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Chemistry
Q:
Calculate the pH of a 0.020 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants and A) 1.70
B) 4.03
C) 6.37
D) 10.25
Q:
What is the second stepwise equilibrium constant expression for phosphoric acid H3PO4?
A) Ka2 = ([H3O+][H2PO4-])/([H3PO4])
B) Ka2 = ([H3O+]2[HPO42-])/([H3PO4])
C) Ka2 = ([H3O+]3[PO43-])/([H3PO4])
D) Ka2 = ([H3O+][HPO42-])/([H2PO4-])
Q:
Which of the following are weak diprotic acids?
A) carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3CO2H
B) formic acid - HCO2H, acetic acid CH3CO2H, benzoic acid C6H5CO2H
C) carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3
D) hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4
Q:
The percent dissociation of acetic acid changes as the concentration of the acid decreases. A 100-fold decrease in acetic acid concentration results in a ________ fold ________ in the percent dissociation.
A) 10, increase
B) 10, decrease
C) 100, increase
D) 100, decrease
Q:
What is the percent dissociation of a benzoic acid solution with pH = 2.59? The acid dissociation constant for this monoprotic acid is A) 0.50%
B) 1.5%
C) 2.5%
D) 3.5%
Q:
Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H) in water. Given that the pH for acetic acid is 2.41, the and assuming the density of vinegar to be 1.00 g/cm3, what is the percent dissociation of acetic acid in vinegar?
A) 0.47%
B) 1.5%
C) 4.0%
D) 5.0%
Q:
Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H) in water. Given that for acetic acid and assuming the density of vinegar to be 1.00 g/cm3, what is the pH of this vinegar solution?
A) 2.00
B) 2.41
C) 2.87
D) 4.74
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 0.40 g of KHP is dissolved in enough water to produce 25.0 mL of solution.
A) 2.10
B) 3.26
C) 4.30
D) 5.41
Q:
Benzoic acid (C6H5CO2H = HBz) solutions are sometimes used in experiments to determine the molarity of a basic solution of unknown concentration. What is the pH of a 0.100 M solution of benzoic acid if and the equilibrium equation of interest is A) 1.00
B) 2.59
C) 4.19
D) 5.19
Q:
A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or was dissolved in enough water to make 100 mL of solution. Given that Ka = 3.0 10-4 for aspirin, what is the pH of the solution?A) 1.57B) 2.54C) 3.52D) 5.08
Q:
Para-Aminobenzoic acid (PABA), p-H2NC6H4(COOH), is used in some sunscreens and hair conditioning products. Calculate the pH of an aqueous solution with and A) 1.52
B) 3.09
C) 4.66
D) 6.18
Q:
What is the hydronium ion concentration of a 0.100 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 10-4B) 5.9 10-4C) 1.9 10-5D) 5.9 10-5
Q:
What is the p of hypobromous acid, HOBr, if a 0.40 M HOBr has a pH of 4.50?
A) 8.60
B) 4.50
C) 6.11
D) 4.92
Q:
The of hypochlorous acid, HOCl, is 3.5 . What is the pH of 0.78 M HOCl?
A) 3.78
B) 3.50
C) 2.82
D) 2.53
Q:
The p of HCN is 9.31. What is the pH of a 0.52 M solution of HCN?
A) 4.80
B) 5.20
C) 6.79
D) 6.33
Q:
What is the hydronium ion concentration of a 0.100 M acetic acid solution with a Ka = 1.8 10-5? The equation for the dissociation of acetic acid is:CH3CO2H(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq).A) 1.3 10-2 MB) 4.2 10-2 MC) 1.3 10-3 MD) 4.2 10-3 M
Q:
What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?
A) hydrofluoric acid with Ka = 3.5 10-4
B) benzoic acid with Ka = 6.5 10-5
C) acetic acid with Ka = 1.8 10-5
D) hypochlorous acid with Ka = 3.5 10-8
Q:
The pH of 0.150 M CH3CO2H, acetic acid, is 2.78. What is the value of Ka for acetic acid?
A) 2.8 10-6
B) 1.9 10-5
C) 1.7 10-3
D) 1.1 10-2
Q:
The pH of 0.255 M HCN is 4.95. What is the value of Ka for hydrocyanic acid?
A) 1.3 10-10
B) 4.9 10-10
C) 1.1 10-5
D) 4.4 10-5
Q:
Determine the acid dissociation constant for a 0.020 M formic acid solution that has a pH of 2.74. Formic acid is a weak monoprotic acid and the equilibrium equation of interest is A) 1.8 10-3
B) 1.8 10-4
C) 3.6 10-4
D) 3.6 10-5
Q:
Determine the acid dissociation constant for a 0.010 M nitrous acid solution that has a pH of 2.70. Nitrous acid is a weak monoprotic acid and the equilibrium equation of interest is A) 8.0 10-3
B) 2.0 10-3
C) 5.0 10-4
D) 4.0 10-4
Q:
Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is A) 1.3 10-2
B) 1.3 10-3
C) 1.8 10-5
D) 1.8 10-6
Q:
What is the equilibrium constant expression (Ka) for the acid dissociation of nitrous acid HNO2? The equation of interest isHNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq).A) Ka = ([H3O+][NO2-])/([HNO2][H2O])B) Ka = ([H3O+][NO2-])/([HNO2])C) Ka = ([HNO2][H2O])/([H3O+][NO2-])D) Ka = ([HNO2])/([H3O+][NO2-])
Q:
What is the equilibrium constant expression (Ka) for the acid dissociation of hydrocyanic acid HCN? The equation of interest isHCN(aq) + H2O(l) H3O+(aq) + CN-(aq).A) Ka = ([H3O+][CN-])/([HCN][H2O])B) Ka = ([H3O+][CN-])/([HCN])C) Ka = ([HCN][H2O])/([H3O+][CN-])D) Ka = ([HCN])/([H3O+][CN-])
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 0.100 M NaOH? Assume that the volumes are additive.
A) 12.67
B) 12.78
C) 12.95
D) 13.25
Q:
What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO3, 50.0 mL of 0.20 M HCl, and 100.0 mL of water? Assume that the volumes are additive.
A) 0.30
B) 0.82
C) 1.00
D) 1.10
Q:
What is the pH of a solution made by mixing 100.00 mL of 0.20 M HCl with 50.00 mL of 0.10 M HCl? Assume that the volumes are additive.
A) 0.15
B) 0.52
C) 0.78
D) 1.70
Q:
What is the pH of a solution prepared by diluting 25.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?
A) 2.40
B) 2.70
C) 11.30
D) 11.60
Q:
What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?
A) 1.00
B) 1.60
C) 2.00
D) 3.20
Q:
What is the pH of a solution prepared by dissolving 0.15 gram 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) 2.57B) 2.87C) 11.13D) 11.43
Q:
What is the pH of a 0.020 M Ba(OH)2 solution?
A) 1.40
B) 1.70
C) 12.30
D) 12.60
Q:
What is the pH of a 0.020 M RbOH solution?
A) 0.020
B) 0.040
C) 1.70
D) 12.30
Q:
What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators
HIn In-
pH range
Solution X methyl orange
red-yellow
3.2-4.4
yellow methyl red
red-yellow
4.8-6.0
yellow bromthymol blue
yellow-blue
6.0-7.6
blue phenolphthalein
colorless-pink
8.2-10.0
pink A) 4.8 - 6.0
B) 6.0 - 7.6
C) 7.6 - 8.2
D) > 8.2
Q:
What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators
HIn In-
pH range
Solution X methyl orange
red-yellow
3.2-4.4
yellow methyl red
red-yellow
4.8-6.0
orange bromthymol blue
yellow-blue
6.0-7.6
yellow phenolphthalein
colorless-pink
8.2-10.0
colorless A) 3.2 - 4.4
B) 4.8 - 6.0
C) 6.0 - 7.6
D) 8.2 - 10.0
Q:
What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators
HIn In-
pH range
Solution X methyl orange
red-yellow
3.2-4.4
yellow methyl red
red-yellow
4.8-6.0
yellow bromthymol blue
yellow-blue
6.0-7.6
green phenolphthalein
colorless-pink
8.2-10.0
colorless A) 3.2 - 4.4
B) 4.8 - 6.0
C) 6.0 - 7.6
D) 8.2 - 10.0
Q:
At 25C, the pH of a vinegar solution is 2.60. What are the values of [H3O+] and [OH-] in the solution?
A) 3.99 10-12 M, 2.51 10-3 M
B) 2.51 10-3 M, 3.98 10-12 M
C) 2.51 10-3 M, 11.40 M
D) 2.60 M, 11.40 M
Q:
What statement is most consistent for an acid with a pH = 3?
A) one one-hundredth as strong as an acid with a pH of 5
B) half a strong as an acid with a pH = 5
C) twice as strong as an acid with a pH of 5
D) one hundred times as strong as an acid with a pH = 5
Q:
What is the hydroxide ion concentration of a lye solution that has a pH of 11.20?
A) 6.31 10-12 M
B) 1.58 10-3 M
C) 2.80 M
D) 11.20 M
Q:
What is the hydronium ion concentration of an acid rain sample that has a pH of 3.15?
A) 1.41 10-11 M
B) 7.08 10-4 M
C) 3.15 M
D) 10.85 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 10-11 M, 3.65
B) 4.44 10-11 M, 10.35
C) 4.44 10-12 M, 2.65
D) 4.44 10-12 M, 11.35
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 10-10 M, 4.82
B) 6.67 10-10 M, 9.18
C) 6.67 10-11 M, 3.82
D) 6.67 10-11 M, 10.18
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
B) 2.15 10-3
C) 2.67
D) 11.33
Q:
If the ionization constant of water, Kw, at 40C is 2.92 10-14, then what is the hydronium ion concentration and pH for an acidic solution?
A) [H3O+] > 1.71 10-7 M and pH > 6.77
B) [H3O+] > 1.71 10-7 M and pH < 6.77
C) [H3O+] < 1.71 10-7 M and pH > 6.77
D) [H3O+] < 1.71 10-7 M and pH < 6.77
Q:
An acidic solution at 25C will have a hydronium ion concentration ________ and a pH value ________.
A) [H3O+] > 1 10-7 M, pH > 7.00
B) [H3O+] > 1 10-7 M, pH < 7.00
C) [H3O+] < 1 10-7 M, pH > 7.00
D) [H3O+] < 1 10-7 M, pH < 7.00
Q:
If the ionization constant of water, Kw, at 40C is 2.92 10-14, then what is the hydronium ion concentration for a neutral solution?
A) [H3O+] < 1.00 10-7 M
B) [H3O+] > 1.71 10-7 M
C) [H3O+] = 1.71 10-7 M
D) [H3O+] < 1.71 10-7 M
Q:
A solution with a hydroxide ion concentration of 4.15 10-4 M is ________ and has a hydrogen ion concentration of ________.
A) acidic, 2.41 10-10 M
B) acidic, 2.41 10-11 M
C) basic, 2.41 10-10 M
D) basic, 2.41 10-11 M
Q:
A solution with a hydrogen ion concentration of 3.25 10-2 M is ________ and has a hydroxide concentration of ________.
A) acidic, 3.08 10-12 M
B) acidic, 3.08 10-13 M
C) basic, 3.08 10-12 M
D) basic, 3.08 10-13 M
Q:
Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 10-3 M in hydronium ion.
A) 2.86 10-4 M
B) 2.86 10-11 M
C) 2.86 10-12 M
D) 3.50 10-12 M
Q:
Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 10-4 M in hydroxide ion.
A) 4.00 10-9 M
B) 4.00 10-10 M
C) 4.00 10-11 M
D) 5.00 10-11 M
Q:
At 50C the value of Kw is 5.5 10-14. A basic solution at 50C has
A) [H3O+] < [OH-] < 2.3 10-7 M.
B) [H3O+] < 2.3 10-7 M < [OH-].
C) [H3O+] = [OH-] < 2.3 10-7 M.
D) [H3O+] > 2.3 10-7 M < [OH-].
Q:
An acidic solution at 25C has
A) [H3O+] > [OH-] > 1 10-7 M.
B) [H3O+] > 1 10-7 M > [OH-].
C) [H3O+] = [OH-] > 1 10-7 M.
D) [H3O+] < 1 10-7 M > [OH-].
Q:
What is the geometric shape of the hydrated proton; that is, the hydronium ion H3O+?
A) angular
B) trigonal pyramidal
C) trigonal planar
D) tetrahedral
Q:
Arrange the acids in order of increasing acid strength.
A) D < C < A < B
B) D < C < B < A
C) D < B < A < C
D) D < A < C < B
Q:
The following pictures represent aqueous solutions of binary acids of the type HA where the water molecules have been omitted for clarity.Determine the strongest acid of the set.A) AB) BC) CD) D
Q:
The equilibrium constant, K, for the reaction shown below has a value 1.8 10-5. In this reaction which is the strongest acid and which is the strongest base?CH3CO2H(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq)A) CH3CO2H and CH3CO2-B) CH3CO2H and H2OC) H3O+ and H2OD) H3O+ and CH3CO2-
Q:
From the following chemical reactions determine the relative Brnsted-Lowry base strengths (strongest to weakest).2 NaH(s) + H2O(l) -> 2 NaOH + H2(g)NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)A) H- > OH- > NH3B) H- > NH3 > OH-C) OH-> H- > NH3D) OH- > NH3 > H-
Q:
From the following chemical reactions determine the relative Brnsted-Lowry base strengths (strongest to weakest).HNO3(aq) + H2O(l) -> H3O+(aq) + NO3-(aq)HF(aq) + H2O(l) H3O+(aq) + F-(aq)A) HNO3 > H3O+ > HFB) NO3- > H2O > F-C) F- > H2O > NO3-D) F- > NO3- > H2O
Q:
From the following chemical reactions determine the relative Brnsted-Lowry acid strengths (strongest to weakest).HClO4(sol) + CH3COOH(l) -> CH3C2(OH)2+(sol) + ClO4-(aq)H2SO4(sol) + CH3COOH(l) CH3C(OH)2+(sol) + HSO4-(sol)A) HClO4 > H2SO4 > CH3COOHB) HClO4 > H2SO4 > CH3C(OH)2+C) HClO4 > CH3COOH > H2SO4D) HClO4 > CH3C(OH)2+ > H2SO4
Q:
From the following chemical reactions determine the relative Brnsted-Lowry acid strengths (strongest to weakest).HClO4(aq) + H2O(l) -> H3O+(aq) + ClO4-(aq)HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)A) HClO4 > H3O+ > HNO2B) HClO4 > HNO2 > H3O+C) H3O+ > HClO4 > HNO2D) H3O+ > HNO2 > HClO4
Q:
From the following chemical reactions determine the relative Brnsted-Lowry acid strengths (strongest to weakest).HCl(aq) + H2O(l) -> H3O+(aq) + Cl-(aq)HCN(aq) + H2O(l) H3O+(aq) + CN-(aq)A) HCl > HCN > H3O+B) HCl > H3O+ > HCNC) H3O+ > HCl > HCND) HCN > H3O+ > HCl
Q:
What is the strongest Brnsted-Lowry acid in the chemical reaction shown below?2 HNO3(aq) + Ba(OH)2(aq) Ba(NO3)2(aq) + 2 H2O(l)A) HNO3B) Ba(OH)2C) Ba(NO3)2D) H2O
Q:
Which Brnsted-Lowry acid has the strongest conjugate base?
A) HCl
B) HClO4
C) HF
D) H
Q:
Which Brnsted -Lowry base has the strongest conjugate acid?
A) CH3CO2-
B) CN-
C) F-
D) NO3-
Q:
Which of the following Brnsted-Lowry acids does not behave as a strong acid when it is dissolved in water?
A) H
B) HCl
C) HNO2
D) HClO4
Q:
Write a balanced equation for the dissociation of the Brnsted-Lowry acid HSO4- in water.A) HSO4-(aq) + H2O(l) H2SO4(aq) + OH-(aq)B) HSO4-(aq) + H2O(l) SO42-(aq) + H3O+(aq)C) HSO4-(aq) + H2O(l) SO32-(aq) + OH-(aq)D) HSO4-(aq) + H2O(l) SO3(g) + OH-(aq) + H2O(l)
Q:
Which one of the following can behave either as a Brnsted-Lowry acid or a Brnsted-Lowry base in an aqueous solution reaction?
A) HSO3-
B) NH3
C) HI
D) H3PO4
Q:
What is the conjugate acid of the Brnsted-Lowry base HAsO42-?
A) H2AsO4-
B) AsO43-
C) H2O
D) H3O+
Q:
What is the conjugate base of the Brnsted-Lowry acid HPO42-?
A) H3PO4
B) H2PO4-
C) HPO42-
D) PO43-
Q:
Identify the conjugate acid/base pairs present in an aqueous solution of hydrogen sulfate ion, HSO4-.
A) HSO4-/SO42- and H3O+/H2O
B) H2SO4/HSO4- and H2O/OH-
C) HSO4-/H2O and H3O+/SO42-
D) HSO4-/H2O and H2SO4/OH-
Q:
What are the conjugate acid-base pairs in the following chemical reactionNH3(aq) + H2O(l) NH4+(aq) + OH-(aq)?A) NH3, H2O and NH4+, OH-B) NH3, NH4+ and H2O, OH-C) NH3, OH- and H2O, NH4+D) NH3 and NH4+
Q:
What are the Brnsted-Lowry acids in the following chemical reactionHBr(sol) + CH3COOH(sol) CH3C(OH)2+(sol) + Br-(sol)?A) HBr, CH3COOHB) HBr,C) CH3COOH, CH3C(OH)2+D) CH3COOH, Br-
Q:
What are the Brnsted-Lowry bases in the following chemical reactionC5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq)?A) C5H5N, H2OB) C5H5N, C5H5NH+C) C5H5N,D) C5H5N, H2O, OH-
Q:
Indicate all the Brnsted-Lowry acids in the following chemical reactionHCl(aq) + H2O(aq) H3O+(aq) + Cl-(aq).A) HCl, H2OB) HCl,C) HCl, Cl-D) HCl, H2O, H3O+
Q:
In the following chemical equation indicate the reactant that is a Brnsted-Lowry acidHCN(aq) + H2O(l) H3O+(aq) + CN-(aq).A) HCNB) H2OC) H3O+D) CN-
Q:
Which one of the following species acts as a Brnsted-Lowry acid in water?
A) NaH
B) NH4+
C) CH3NH2
D) C6H6
Q:
A Brnsted-Lowry acid is best defined as a substance that can
A) accept a hydroxide ion.
B) donate a hydroxide ion.
C) accept a proton.
D) donate a proton.
Q:
When dissolved in water, which of the following compounds is an Arrhenius base?
A) CH3OH
B) HOCl
C) KOH
D) KCl
Q:
An Arrhenius base is best defined as a
A) proton donor.
B) hydroxide acceptor.
C) substance that dissociates in water to produce aqueous hydrogen ions.
D) substance that dissociates in water to produce aqueous hydroxide ions.
Q:
When dissolved in water, which of the following compounds is an Arrhenius acid?
A) HCN
B) NaOH
C) NaF
D) CH3CH2OH