2-
C)[Cu(CO)5Br]Cl and [Cu(CO)5Cl]Br
D)[Fe(NH3)2(H2O)4]Cl2 and [Fe(NH3)2(H2O)4]Br2 E) [Fe(CO)5NO2]2+ and [Fe(CO)5ONO]2+
Answer: C
