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Q:
Which picture represents the system halfway between the first and second equivalence points?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which picture represents the system at the first equivalence point?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
The following pictures represent solutions at various stages in the titration of a weak diprotic acid H2A with aqueous KOH. Unshaded spheres represent H atoms, black spheres represent oxygen atoms, and shaded spheres represent A2- ions. (K+, H3O+ initially present, OH- initially present and solvent water molecules have been omitted for clarity).Which picture represents the system halfway to the first equivalence point?A) (1)B) (2)C) (3)D) (4)
Q:
Which picture represents the solution after the equivalence point?A) (1)B) (2)C) (3)D) (4)
Q:
Which picture represents the solution at the equivalence point?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which picture represents the solution before the equivalence point?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH. Unshaded spheres represent H atoms, black spheres represent oxygen atoms, and shaded spheres represent A- ions. (K+, H3O+ initially present, OH- initially present and solvent water molecules have been omitted for clarity).Which picture represents the solution before the addition of any KOH?A) (1)B) (2)C) (3)D) (4)
Q:
Which picture represents the equilibrium state of the solution after addition of one OH- ion to the solution shown in picture (1)?A) (2)B) (3)C) (4)D) (5)
Q:
The following pictures represent solutions that contain a weak acid HA (pKa = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms, black spheres represent oxygen atoms, and shaded spheres represent A- ions. (K+, H3O+ initially present, OH- initially present and solvent water molecules have been omitted for clarity.)Which picture represents the equilibrium state of the solution after addition of one H3O+ ion to the solution shown in picture (1)?A) (2)B) (3)C) (4)D) (5)
Q:
For which of these solutions is pH = pKa?A) All have pH = pKa.B) (1), (2) and (3)C) (1) and (4)D) (2) and (3)
Q:
Which solution has the greatest buffer capacity?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which of these solutions are buffers?
A) (1) and (2)
B) (1) and (3)
C) (1), (2) and (3)
D) All are buffer solutions.
Q:
Which solution has the largest percent dissociation of HA?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which solution has the lowest pH?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
The following pictures represent solutions that contain a weak acid HA (pKa = 5.0) and its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A- ions. (K+, H3O+, OH-, and solvent H2O molecules have been omitted for clarity.)Which solution has the highest pH?A) (1)B) (2)C) (3)D) (4)
Q:
For which solution(s) is pH = pKa?A) only solution (1)B) only solution (2)C) only solution (3)D) solutions (1) and (3)
Q:
Which solution has the greatest buffer capacity?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which of the solutions are buffer solutions?
A) (1) and (2)
B) (1) and (3)
C) (2) and (3)
D) (2) and (4)
Q:
Which solution has the largest percent dissociation of HA?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
Which solution has the lowest pH?
A) (1)
B) (2)
C) (3)
D) (4)
Q:
The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA. Unshaded spheres represent H atoms and shaded spheres represent A- ions. (K+, H3O+, OH-, and solvent H2O molecules have been omitted for clarity.)Which solution has the highest pH?A) (1)B) (2)C) (3)D) (4)
Q:
Which pair of ions can be separated by the addition of sulfide ion?A) Ag+ and Mn2+B) Cu2+ and Bi3+C) Pb2+ and Ca2+D) Ca2+ and Ba2+
Q:
Which pair of ions can be separated by the addition of chloride ion?
A) Ag+ and Co2+
B) Cu2+ and Bi3+
C) Pb2+ and Hg22+
D) Ca2+ and Ba2+
Q:
Which set of ions precipitate as sulfides?
A) , Pb2+, Sn2+
B) Pb2+, Fe2+, Ca2+
C) Co2+, Ba2+, K+
D) NH4+, Na+, K+
Q:
A solution may contain the following ions Ag+, Cu2+, Mn2+, Ca2+, and Na+. No precipitate formed when 0.10 M HCl was added but a dark colored precipitate formed when H2S was added to an acidic portion of the solution. After the removal of the solid the solution was made basic and more H2S was added and a dark precipitate again formed. Treatment of the filtrate with (NH4)2CO3 resulted in a white precipitate. If no further tests were made then what conclusions can you draw?
A) possible ions present Cu2+, Mn2+, Na+
B) possible ions present Cu2+, Mn2+, Ca2+
C) possible ions present Cu2+, Mn2+, Ca2+, Na+
D) possible ions present Ag+, Cu2+, Mn2+, Ca2+, Na+
Q:
A solution may contain the following ions Ag+, Cu2+, Cd2+, Mn2+, Ni2+ and Na+. A white precipitate formed when 0.10 M HCl was added and after this was removed the solution was treated with H2S gas under acidic conditions and no precipitate formed. When the solution was made basic and again treated with H2S gas a dark colored precipitate formed. If no further tests were made then what conclusions can you draw?
A) possible ions present Ag+, Mn2+, Ni2+
B) possible ions present Ag+, Mn2+, Ni2+, Na+
C) possible ions present Ag+, Cu2+, Cd2+
D) possible ions present Ag+, Cu2+, Cd2+, Na+
Q:
Which metal ions can be precipitated out of solution as chlorides?
A) Ag+, Hg2+, Co2+
B) Cu2+, Cd2+, Bi3+
C) Ag+, Hg22+, Pb2+
D) Na+, K+, Mg2+
Q:
Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+, Zn2+, Pb2+ and Cu2+ and 0.10 M in H2S at a pH of 0.50? A) MnS
B) CuS
C) PbS, CuS
D) ZnS, PbS, CuS
Q:
Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+, Zn2+, Pb2+ and Cu2+ and 0.10 M in H2S at a pH of 1.0? A) MnS
B) CuS
C) PbS, CuS
D) ZnS, PbS, CuS
Q:
0.10 M potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? Ksp for Ag2CrO4 and BaCrO4 are 1.1 10-12 and 1.2 10-10, respectively.
A) 6.5 10-5 M
B) 1.3 10-4 M
C) 3.2 10-4 M
D) 4.3 10-2 M
Q:
Potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2. Describe what happens if the Ksp for Ag2CrO4 is and the Ksp of BaCrO4 is A) The BaCrO4 precipitates first out of solution.
B) The Ag2CrO4 precipitates first out of solution and then BaCrO4 precipitates.
C) Both BaCrO4 and Ag2CrO4 precipitate simultaneously out of solution.
D) Neither BaCrO4 nor Ag2CrO4 precipitates out of solution.
Q:
Precipitation of an ionic compound will occur upon mixing of desired reagents if the initial ion product is
A) greater than the Ksp.
B) equal to the pKsp.
C) equal to the Ksp.
D) less than the Ksp.
Q:
Which of the following reactions are not consistent with the concept of acid base amphoterism?A) Al(OH)3(s) + OH-(aq) -> Al(OH)4-(aq)B) Al(OH)3(s) + 3 H3O+(aq) -> Al3+(aq) + 6 H2O(l)C) H2O(l) + H2O(l) H3O+(aq) + OH-(aq)D) Al(OH)3(s) Al3+(aq) + 3 OH-(aq)
Q:
Which of the following metal hydroxides are amphoteric?
A) Al(OH)3, Zn(OH)2, Cr(OH)3, Sn(OH)2
B) Cu(OH)2 , Mn(OH)2, Fe(OH)2, Fe(OH)3
C) Be(OH)2, Ca(OH)2, Ba(OH)2, Sr(OH)3
D) LiOH, NaOH, KOH, RbOH
Q:
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 A) 0.050 M
B) 0.10 M
C) 0.20 M
D) 0.40 M
Q:
What is the molar solubility of AgCl in 1.0 M K2S2O3 if the complex ion Ag(S2O3)23- forms? The Ksp for AgCl is 1.8 and the Kf for Ag(S2O3)23- is A) 0.50 M
B) 1.0 M
C) 1.5 M
D) 2.0 M
Q:
What is the molar solubility of AgCl in 0.10 M NH3? Ksp for AgCl is 1.8 10-10 and the Kf for Ag(NH3)2+ is A) 1.3 10-5 M
B) 5.0 10-3 M
C) 5.5 10-3 M
D) 5.5 10-2 M
Q:
In which of the following solutions would solid PbCl2 be expected to be the least soluble at 25C?
A) 0.1 M HCl
B) 0.1 M NaCl
C) 0.1 M CaCl2
D) 0.1 M KNO3
Q:
What is the molar solubility of lead(II) chromate in 0.10 M HNO3 if the Ksp for PbCrO4 is 2.8 and the Ka2 for H2CrO4 is Note that H2CrO4 is considered to be a strong acid.
A) 9.2 10-11 M
B) 2.9 10-10 M
C) 9.3 10-7 M
D) 3.1 10-4 M
Q:
Calculate the molar solubility of thallium(I) chloride in 0.30 M NaCl at 25C. Ksp for TlCl is A) 5.1 10-5 M
B) 5.7 10-4 M
C) 7.1 10-3 M
D) 1.3 10-2 M
Q:
What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is A) 5.6 10-10 M
B) 5.6 10-8 M
C) 2.4 10-6 M
D) 1.1 10-4 M
Q:
What is the molar solubility of CaF2 in 0.10 M NaF solution at 25C? The Ksp for CaF2 is A) 8.5 10-10 M
B) 3.4 10-10 M
C) 3.4 10-9 M
D) 2.0 10-4 M
Q:
Calculate the solubility (in g/L) of silver carbonate in water at 25C if the Ksp for Ag2CO3 is 8.4 10-12.
A) 8.0 10-4 g/L
B) 3.5 10-2 g/L
C) 4.4 10-2 g/L
D) 5.6 10-2 g/L
Q:
Calculate the Ksp for silver sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L.
A) 3.0 10-6
B) 1.2 10-5
C) 2.1 10-4
D) 4.2 10-4
Q:
One liter of a saturated solution of Ca contains 0.0167 g of dissolved Ca. What is the for Ca?
A) 3.9 B) 9.6 C) 2.8 D) 3.7
Q:
One liter of a saturated solution of Mg contains 0.0726 g of dissolved Mg. What is the for Mg?
A) 6.3 B) 1.6 C) 3.2 D) 6.4
Q:
One liter of a saturated solution of Ba contains 1.32 g of dissolved Ba. What is the for Ba?
A) 1.7 B) 4.4 C) 5.7 D) 8.8
Q:
What is the most soluble salt of the following set?
A) AgCN with Ksp = 6.0 10-17
B) Al(OH)3 with Ksp = 1.9 10-33
C) Fe(OH)3 with Ksp = 2.6 10-39
D) Sn(OH)2 with Ksp = 1.6 10-19
Q:
What is the most soluble salt of the following set?
A) Ba(OH)2 with Ksp = 5.0 10-3
B) Ca(OH)2 with Ksp = 4.7 10-6
C) Cd(OH)2 with Ksp = 5.3 10-15
D) Fe(OH)2 with Ksp = 2.5 10-37
Q:
What is the chromium ion concentration for a saturated solution of Cr(OH)3 if the Ksp for Cr(OH)3 is A) 8.19 10-16 M
B) 1.26 10-8 M
C) 2.17 10-8 M
D) 3.76 10-8 M
Q:
What is the silver ion concentration for a saturated solution of Ag2CO3 if the Ksp for Ag2CO3 is A) 2.90 10-6 M
B) 2.03 10-4 M
C) 2.56 10-4 M
D) 4.06 10-4 M
Q:
What is the equilibrium constant expression for the Ksp of Ca3(PO4)2?
A) Ksp = [Ca2+]3[PO43-]2
B) Ksp = {[Ca2+]3[PO43-]2}/[Ca3PO4]
C) Ksp = {[Ca2+]3[PO43-]2}/{[Ca3PO4][H2O]}
D) Ksp = 1/{[Ca2+]3[PO43-]2}
Q:
The balanced equation for the solubility equilibrium of Fe(OH)2 is shown below. What is the equilibrium constant expression for the Ksp of Fe(OH)2? A) Ksp = {[Fe2+][OH-]2}/{[Fe(OH)2][H2O]}
B) Ksp = {[Fe2+][OH-]2}/[Fe(OH)2]
C) Ksp = [Fe2+][OH-]2
D) Ksp = 1/{[Fe2+][OH-]2}
Q:
The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H2X+) are and What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?
A) 9.70
B) 10.69
C) 11.85
D) 12.70
Q:
The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid, H2X+) are and What is the pH of 50.00 mL of a solution of alanine after 37.50 mL of 0.100 M NaOH has been added?
A) 4.85
B) 6.02
C) 7.39
D) 9.70
Q:
The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid, H2X+) are and What is the pH of 50.00 mL of a 0.0500 M solution of alanine after 25.00 mL of NaOH has been added?
A) 2.34
B) 4.85
C) 6.02
D) 6.72
Q:
Oxalic acid, H2C2O4 has acid dissociation constants Ka1 = 5.9 10-2 and Ka2 = 6.4 10-5. What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H2C2O4?A) 1.23B) 2.10C) 2.70D) 4.19
Q:
Sulfurous acid, H2SO3 has acid dissociation constants Ka1 = 1.5 10"2 and Ka2 = 6.3 10"8. What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H2SO3?
A) 1.82
B) 3.60
C) 4.51
D) 7.20
Q:
What is the pH of the resulting solution if 25 mL of 0.432 M methylamine, CH3NH2, is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 10-11 for CH3NH3+.
A) 3.11
B) 3.74
C) 10.26
D) 10.89
Q:
Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 28.30 mL of 0.500 M HCl to reach the equivalence point?
A) 0.208 M
B) 0.353 M
C) 0.708 M
D) 1.21 M
Q:
Which of the following titrations result in an acidic solution at the equivalence point?
A) CH3COOH titrated with NaOH
B) KF titrated with KOH
C) HCl titrated with NaOH
D) C5H5N titrated with HCl
Q:
What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 10-5 for CH3CO2H.
A) 8.26
B) 9.26
C) 11.13
D) 12.15
Q:
What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 30.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 10-5 for CH3CO2H.
A) 5.28
B) 7.00
C) 8.72
D) 10.02
Q:
What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive. Ka = 1.8 10-5 for CH3CO2H.
A) 9.56
B) 8.95
C) 5.05
D) 4.44
Q:
Formic acid (HCO2H, Ka = 1.8 10-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?
A) 0.0134 M
B) 0.0476 M
C) 0.0567 M
D) 0.0676 M
Q:
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? Ka = 6.76 10-4 for HF.
A) 1.74
B) 5.75
C) 8.25
D) 12.26
Q:
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka = 1.8 10-4 for formic acid.
A) 2.46
B) 5.88
C) 8.12
D) 11.54
Q:
What is the pH at the equivalence point of a weak acid-strong base titration?
A) pH < 7
B) pH = 7
C) pH > 7
D) pH = 14.00
Q:
Which of the following titrations result in a basic solution at the equivalence point?
A) HI titrated with NaCH3CO2
B) HOCl titrated with NaOH
C) HBr titrated with KOH
D) Pb(NO3)2 titrated with NaI
Q:
What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.
A) 0.85
B) 1.85
C) 12.15
D) 13.15
Q:
What volume of 5.00 10-3 M HNO3 is needed to titrate 100.00 mL of 5.00 10-3 M Ca(OH)2 to the equivalence point?A) 12.5 mLB) 50.0 mLC) 100. mLD) 200. mL
Q:
At what pH is the amino acid glycine with a Ka of 2.51 10-10 sixty-six (66%) percent dissociated?
A) 9.60
B) 9.89
C) 10.10
D) 10.60
Q:
What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pKa = 4.10?
A) 96%
B) 10%
C) 5%
D) 1%
Q:
What is the percent dissociation of acetic acid if the solution has a pH = 4.74 and a pKa = 4.74?
A) 100%
B) 50%
C) 10%
D) 1%
Q:
What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pKa = 9.60?
A) 50%
B) 9%
C) 5%
D) 1%
Q:
Which is the best acid to use in the preparation of a buffer with pH = 9.3?A) CH3NH2 (Kb = 3.7 10-4)B) NH3 (Kb = 1.8 10-5)C) NH2OH (Kb = 9.1 10-9)D) C6H5NH2 (Kb = 4.3 10-10)
Q:
Which is the best acid to use in the preparation of a buffer with pH = 3.3?A) HOI (Ka = 2.0 10-11)B) HNO2 (Ka = 4.5 10-4)C) HNO3D) HIO3 (Ka = 1.7 10-1)
Q:
What is not a correct expression for the weak acid HA?
A) Ka = [H3O+][A-]/[HA]
B) pKa = pH - log{[A-]/[HA]}
C) pKa = logKa
D) pKa = 14 - pKb
Q:
What is the Henderson-Hasselbalch equation for the acidic buffer HA/A-?
A) pH = -log[H3O+]
B) pH = 14 - pOH
C) pH = pKa + log{[A-]/[HA]}
D) pH = pKa - log{[A-]/[HA]}
Q:
What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H2PO4- and 0.100 M HPO42- and the A) 5.21
B) 5.61
C) 6.73
D) 7.69