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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 theKa2 = 6.2 10-8?
A) 5.21
B) 5.61
C) 6.73
D) 7.69
Q:
What is the magnitude of the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH3CO2H and 0.100 M NaCH3CO2? The Ka for acetic acid is1.8 10-5.
A) 0.00
B) 0.20
C) 0.47
D) 1.30
Q:
What volume of 0.100 M NaOH is needed to make 100.0 mL of a buffer solution with a pH of 6.00 if one starts with 50.0 mL of 0.100 M potassium hydrogen phthalate? The Ka2 for potassium hydrogen phthalate is 3.1 10-6.
A) 22.4 mL
B) 27.6 mL
C) 30.2 mL
D) 37.8 mL
Q:
What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The Ka2 for hydrogen phthalate is 3.1 10-6.
A) 3.25
B) 5.08
C) 5.51
D) 5.94
Q:
What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 10-5 for CH3CO2H.
A) 0.50:1
B) 0.94:1
C) 1.1:1
D) 2.0:1
Q:
A buffer solution is prepared by dissolving 27.22 g of KH2PO4 and 3.37 g of KOH in enough water to make 0.100 L of solution. What is the pH of the H2PO4-/HPO42- buffer if the Ka2 = 6.2 10-8?
A) 6.84
B) 7.00
C) 7.21
D) 7.84
Q:
What is the pH of 1 L of 0.30 M TRIS, 0.60 M TRISH+ buffer to which one has added 5.0 mL of 12 M HCl? The Kb for the TRIS/TRISH+ is 1.2 10-6.
A) 5.92
B) 6.36
C) 7.36
D) 7.64
Q:
A buffer solution is prepared by dissolving 0.200 mol of NaH2PO4 and 0.100 mol of NaOH in enough water to make 1.00 L of solution. What is the pH of the H2PO4-/HPO42- buffer if the
Ka2 = 6.2 10-8?
A) 6.91
B) 7.21
C) 7.51
D) 7.71
Q:
TRIS {(HOCH2)3CNH2} is one of the most common buffers used in biochemistry. A solution is prepared by adding enough TRIS and 12 M HCl(aq) to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH+] = 0.60 M. What is the pH of this buffered system if the pKb is 5.92?
A) 5.92
B) 6.22
C) 7.78
D) 8.08
Q:
What is the pH of a buffer system made by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12.0 M NH3 in enough water to make 1.000 L of solution? Kb = 1.8 10-5 for NH3.
A) 9.18
B) 9.26
C) 9.34
D) 11.03
Q:
What is the pH of a buffered system made by dissolving 17.42 g of KH2PO4 and 20.41 g of K2HPO4 in water to give a volume of 200.0 mL? The Ka2 for dihydrogen phosphate is 6.2 10-8 and the equilibrium reaction of interest isH2PO4-(aq) + H2O(l) H3O+(aq) + HPO4-(aq).A) 7.03B) 7.17C) 7.38D) 7.58
Q:
Which statement about buffers is true?
A) Buffers have a pH = 7.
B) Buffers consist of a strong acid and its conjugate base.
C) A buffer does not change pH on addition of a strong acid or strong base.
D) Buffers resist change in pH upon addition of small amounts of strong acid or strong base.
Q:
Which of the following combinations of chemicals could be used to make a buffer solution?
A) HCl/NaOH
B) HCl/NH3
C) HCl/H3PO4
D) NaOH/NH3
Q:
When equal molar amounts of the following sets of compounds are mixed in water, which will not form a buffer solution?
A) NaH2PO4 with Na2HPO4
B) NH3 with NH4Cl
C) CH3CO2H with NaCH3CO2
D) HNO3 with NaNO3
Q:
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 10-4 for methylamine.
A) 10.27
B) 10.57
C) 10.87
D) 11.78
Q:
What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 25.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 10-5 for NH3.
A) 8.95
B) 9.26
C) 9.56
D) 11.13
Q:
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.050 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 10-5 for CH3CO2H.
A) 2.87
B) 4.44
C) 4.74
D) 5.05
Q:
What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 10-10 for HCN.
A) 2.4 10-10 M
B) 4.9 10-10 M
C) 9.8 10-10 M
D) 7.0 10-6 M
Q:
When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF, relative to the pH of the 0.10 M HF solution the pH of the resulting solution will
A) become 7.
B) decrease.
C) increase.
D) remain the same.
Q:
When 50 mL of 0.10 M NH4Cl is added to 50 mL of 0.10 M NH3, relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will
A) become 7.
B) decrease.
C) increase.
D) remain the same.
Q:
What is the common ion in a solution prepared by mixing 0.10 M NaCH3CO2 with 0.10 M CH3CO2H?
A) H3O+
B) Na+
C) CH3CO2-
D) OH-
Q:
Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?A) CH3CO2H(aq) + NaOH(aq) H2O(l) + NaCH3CO2(aq)B) HCl(aq) + C5H5N(aq) C5H5NHCl(aq)C) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)D) H2SO4(aq) + 2 KOH(aq) 2 H2O(l) + K2SO4(aq)
Q:
Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?A) CH3CO2H(aq) + NaOH(aq) H2O(l) + NaCH3CO2(aq)B) HCl(aq) + C5H5N(aq) C5H5NHCl(aq)C) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)D) H2SO4(aq) + 2 KOH(aq) 2 H2O(l) + K2SO4(aq)
Q:
Which of these neutralization reactions has a pH = 7 when equal molar amounts of acid and base are mixed?A) CH3CO2H(aq) + NaOH(aq) H2O(l) + NaCH3CO2(aq)B) HCl(aq) + C5H5N(aq) C5H5NHCl(aq)C) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)D) HNO2(aq) + NH3(aq) NH4NO2(aq)
Q:
The neutralization constantKn for the neutralization of phenobarbital (C12H12N2O3) and morphine (C17H19NO3) is 2.9. The acid dissociation constant Ka for phenobarbital is 3.9 10-8. What is the base dissociation constant Kb for morphine?
A) 1.3 10-22
B) 6.3 10-23
C) 7.4 10-7
D) 1.1 107
Q:
The neutralization constantKn for the neutralization of acetylsalicylic acid (C9H8O4) and codeine (C18H21NO3) is 4.8 104. The acid dissociation constant Ka for acetylsalicylic acid is 3.0 10-4. What is the base dissociation constant Kb for codeine?
A) 4.8 10-24
B) 6.3 10-23
C) 1.6 10-6
D) 1.4 1015
Q:
What is the approximate value of the equilibrium constant, Kn, for the neutralization of hydrochloric acid with sodium hydroxide, shown in the equation below?HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)A) 1.0 102B) 1.0 107C) 1.0 1014D) 1.0 1028
Q:
What is the approximate value of the equilibrium constant, Kn, for the neutralization of nitrous acid with ammonia, shown in the equation below? The Ka for HNO2 is 4.5 10-4 and the Kb for NH3 is1.8 10-5.HNO2(aq) + NH3(aq) NH4NO2(aq)A) 8.1 105B) 1.8 109C) 4.5 1010D) 8.1 1019
Q:
What is the approximate value of the equilibrium constant, Kn, for the neutralization of pyridine with hydrochloric acid, shown in the equation below? The Kb for pyridine is 1.8 10"9.HCl(aq) + C5H5N(aq) C5H5NHCl(aq)A) 5.6 10-10B) 5.6 10-6C) 1.8 105D) 5.6 108
Q:
What is the approximate value of the equilibrium constant, Kn, for the neutralization of acetic acid with sodium hydroxide, shown in the equation below? The Ka for acetic acid is 1.8 10"5.CH3CO2H(aq) + NaOH(aq) H2O(l) + NaCH3CO2(aq)A) 1.8 10-19B) 5.6 10-10C) 1.8 10-8D) 1.8 109
Q:
What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid, the Kb of the base and Kw?
A) Kn = KaKbKw
B) Kn = C) Kn = D) Kn =
Q:
Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?A) H3O+(aq) + OH-(aq) 2 H2O(l)B) HF(aq) + NH3(aq) NH4+(aq) + F-(aq)C) HF(aq) + OH-(aq) H2O(l) + F-(aq)D) H3O+(aq) + NH3(aq) NH4+(aq) + H2O(l)
Q:
Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?A) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)B) H3O+(aq) + OH-(aq) 2 H2O(l)C) HCl(aq) + NH3(aq) NH4Cl(aq)D) H3O+(aq) + NH3(aq) NH4+(aq) + H2O(l)
Q:
Which is a net ionic equation for the neutralization of a weak acid with a strong base?A) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)B) H3O+(aq) + OH-(aq) 2 H2O(l)C) HF(aq) + NaOH(aq) H2O(l) + NaF(aq)D) HF(aq) + OH-(aq) H2O(l) + F-(aq)
Q:
Which is a net ionic equation for the neutralization of a strong acid with a strong base?A) HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)B) H3O+(aq) + OH-(aq) 2 H2O(l)C) HF(aq) + NaOH(aq) H2O(l) + NaF(aq)D) HF(aq) + OH-(aq) H2O(l) + F-(aq)
Q:
CaF2 has Ksp = 3.5 10-11. If 25 mL of 8.0 10-4 M Ca(NO3)2 is mixed with 75 mL of
4.0 10-4 M KF, a precipitate of CaF2 ________ (will, will not) form.
Q:
State whether the solubility of Cu(OH)2 will increase or decrease upon the addition of aqueous solutions of a) HCl, b) NaOH, c) NH3.
Q:
The artist's pigment cadmium yellow, CdS, has a water solubility of 0.13 g/L. The solubility product of CdS, Ksp = ________.
Q:
Silver oxalate, Ag2C2O4, has a molar solubility = 1.1 10-4 mol/L. Ag2C2O4 has a solubility product Ksp = ________.
Q:
At 25C calcium fluoride has a solubility product constant Ksp = 3.5 10-11. The solubility of CaF2 at this temperature is ________ mol/L.
Q:
Selenous acid, H2SeO3 has acid dissociation constants Ka1 = 3.5 10-2 and Ka2 = 5 10-8. When 25.00 mL of 0.100 M selenous acid is titrated with 0.200 M NaOH the first equivalence point occurs at pH = ________.
Q:
The half equivalence point in the titration of 0.100 M CH3NH2 (Kb = 3.7 10-4) with 0.250 M HCl occurs at pH = ________.
Q:
The half equivalence point in the titration of 0.100 M HCO2H (Ka = 1.8 10-4) with 0.250 M NaOH occurs at pH = ________.
Q:
What is the pH of the solution formed when 25 mL of 0.173 M NaOH is added to 35 mL of 0.342 M HCl?
Q:
What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?
Q:
The addition of ________ mL of 0.1500 M NaOH is required to titrate 25.00 mL of 0.2250 M HCl to the equivalence point, which occurs at a pH of ________.
Q:
What is the Ka of the amino acid glutamine if it is 33.0% dissociated at pH = 8.82?
Q:
What is the Ka of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?
Q:
Addition of 0.0125 mol HCl to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________? The Ka of formic acid is 1.8 10-4.
Q:
Addition of 0.0125 mol KOH to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________? The Ka of formic acid is 1.8 10-4.
Q:
The pH of a 0.150 M formic acid/0.250 M sodium formate buffer = ________? The Ka of formic acid is 1.8 10-4.
Q:
A buffer prepared by mixing equal moles of an acid having Ka = 4.5 10-4 and a salt of its conjugate base has a pH = ________.
Q:
A buffer prepared by mixing 50.00 mL of 0.10 M HF with 50.00 mL of 0.10 M NaF will have a pH that is ________ 7.0.
Q:
The pH of a solution of ethylamine, C2H5NH2 (Kb = 6.4 10-4) and ethylammium bromide, C2H5NH3Br is 11.00. What is the molarity of C2H5NH3Br if the molarity of C2H5NH2 is 0.025 M?
Q:
The pH of a solution of HIO3 (Ka = 1.7 10-1) and KIO3 is 1.00. What is the molarity of KIO3 if the molarity of HIO3 is 0.025 M?
Q:
The solution formed upon adding 50.00 mL of 0.10 M NH4Cl to 50.00 mL of 0.10 M NH3 will have a pH that is ________ the pH of the original NH3 solution.
Q:
The neutralization constantKn for the neutralization of penicillin V (C16H18N2O5S) and erythromycin (C37H67NO13) is 1.3 106. The acid dissociation constant Ka for penicillin V is
2.0 10-3. What is the base dissociation constant Kb for erythromycin?
Q:
What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid, the Kb of the base and Kw?
Q:
The balanced net ionic equation for the neutralization reaction involving equal molar amounts of
HCl and CH3CH2NH2 is ________.
Q:
The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HNO3 and KOH is ________.
Q:
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.A) 6.5 10-5 MB) 1.3 10-4 MC) 3.2 10-4 MD) 6.8 10-2 M
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 1.0 1021.
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 0. 20 M NH3? Ksp for AgCl is 1.8 10-10 and Kf for Ag(NH3)2+ is 1.7 107.
A) 1.3 10-5 M
B) 1.0 10- 2 M
C) 1.1 10- 2 M
D) 5.5 10-2 M
Q:
In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25C?
A) 0.1 M H Br
B) 0.1 M NaBr
C) 0.1 M CaBr2
D) 0.1 M KNO3
Q:
Calculate the molar solubility of thallium(I) chloride in 0. 40 M NaCl at 25C. Ksp for TlCl is
1.7 10-4.
A) 6.8 10-5 M
B) 4.2 10- 4 M
C) 8.2 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 12.50? Ksp for Mg(OH)2 is 5.61 10-12.
A) 1.8 10- 10 M
B) 5.6 10- 9 M
C) 2.4 10-6 M
D) 1.1 10-4 M
Q:
Calculate the solubility (in g/L) of silver chromate in water at 25C if the Ksp for Ag2CrO4 is
1.1 10-12.
A) 3.5 10-4 g/L
B) 6.5 10-5 g/L
C) 2.7 10-2 g/L
D) 3.4 10-2 g/L
Q:
Calculate the Ksp for silver sulfite if the solubility of Ag2SO3 in pure water is 4.6 10-3 g/L.
A) 3.8 10-15
B) 1.5 10-14
C) 2.4 10-10
D) 4.8 10-10
Q:
What is the pH of the resulting solution if 45 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) 2.77
B) 4.09
C) 9.91
D) 11.23
Q:
What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 10-8 for HOCl.
A) 0.30
B) 3.18
C) 3.76
D) 4.03
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 32.00 mL of 0.500 M HCl to reach the equivalence point?
A) 0. 300 M
B) 0. 312 M
C) 0. 800 M
D) 1. 30 M
Q:
What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0. 100 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. 40
Q:
What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 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 25.00 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. 43
B) 9.08
C) 4.92
D) 4. 57