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Chemistry
Q:
What is the magnitude of the change in pH when 1.8 g of NaOH is added to 1.00 L of a solution that is 0.100 M in N and 0.100 M in NCl? for N is 1.8 .
A) 0.42
B) 0.00
C) 0.19
D) 1.33
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 The Ka for acetic acid is 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 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 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 / buffer if the 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 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 / buffer if the 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:
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 is 1.8 10"5.
HNO2(aq) + NH3(aq) ⇌ NH4NO2(aq)
A) 8.1 105
B) 1.8 109
C) 4.5 1010
D) 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. A) 1.8 10-19B) 5.6 10-10C) 1.8 10-8D) 1.8 109
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:
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:
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:
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 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 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 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 and Kf for Ag(NH3)2+ is 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 HBr
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 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 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 .
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 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 = for CH3CO2H.
A) 5.28
B) 7.00
C) 8.72
D) 10.02
Q:
Equal volumes of 0.10 M NH3 (Kb = 1.8 10-5) and 0.10 M HCN (Ka = 4.9 10-10) are mixed together. Will the resulting solution be acidic, basic, or neutral?
A) acidic
B) basic
C) neutral
D) insufficient information to solve
Q:
Calculate the pH of a 0.100 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is A) 2.22
B) 5.78
C) 8.22
D) 11.78
Q:
Calculate the pH of a of 0.100 M KBrO solution. Ka for hypobromous acid, HBrO, is A) 3.15
B) 4.85
C) 9.15
D) 10.85
Q:
Calculate the pH of a 0.100 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is A) 2.87
B) 5.13
C) 8.87
D) 11.13
Q:
Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?
A) NH4Cl
B) BaO
C) NaHSO4
D) RbI
Q:
Which one of the following salts, when dissolved in water, produces the solution with the highest pH?
A) KI
B) KBr
C) KCl
D) KF
Q:
Arrange the following 0.10 M aqueous solutions in order of increasing pH: NaOH, HBr, NaCH3CO2, KBr, NH4Br.
A) HBr, KBr, NH4Br, NaCH3CO2, NaOH
B) NaOH, NaCH3CO2, NH4Br, KBr, HBr
C) NaOH, NaCH3CO2, KBr, NH4Br, HBr
D) HBr, NH4Br, KBr, NaCH3CO2, NaOH
Q:
Which one of the following salts, when dissolved in water, produces the solution with the highest pH?
A) NaHSO4
B) LiClO4
C) MgO
D) CH3NH3I
Q:
Which of the following salts are acidic?
A) LiCl, NaCl, KCl
B) NH4Cl, CuCl2, AlCl3
C) NaCH3CO2, KCH3CO2, RbCH3CO2
D) NaCl, NH4Cl, Na2CO3
Q:
Dihydrogen phosphate H2PO4-, has an acid dissociation constant of What is the conjugate base of H2PO4- and what is its base dissociation constant?
A) H3PO4, 1.6 106
B) H3PO4, 1.6 10-8
C) HPO42-, 1.6 106
D) HPO42-, 1.6 10-8
Q:
Acetic acid CH3COOH, has an acid dissociation constant of 1.8 10-5. What is the conjugate base of acetic acid and what is its base dissociation constant?
A) CH3C(OH)2+, 5.6 104
B) CH3C(OH)2+, 5.6 10-10
C) CH3COOH, 5.6 10-10
D) CH3CO2-, 5.6 10-10
Q:
Methylamine CH3NH2, has a base dissociation constant of 3.7 10-4. What is the conjugate acid of methylamine and what is its acid dissociation constant?
A) CH3NH3+, 2.7 103
B) CH3NH3+, 3.7 10-4
C) CH3NH3+, 2.7 10-11
D) CH3NH2-, 2.7 10-11
Q:
Ammonia NH3, has a base dissociation constant of 1.8 10-5. What is the conjugate acid of ammonia and what is its acid dissociation constant?
A) NH4+, 1.9 109
B) NH4+, 1.8 10-5
C) NH4+, 5.6 10-10
D) NH2-, 5.6 10-10
Q:
What is the relationship between Ka and Kb at 25C for a conjugate acid base pair?
A) Ka Kb = 1 10-14
B) Ka/Kb = 1 10-14
C) Kb/Ka = 1 10-14
D) Ka + Kb = 1 10-14
Q:
How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH of 9.00? The Kb for pyridine is 1.9 and the equation of interest isC5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq).A) 0.053 gB) 0.42 gC) 0.79 gD) 7.9 g
Q:
Determine the ammonia concentration of an aqueous solution that has a pH of 11.50. The equation for the dissociation of NH3 (Kb = 1.8 10-5) is A) 2.5 M
B) 0.55 M
C) 5.7 10-3 M
D) 3.2 10-3 M
Q:
Aniline, (C6H5NH2, Kb = 4.3 10-10 at 25C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 3.90 g of aniline in enough water to make 100 mL of solution.
A) 4.87
B) 9.13
C) 9.74
D) 10.74
Q:
What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 10-9 ? The equation for the dissociation of pyridine is A) 4.62
B) 8.72
C) 9.38
D) 10.38
Q:
The concentration of CN in a 0.20 M methylamine (C) solution is 2.32 M. What is for methylamine?
A) 2.7 B) 5.4 C) 1.2 D) 3.3
Q:
What is the concentration of N in a 0.20 M ammonia solution? The base dissociaton constant for ammonia is 1.8 .
A) 0.0019 M
B) 0.20 M
C) 0.020 M
D) 0.040 M
Q:
What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 10-5 ? The equation for the dissociation of NH3 is A) 1.87
B) 2.87
C) 11.13
D) 12.13
Q:
Which of the following can be classified as a weak base?
A) CH3NH2
B) NH2OH
C) Both CH3NH2 and NH2OH
D) Neither CH3NH2 nor NH2OH
Q:
What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 10-4 and Ka2 = 1.0 10-11?
A) 3.6 10-3 M
B) 1.3 10-4 M
C) 1.3 10-5 M
D) 1.0 10-11 M
Q:
What is the pH of a 0.10 M H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 10-4 and Ka2 = 1.0 10-11?
A) 2.44
B) 3.89
C) 4.89
D) 5.50
Q:
Calculate the concentration of bicarbonate ion, HCO3-, in a 0.010 M H2CO3 solution that has the stepwise dissociation constants and A) 6.6 10-5 M
B) 4.3 10-7 M
C) 4.3 10-9 M
D) 5.6 10-11 M
Q:
Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 10-2 and Ka2 = 6.3 10-8.
A) 1.26
B) 1.32
C) 1.82
D) 2.52