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Chemistry
Q:
An Arrhenius acid is best defined as a
A) hydroxide donor.
B) proton acceptor.
C) substance that dissociates in water to produce aqueous hydrogen ions.
D) substance that dissociates in water to produce aqueous hydroxide ions.
Q:
The acid strength of an oxoacid having the general formula HnYOm increases as the electronegativity of Y ________ and as the oxidation number of Y ________.
Q:
A 0.10 M KNO2 solution will have a pH ________ seven.
Q:
A 0.050 M solution of hydroxylamine, NH2OH, having Kb = 9.1 10-9 has a pH of ________.
Q:
The value of Ka for a 0.250 M HCN solution having a pH of 4.956 is ________.
Q:
The pH of a 0.025 M KOH solution is ________.
Q:
At 50C the value of Kw is 5.5 10-14, and the pH of a neutral solution at 50C is ________.
Q:
An acidic solution with hydronium ion concentration [H+] = 1.60 10-3 M has a hydroxide ion concentration [OH-] = ________.
Q:
A proton hydrated by four water molecules has the formula ________.
Q:
The equilibrium constant for the reaction below has the value Ka = 3.5 10-4. In this reaction the Brnsted-Lowry acid is ________.HF(aq) + H2O(l) H3O+(aq) + F-(aq)
Q:
The Brnsted-Lowry acid in the chemical equation below is _________.HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)
Q:
Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?A) NaClB) KClC) MgCl2D) AlCl3
Q:
Calculate the pH of a 1.60 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is A) 1.61
B) 5.18
C) 8.82
D) 12.39
Q:
Calculate the pH of a 1.60 M KBrO solution. Ka for hypobromous acid, HBrO, is A) 2.55
B) 4.25
C) 9.75
D) 11.45
Q:
Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is A) 2.42
B) 4.68
C) 9.32
D) 11.58
Q:
Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?
A) NH4Br
B) CaO
C) KHSO4
D) CsI
Q:
Which one of the following salts, when dissolved in water, produces the solution with the highest pH?
A) RbI
B) RbBr
C) RbCl
D) RbF
Q:
If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral?
A) acidic
B) basic
C) neutral
D) There is insufficient information provided to answer this question.
Q:
Which one of the following salts, when dissolved in water, produces the solution with the highest pH?
A) KHCO3
B) CsClO4
C) RaO
D) CH3CH3NH3Cl
Q:
Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH3 (Kb = 1.8 10-5) is A) 3.0 M
B) 0.056 M
C) 1.8 10-2 M
D) 1.0 10-3 M
Q:
Aniline, (C6H5NH2, Kb = at 25C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 6.90 g of aniline in enough water to make 100 mL of solution.
A) 4.75
B) 9.25
C) 9.50
D) 10.50
Q:
What is the pH of a 0.30 M pyridine solution that has 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:
What is the pH of a 0.200 M NH3 solution that has Kb = 1.8 10-5? The equation for the dissociation of NH3 is A) 2.02
B) 2.72
C) 11.98
D) 11.28
Q:
What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of and 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 0.40 M H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 10-4 and A) 2.14
B) 3.89
C) 4.28
D) 5.57
Q:
Calculate the concentration of bicarbonate ion, HCO3-, in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 10-7 and Ka2 = 5.6 10-11.
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 0.60 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5 10-2 and A) 1.02
B) 1.06
C) 1.82
D) 2.04
Q:
Calculate the pH of a 0.080 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 10-7 and Ka2 = 5.6 10-11.
A) 1.10
B) 3.73
C) 6.37
D) 10.25
Q:
Potassium hydrogen phthalate (molar mass = 204.2 g/mol)is one of the most commonly used acids for standardizing solutions containing bases. KHP is a monoprotic weak acid with Calculate the pH of the solution that results when 0.50 g of KHP is dissolved in enough water to produce 25.0 mL of solution.
A) 2.05
B) 3.21
C) 4.40
D) 5.41
Q:
What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with The equation for the dissociation of hypochlorous acid is:HOCl(aq) + H2O(l) -> H3O+(aq) + OCl-(aq).A) 1.9 10-4 MB) 7.2 10-4 MC) 2.8 10-5 MD) 7.2 10-5 M
Q:
What is the hydronium ion concentration of a 0.500 M acetic acid solution with Ka = 1.8 10-5? The equation for the dissociation of acetic acid is:CH3CO2H(aq) + H2O(l) -> H3O+(aq) + CH3CO2-(aq).A) 3.0 10-2 MB) 4.2 10-2 MC) 3.0 10-3 MD) 4.2 10-3 M
Q:
What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.300 M NaOH? Assume that the volumes are additive.
A) 13.05
B) 13.10
C) 13.28
D) 13.58
Q:
What is the pH of a solution prepared by mixing 100.00 mL of 0.20 M HCl with 150.00 mL of 0.10 M HCl? Assume that the volumes are additive.
A) 0.17
B) 0.52
C) 0.85
D) 1.70
Q:
What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?
A) 1.80
B) 2.10
C) 11.90
D) 12.20
Q:
What is the pH of a solution prepared by diluting 20.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?
A) 1.00
B) 1.70
C) 2.00
D) 3.40
Q:
What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)?CaO(s) + H2O(l) -> Ca2+(aq) + 2 OH-(aq)A) 2.10B) 2.40C) 11.60D) 11.90
Q:
What is the pH of a 0.040 M Ba(OH)2 solution?
A) 1.10
B) 1.40
C) 12.60
D) 12.90
Q:
What is the pH of a 0.020 M HClO4 solution?
A) 0.020
B) 0.040
C) 1.70
D) 12.30
Q:
What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?
A) 6.31 10-10 M
B) 1.58 10-5 M
C) 4.80 M
D) 9.20 M
Q:
What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45?
A) 2.82 10-11 M
B) 3.55 10-4 M
C) 3.45 M
D) 10.55 M
Q:
What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of
A) 4.44 10-12 M and 2.65
B) 4.44 10-12 M and 11.35
C) 4.44 10-13 M and 1.65
D) 4.44 10-13 M and 12.35
Q:
What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of A) 6.67 10-12 M, 2.82
B) 6.67 10-12 M, 11.18
C) 6.67 10-13 M, 1.82
D) 6.67 10-13 M, 12.17
Q:
Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.
A) 4.65 10-11
B) 2.15 10-4
C) 3.67
D) 10.33
Q:
Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion.
A) 4.65 10-12 M
B) 2.15 10-3 M
C) 2.67
D) 11.33
Q:
A solution with a hydroxide ion concentration of 4.15 10-6 M is ________ and has a hydrogen ion concentration of ________.
A) acidic, 2.41 10-8 M
B) acidic, 2.41 10-9 M
C) basic, 2.41 10-8 M
D) basic, 2.41 10-9 M
Q:
A solution with a hydrogen ion concentration of 3.25 10-6 M is ________ and has a hydroxide ion concentration of ________.
A) acidic, 3.08 10-8 M
B) acidic, 3.08 10-9 M
C) basic, 3.08 10-8 M
D) basic, 3.08 10-9 M
Q:
Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 10-4 M in hydronium ion.
A) 2.86 10-3 M
B) 2.86 10-10 M
C) 2.86 10-11 M
D) 3.50 10-11 M
Q:
Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 10-6 M in hydroxide ion.
A) 4.00 10-7 M
B) 4.00 10-8 M
C) 4.00 10-9 M
D) 5.00 10-9 M
Q:
When dissolved in water, which compound is generally considered to be an Arrhenius acid?
A) HNO2
B) KOH
C) LiF
D) CH3OH
Q:
BF3 and NH3 undergo a Lewis acid-base reaction forming an adduct. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?A) Picture (1) is correct; NH3 is the Lewis acid and BF3 is the Lewis base.B) Picture (2) is correct; BF3 is the Lewis acid and NH3 is the Lewis base.C) Picture (3) is correct; NH3 is the Lewis acid and BF3 is the Lewis base.D) Picture (4) is correct; BF3 is the Lewis acid and NH3 is the Lewis base.
Q:
CO2 reacts with H2O to form HCO3- and H+. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?(1) (2)A) Picture (1) is correct; H2O is the Lewis acid and CO2 is the Lewis base.B) Picture (1) is correct; CO2 is the Lewis acid and H2O is the Lewis base.C) Picture (2) is correct; H2O is the Lewis acid and CO2 is the Lewis base.D) Picture (2) is correct; CO2 is the Lewis acid and H2O is the Lewis base.
Q:
SO3 reacts with H2O to form H2SO4. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base? A) Picture (1) is correct; H2O is the Lewis acid and SO3 is the Lewis base.
B) Picture (1) is correct; SO3 is the Lewis acid and H2O is the Lewis base.
C) Picture (2) is correct; H2O is the Lewis acid and SO3 is the Lewis base.
D) Picture (2) is correct; SO3 is the Lewis acid and H2O is the Lewis base.
Q:
Of the elements indicated on the periodic table shown above, which forms the weakest oxoacid acid with the formula H2XO3 or HXO3, where A) A
B) B
C) C
D) D
Q:
Of the elements indicated on the periodic table shown above, which forms the strongest oxoacid acid with the formula H2XO3 or HXO3, where A) A
B) B
C) C
D) D
Q:
Of the elements indicated on the periodic table shown above, which forms the weakest binary acid, H2X or HX, where A) A
B) B
C) C
D) D
Q:
Of the elements indicated on the periodic table shown above, which forms the strongest binary acid, H2X or HX, where A) AB) BC) CD) D
Q:
Which picture represents a basic salt?A) (1)B) (2)C) (3)D) none of the above
Q:
Which picture represents a neutral salt?
A) (1)
B) (2)
C) (3)
D) none of the above
Q:
The following pictures represent solutions of three salts MA; water molecules have been omitted for clarity. Dotted spheres represent Ay- ions; gray spheres represent Mx+ ions; black spheres represent oxygen atoms; and unshaded spheres represent hydrogen atoms.Which picture represents an acidic salt?A) (1)B) (2)C) (3)D) none of the above
Q:
The following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions have been omitted for clarity. Arrange the three A- ions in order of decreasing base strength.A) X- > Y- > Z-B) X- > Z- > Y-C) Y- > Z- > X-D) Z- > Y- > XZ-
Q:
Arrange the conjugate bases (A- = X-, Y-, or Z-) in order of increasing value of Kb.
A) Kb(Z-) < Kb(Y-) < Kb(X-)
B) Kb(Y-) < Kb(Z-) < Kb(X-)
C) Kb(Z-) < Kb(X-) < Kb(Y-)
D) Kb(X-) < Kb(Z-) < Kb(Y-)
Q:
Arrange the conjugate bases (A- = X-, Y-, or Z-) in order of increasing base strength.
A) Z- < Y- < X-
B) Y- < Z- < X-
C) Z- < X- < Y-
D) X- < Z- < Y-
Q:
Arrange the acids in order of increasing pH.
A) HZ < HY < HX
B) HY < HZ < HX
C) HZ < HX < HY
D) HX < HZ < HY
Q:
Arrange the acids in order of increasing value of percent dissociation.
A) HZ < HY < HX
B) HY < HZ < HX
C) HZ < HX < HY
D) HX < HZ < HY
Q:
Arrange the acids in order of increasing value of Ka.
A) Ka(HZ) < Ka(HY) < Ka(HX)
B) Ka(HY) < Ka(HZ) < Ka(HX)
C) Ka(HZ) < Ka(HX) < Ka(HY)
D) Ka(HX) < Ka(HZ) < Ka(HY)
Q:
The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity.Arrange the acids in order of increasing acid strength.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HY
Q:
Which of the above pictures represents a solution of a diprotic acid H2A for which and Ka2 is exceptionally small. (Water molecules have been omitted for clarity.)A) picture (a)B) picture (b)C) picture (c)D) picture (d)
Q:
Which of the above pictures represents a solution of a weak diprotic acid H2A for which (Water molecules have been omitted for clarity.)A) picture (a)B) picture (b)C) picture (c)D) picture (d)
Q:
Which acid solution has the lowest pH?A) HXB) HYC) HZD) All have the same pH.
Q:
Which acid has the lowest percent dissociation?
A) HX
B) HY
C) HZ
D) All have the same percent dissociation.
Q:
Which acid has the smallest value of Ka?
A) HX
B) HY
C) HZ
D) All have the same Ka value.
Q:
Which acid, if any, is a strong acid?
A) All are strong acids.
B) HX and HZ
C) HY
D) None are strong acids.
Q:
The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity.Arrange the three acids in order of increasing acid strength.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HY
Q:
In the following reaction the unshaded spheres represent H atoms.Identify the Brnsted-Lowry acid/base conjugate pairs.A) (1)/(2) and (3)/(4)B) (1)/(3) and (2)/(4)C) (1)/(4) and (2)/(3)
Q:
In the following reaction the unshaded spheres represent H atoms.Identify the Brnsted-Lowry acid/base conjugate pairs.A) (1)/(2) and (3)/(4)B) (1)/(3) and (2)/(4)C) (1)/(4) and (2)/(3)
Q:
Identify the Brnsted-Lowry bases.A) (1) and (3)B) (1)C) (2) and (3)D) (2) and (4)
Q:
In the following reaction the unshaded spheres represent H atoms.Identify the Brnsted-Lowry acids.A) (1) and (3)B) (1) and (4)C) (2)D) (2) and (4)
Q:
Identify the Brnsted-Lowry bases.A) (1) and (3)B) (1) and (4)C) (2)D) (2) and (4)
Q:
In the following reaction the unshaded spheres represent H atoms.Identify the Brnsted-Lowry acids.A) (1) and (3)B) (1)C) (2) and (3)D) (2) and (4)
Q:
Which one of the following is expected to be the strongest Lewis acid?A) FeB) Fe+C) Fe2+D) Fe3+