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WorksheetsChemistry Two Exam Three
Total questions: 125
Worksheet time: 1hrs 3mins
2BrNO(g)<->2NO(g)+Br2(g)
What could we do to push the reaction to the right?
Add BrNo
Remove NO
Add NO
Remove BrNo
CaCO3(s)<->CaO(g)+CO2(g)
What can we do to shift it left?
Add more CO2
Remove some CO2
Add more CaCO3
2KClO3(s)<->2KCl(s)+3O2(g)
What change in volume is needed to move it to the right?
no change
increase the volume
decrease the volume
2SO2(g)+O2(g)<->2SO3(g)
Delta H= -253 kJ
list five things we can do to move the reaction to the left?
Add SO3(g)
Remove SO2(g)
Remove O2 (g)
Increase the volume
Increase the heat
Remove SO3(g)
Add SO2(g)
Add O2 (g)
Decrease the volume
Decrease the heat
Consider an exothermic reaction:
2NO(g)+Cl2(g)<->2NOCl(g)
Which change causes a reaction mixture at equilibrium to shift right?
Adding NOCl to the reaction mixture
Increasing the volume of the reaction vessel at constant temperature
Increasing the temperature of the reaction vessel
None of the above
A
B
C
HF= 1.0x10^-4=Ka
HCHO3 Ka=1.8x10^-7
HC2H3O2 Ka=1.6x10^-5
HI
Write them in order from the weakest to the strongest
HI, HCHO3, HC2H3O2, HF,
HC2H3O2, HCHO3, HF, HI
HCHO3, HC2H3O2, HF, HI
[HCl]= 0.20 M
[HNO3]= 0.33 M
[H3O^+]=???
53 M
0.48 M
0.53 M
48 M
A
B
C
HPO4^2- is the conjugate base of what?
H2PO4^-
H3PO4
HPO4^+
C2H5NH3^+ is the conjugate acid of what base?
CH4NH5
C4H2NH6
C2H4NH3
HSO4^- is the conjugate base of what acid?
HSO4
H3SO4
H2SO4
Fill in the Blanks and Balance the Equation.
H2SO4+_NaOH->_H2O+ (a)
Predict if the reaction would shift towards the reactants, products, or no change
C(s)+H2O(g)<->CO(g)+H2(g)
delta H of reaction= 131 J
a. Increasing the temperature
b. Increasing the volume of the container
c. Adding C to the reaction vessel
a. Shifts towards products
b. Shifts towards products
c. No change
a. Shifts towards reactants
b. Shifts towards products
c. Shifts towards reactants
a. Shifts towards products
b. Shifts towards reactants
c. No change
What is the pH of a 0.61 M solution of ammonia in water?
Kb is 1.76x10^-5
11.5
10.5
3.5
12.5
What is the pH of a 0.50 liter buffer solution containing 0.250 M KClO and 0.300 M HClO?
7.46
0.746
9.56
0.956
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
A
B
C
D
E
in a 0.05 M Sr(OH)2 Solution what is the pH?
2
13
1
14
0.2 M of NaHCO3
Kb HCO3=2.3x10^-8
pH=?
9.83
0.500 M HC7H5O2 ka=6.5x10^-5
and 0.500 M HCN ka=4.9x10^-10
PH=??
2.24
H3PO4, HClO4, H2SO4
arrange from weakest to strongest acid
H3PO4, H2SO4, HClO4
0.125 M NaOH
pH=??
2.3
13.1
14.5
10.9
0.01 M LiOH and 0.005 M kOH
pH=??
12.8
8.7
14.6
10.5
Will the following salts make an acidic, basic, or neutral solution:
a. KCN
b. LiBr
c. NH4I
d. C2H5NH3F
a. acidic
b. neutral
c. basic
d. basic
a. basic
b. neutral
c. acidic
d. acidic
a. neutral
b. acidic
c. basic
d. acidic
What is the pH of a 0.0100 M H2SO4 solution?
1.83
C5H5NHC2H3O2
kb of C5H5NH4^+= 1.7x10^-9
ka of C2H3O2^-= 1.8x10^-5
acidic basic or neutral?
neutral
basic
acidic
Identify the Lewis acid and Lewis base:
Fe^3+(aq)+6H20(l)<->Fe(H20)6(aq)
Fe^3+ is the Lewis acid and H2O is the Lewis base.
Identify the Lewis acid and the Lewis base:
F^-(aq)+BF3(aq)<->BF4^-(aq)
What solution is a buffer?
a solution that is 0.100 M in HNO2 and 0.100 M in HCl
a solution that is 0.100 M in HNO3 and 0.100 M in NaNO3
a solution that is 0.100 M in HNO2 and 0.100 M in NaCl
a solution that is 0.100 M in HNO2 and 0.100 M in NaNO2
What is the pH of a buffer solution that contains 0.250 M NH3 and 0.200 M NH4^+
What would the pH be if we added 0.010 M HCl to a 0.200 M HC2H3O2, 0.200 M NaC2H3O2 buffer?
4.74
6.783
3.89
2.56
Which is the Ksp for FeCl3 (s)?
x^2
4x^3
6x^4
9x^4
27x^4
In which solution is BaSO4 most soluble?
a solution that is 0.10 M in BaNO3
a solution that is 0.10 M. in Na2SO4
a solution that is 0.10 M in NaNO3
Ca(OH)2
x=1.2x10^-3
Ksp=?
6.912x10^-9
What concentration of Fluoride would you need to find in a saturated solution of CaF2
Ksp= 1.46x10^-10
6.63x10^-4
What is the molar solubility of PbSO4?
Ksp PbSO4= 1.82x10^-8
What is the molar solubility of BaF2(s)?
Ksp=2.45x10^-5
0.0183 M
What is the molar solubility of AgCl?
Ksp= 1.77x10^-10
1.33x10^-5
3.45x10^-5
5.63x10^-5
7.34x10^-5
A 1.0 L buffer solution is 0.10 M in HF and 0.050 M in NaF. Which action destroys the buffer?
adding 0.050 mol of NaF
adding 0.050 mol of NaOH
adding 0.050 mol of HCl
none of the above
A buffer contains the weak acid HA and its conjugate base A^-. The weak acid has a pKa of 4.82 and the buffer has a pH of 4.25
Which statement is true of the relative concentrations of the weak acid and conjugate base in the buffer?
[HA]>[A^-]
[HA]<[A^-]
[HA]=[A^-]
a
b
c
a. Shift right
b. Shift left
c. Shift left
a. Shift left
b. Shift right
c. Shift right
a. Shift right
b. Shift right
c. Shift left
a shift right
b unchanged
c unchanged
d shift left
a shift left
b unchanged
c unchanged
d shift right
a unchanged
b shift left
c shift right
d unchanged
a. no effect
b. shift left
c. shift left
a. no effect
b. shift right
c. no effect
a. shift left
b. shift right
c. no effect
a. shift right
b. shift left
c. no effect
increase temp: shift right
decrease temp: shift left
increasing temp increases the equilibrium constant
increase temp: shift right
decrease temp: shift left
increasing temp decreases the equilibrium constant
increase temp: shift left
decrease temp: shift right
increasing temp increases the equilibrium constant
increase temp: shift left
decrease temp: shift right
increasing temp decreases the equilibrium constant
a. base, HNO3(aq)->H^+(aq)+5NO3^-(aq)
b. acid, NH4^+(aq)<->H^+(aq)+NH3(aq)
c. base, KOH(aq)->K^+(aq)+OH^-(aq)
d.acid, HC2H3O2(aq)<->H^+(aq)+4C2H3O2^-(aq)
a. acid, HNO3(aq)->H^+(aq)+NO3^-(aq)
b. acid, NH4^+(aq)<->H^+(aq)+NH3(aq)
c. base, KOH(aq)->K^+(aq)+OH^-(aq)
d.acid, HC2H3O2(aq)<->H^+(aq)+C2H3O2^-(aq)
a. acid, HNO3(aq)->H^+(aq)+NO3^-(aq)
b. acid, NH4^+(aq)<->2H^+(aq)+NH3(aq)
c. base, 3KOH(aq)->K^+(aq)+OH^-(aq)
d.base HC2H3O2(aq)<->H^+(aq)+C2H3O2^-(aq)
a. acid, HNO3(aq)->H^+(aq)+NO3^-(aq)
b. base, NH4^+(aq)<->H^+(aq)+NH3(aq)
c. acid, KOH(aq)->K^+(aq)+OH^-(aq)
d.acid, HC2H3O2(aq)<->H^+(aq)+C2H3O2^-(aq)
a. A=H2CO3, B=H2O, CA=H3O, CB=HCO3
b. A=H2O, B=NH3, CA=NH4, CB=OH
c. A=HNO3, B=H2O, CA=H3O, CB=NO3
d. A=H2O, B=C2H5N, CA=C2H5NH, CB=OH
a. A=H2O, B=C2H5N, CA=C2H5NH, CB=OH
b. A=H2O, B=NH3, CA=NH4, CB=OH
c. A=HNO3, B=H2O, CA=H3O, CB=NO3
d. A=H2CO3, B=H2O, CA=H3O, CB=HCO3
A. HSO4^-
B.HClO4
C.HCO2
D. NH4
A. HSO5
B.HClO3
C.H2CO3
D. NH4^+
A. HSO4^-
B.HClO4
C.H2CO3
D. NH4^+
c,a,b
c,b,a
a,b,c
c,a,b
HClO>HF>HCl>HC6H5O
HC6H5O>HClO>HF>HCl
HCl>HF>HClO>HC6H5O
a. CN^-
b. CIO^-
c. H2O
a. ClO2^-
b.ClO4^-
c.Br^-
a.CN^-
b.ClO4^-
c.H2O
a. 6.7 x10^-12 M, basic
b. 2.9x10^-6 M, acidic
c. 1.2x10^-4 M, acidic
a. 67.6 x10^-12 M, acidic
b. 9.2x10^-6 M, basic
c. 2.1x10^-4 M, basic
a. 6.7 x10^-12 M, acidic
b. 2.9x10^-6 M, basic
c. 1.2x10^-4 M, basic
a. 67.6 x10^-12 M, basic
b. 9.2x10^-6 M, acidic
c. 2.1x10^-4 M, acidic
a. 9.1x10^-12 M, basic
b. 1.1x10^-6 M, acidic
c. 4.2x10^-13 M, basic
a. 1.9x10^-12 M, basic
b. 1.1x10^-6 M, acidic
c. 2.4x10^-13 M, basic
a. 9.1x10^-12 M, acidic
b. 1.1x10^-6 M, basic
c. 4.2x10^-13 M, acidic
a. 1.9x10^-12 M, acidic
b. 1.1x10^-6 M, basic
c. 2.4x10^-13 M, acidic
a. pH= 7.77, pOH=6.23
b. pH=7.00, pOH=7.00
c. pH=5.66, pOH= 8.34
a. pH= 6.23, pOH=7.77
b. pH=7.00, pOH=7.00
c. pH=8.34, pOH= 5.66,
a. [H30^+]=2.8x10^-9 M, [OH^-]=3.6x10^-6 M
b. [H30^+]=5.9x10^-12 M, [OH^-]=1.7x10^-3 M
c. [H30^+]=1.3x10^-3 M, [OH^-]=7.7x10^-12 M
a. [H30^+]=1.3x10^-3 M, [OH^-]=7.7x10^-12 M
b. [H30^+]=5.9x10^-12 M, [OH^-]=1.7x10^-3 M
c.[H30^+]=2.8x10^-9 M, [OH^-]=3.6x10^-6 M
7.1x10^-4, 1.4x10^-11, basic
2.7x10^-6, 8.43, acidic
7.9x10^-12, 1.3x10^-3, acidic
6.3x10^-4, 3.20, basic
9.1x10^-4, 1.4x10^-11, acidic
7.7x10^-6, 8.43, basic
3.9x10^-12, 1.3x10^-3, basic
2.3x10^-4, 3.20, acidic
9.1x10^-4, 1.4x10^-11, basic
7.7x10^-6, 8.43, acidic
3.9x10^-12, 1.3x10^-3, acidic
2.3x10^-4, 3.20, basic
7.1x10^-4, 1.4x10^-11, acidic
2.7x10^-6, 8.43, basic
7.9x10^-12, 1.3x10^-3, basic
6.3x10^-4, 3.20, acidic
a
b
c
d
a.7.86
b.5.67
a. 9.39
b. 3.96
a. 7.60
b. 11.18
c. 4.61
a. 9.43
b. 13.82
c. 7.61
a. 3.60
b. 81.18
c. 0.61
a. 4.63
b. 7.45
a. 3.86
b. 8.95
a. 4.74
b. 4.68
c. 4.81
a. 7.74
b. 7.68
c. 7.81
a. 5.74
b. 5.68
c. 5.81
a. initial=8.00, final=3.40
b. initial=1.74, final=9.56
c. initial=14.78, final=17.66
a. initial=7.00, final=1.70
b. initial=4.71, final=4.56
c. initial=10.78, final=10.66
a. no
b. yes
c. yes
d. yes
a. yes
b. yes
c. yes
d. yes
a. yes
b. no
c. no
d. no
a. 7.4
b. 0.3 g
c. 0.14 g
a. 9.4
b. 0.45 g
c. 0.24 g
a
b
c
i:
a. pH=8
b. pH=7
ii:
a. a weak acid
b. a strong acid
i:
a. pH=6
b. pH=7
ii:
a. a weak acid
b. a strong acid
i:
a. pH=8
b. pH=7
ii:
a. a srtongacid
b. a weak acid
a. 40 mL HI for both
b. KOH is neutral, CH3NH2 is acidic
c.CH3NH2
a. 50 mL HI for both
b. KOH is neutral, CH3NH2 is basic
c.HI
a. 12.06
b. 29.8 mL
c. 11.90
d. 8
e. 1.07
a. 13.06
b. 28.8 mL
c. 12.90
d. 7
e. 2.07
a. 11.94
b. 29.2 mL
c. 11.33
d. 10.64
e. 5.87
f. 1.90
a. 1.94
b. 29.2 mL
c. 19.33
d. 13.64
e. 3.87
f. 2.90
a. 13.94
b. 19.2 mL
c. 15.33
d. 12.64
e. 7.87
f. 3.90
i: a
ii: a
i: a
ii: b
i: b
ii: a
i: b
ii: b
First equivalence: 22.7 mL
Second equivalence: 45.4 mL
First equivalence: 12.7 mL
Second equivalence: 55.4 mL
First equivalence: 7.9 mL
Second equivalence: 35.4 mL
a. 5.31x10^-7 M
b.
2.72x10^-5 M
c. 1.32x10^-4 M
a. 7.31x10^-7 M
b.
3.72x10^-5 M
c. 3.32x10^-4 M
a. 9.31x10^-7 M
b.
4.72x10^-5 M
c. 5.32x10^-4 M
a. 1.07x10^-21
b. 7.14x10^-7
c. 7.44x10^-11
a. 3.07x10^-21
b. 2.14x10^-7
c. 4.44x10^-11
a. 2.07x10^-21
b. 8.14x10^-7
c. 6.44x10^-11
a. 7.07x10^-21
b. 1.14x10^-7
c. 2.44x10^-11
a. 2.86
b. 16.8 mL
c. 4.37
d. 4.74
e. 8.75
f. 12.17
a. 3.86
b. 17.8 mL
c. 5.37
d. 3.74
e. 8.75
f. 2.17
AX2
AX
2.07x10^-5 g/100mL
3.07x10^-5 g/100mL
4.07x10^-5 g/100mL
5.07x10^-5 g/100mL
a. 0.0183 M
b. 0.00755 M
c. 0.00109 M
a. 0.0283 M
b. 0.00855 M
c. 0.00309 M
a. 5x10^8 M
b. 5x10^4 M
c. 5x10^14 M
a. 5x10^14 M
b. 5x10^8 M
c. 5x10^4 M
8.7x10^-8 M
6.7x10^-10 M
8.7x10^-10 M
6.7x10^-8 M
5.6x10^16
4.6x10^16
4.6x10^14
5.6x10^14
do a and b only
a. [H30^+]=0.35 M
b. [OH^-]=5.0x10^-14 M, pH=0.60
c. [H3O^+]=0.025 M, [OH^-]=8.7x10^-13 M, pH=1.82
a. [H30^+]=0.25 M
b. [OH^-]=4.0x10^-14 M, pH=0.60
c. [H3O^+]=0.015 M, [OH^-]=6.7x10^-13 M, pH=1.82
a. 1.8 g
b. 0.57 g
c. 0.045 g
a. 2.8 g
b. 0.37 g
c. 0.085 g
a. 1.8 g
b. 0.63 g
c. 0.045 g
2.55
1.63
4.78
3.47
pH= 3.44
pH=4.83
pH= 2.44
pH=1.32
a. 3.82 (approximation valid)
b. 5.18 (approximation breaks down)
c. 3.72 (approximation breaks down)
a. 3.82 (approximation breaks down)
b. 5.18 (approximation breaks down)
c. 3.72 (approximation breaks down)
a. 1.82 (approximation valid)
b. 2.18 (approximation breaks down)
c. 2.72 (approximation breaks down)
a. 1.82 (approximation valid)
b. 2.18 (approximation valid)
c. 2.72 (approximation breaks down)
3.42
2.64
6.83
4.57
7.8x10^-4
6.8x10^-4
7.8x10^-6
6.8x10^-6
0.0070%
0.673%
1.00%
0.0012%
2.65x10^-3
1.65x10^-2
3.61x10^-5
a. pH= 1.88, percent ionization= 5.1%
b. pH= 2.10, percent ionization= 7.9%
c. pH= 2.26, percent ionization= 11%
a. pH= 2.78, percent ionization= 7.1%
b. pH= 3.10, percent ionization= 7.9%
c. pH= 5.26, percent ionization= 23%
a. pH= 7.88, percent ionization= 9.1%
b. pH= 8.10, percent ionization= 1.9%
c. pH= 2.26, percent ionization= 1%
a. 0.943
b. 6.53
c. 1.78
d. 1.03
a. 0.743
b. 2.53
c. 1.45
d. 7.03
a. 0.939
b. 1.07
c. 2.19
d. 3.02
no equations
a. basic
b. neutral
c. neutral
d. basic
a. neutral
b. basic
c. basic
d. basic
a. neutral
b. basic
c. basic
d. neutral
[OH^-]= 1.4x10^-6 M, pH=8.16
[OH^-]= 1.4x10^-4 M, pH=5.16
[OH^-]= 1.4x10^-2 M, pH=3.16
no equations
a. neutral
b. neutral
c. acidic
d. acidic
a. acidic
b. neutral
c. acidic
d. acidic
a. neutral
b. acidic
c. neutral
d. neutra;
a. basic
b. neutral
c. acidic
d. acidic
e. neutral
a. acidic
b. basic
c. neutral
d. acidic
e. acidic
NH4Cl,NH4ClO2, NaCl, NaHCO3, NaOH
NaHCO3, NaCl, NaOH, NH4ClO2, NH4Cl
NaOH, NaHCO3, NaCl, NH4ClO2, NH4Cl
a. 5.13
b. 8.87
c. 7.0
a. 6.24
b. 7.23
c. 5.7
a. 4.34
b. 6.72
c. 3.0
[K+]= 0.35 M, [F-]= 0.25 M, [HF]= 1.7x10^-4 M, [OH-]= 1.5x10^-2 M, [H30+]= 3.5x10^-7 M
[K+]= 0.15 M, [F-]= 0.15 M, [HF]= 1.5x10^-6 M, [OH-]= 1.5x10^-6 M, [H30+]= 6.7x10^-9 M
a. [H3O+]= 0.048 M, pH= 1.32
b. [H3O+]= 0.12 M, pH= 0.92
a. [H3O+]= 0.073 M, pH= 4.56
b. [H3O+]= 0.27 M, pH= 0.34
a. [H3O+]= 0.035 M, pH= 5.97
b. [H3O+]= 0.98 M, pH= 0.69
a. [H3O+]= 0.023 M, pH= 3.49
b. [H3O+]= 0.93 M, pH= 0.12
[H2SO3] = 0.418 M
[HSO3-]= 0.082 M
[SO3^2-] = 6.4x10^-8 M
[H30+]= 0.082 M
[H2SO3] = 0.673 M
[HSO3-]= 0.065 M
[SO3^2-] = 3.4x10^-2 M
[H30+]= 0.092 M
[H2SO3] = 0.118 M
[HSO3-]= 0.042 M
[SO3^2-] = 1.4x10^-8 M
[H30+]= 0.032 M
a. [H30+]= 0.50 M, pH= 0.30
b. [H30+]= 0.11 M, pH= 0.96
c. [H30+]= 0.059 M, pH= 1.23
a. [H30+]= 0.70 M, pH= 0.10
b. [H30+]= 0.33 M, pH= 0.78
c. [H30+]= 0.043 M, pH= 5.29
a. [H30+]= 0.40 M, pH= 0.20
b. [H30+]= 0.22 M, pH= 0.87
c. [H30+]= 0.042 M, pH= 2.57
a. HF, stronger bond
b. H2O, no bond polarity
c. H2S, stronger bond
a. HCl, weaker bond
b. HF, bond polarity
c. H2Se, weaker bond
a. HF, weaker bond
b. H2O, bond polarity
c. H2S, weaker bond
a. HCl, stronger bond
b. HF, no bond polarity
c. H2Se, stronger bond
a. H2SO4, more oxygen atoms bonded to S
b. HClO2, more oxygen atoms bonded to Cl
c. HClO, Cl has higher electronegativity
d. CCl3COOH, Cl has higher electronegativity
a. H2SO3, more oxygen atoms bonded to S
b. HClO, more oxygen atoms bonded to Cl
c. HBrO, Cl has higher electronegativity
d. CH3COOH, Cl has higher electronegativity
S^2-, its conjugate acid is weaker than the others conjugate acid
Se^2-, its conjugate acid is weaker than the others conjugate acid
S^2-, its conjugate acid is stronger than the others conjugate acid
Se^2-, its conjugate acid is stronger than the others conjugate acid
a. Lewis base
b. Lewis base
c. Lewis acid
d. Lewis acid
a. Lewis acid
b. Lewis acid
c. Lewis base
d. Lewis base
a. acid: H2O, base: Fe3+
b. acid: NH3, base: Zn^2+
c. acid: (CH3)3N, base: BF3
a. acid: Fe3+, base: H2O
b. acid: Zn^2+, base: NH3
c. acid: BF3, base: (CH3)3N
