aqueous equilibrium - manchester high school question… · 5 dec 133:02 am 8 a buffer at a ph...
TRANSCRIPT
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Apr 276:18 PM
Aqueous Equilibrium
Grade:«grade»Subject:AP Chemistry
Date:«date»
Dec 133:02 AM
AB
CD
E
1 At this point in the titration, the pH of the solution is equal to the pKa of the acid.
A A
B B
C C
D D
E E
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2 This is the equivalence point of the titration.
A A
B B
C C
D D
E E
AB
CD
E
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3 At this point the solution is buffered.
A A
B B
C C
D D
E E
AB
CD
E
3
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4 The concentrations of which of the following species will be increased when HCl is added to a solution of HC2H3O2 in water?
A I only
B I and II only
C I and III only
D II and III only
E I, II, and III
I. H+
II. C2H3O2
III. HC2H3O2
Dec 133:02 AM
5 Which of the following procedures will produce a buffered solution?
A I only
B III only
C I and II only
D II and III only
E I, II, and III
I. Equal volumes of 0.5 M NaOH and 1 M HCl solutions are mixed.
II. Equal volumes of 0.5M NaOH and 1 M HC2H3O2 solutions are mixed.
III. Equal volumes of 1 M NaC2H3O2 and HC2H3O2 solutions are mixed.
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6 The solution with the lowest pH.
A NH3 and NH4Cl
B H3PO4 and NaH2PO4
C HCl and NaCl
D NaOH and NH3
E NH3 and HC2H3O2
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7 The most nearly neutral solution.
A NH3 and NH4Cl
B H3PO4 and NaH2PO4
C HCl and NaCl
D NaOH and NH3
E NH3 and HC2H3O2
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8 A buffer at a pH >8.
A NH3 and NH4Cl
B H3PO4 and NaH2PO4
C HCl and NaCl
D NaOH and NH3
E NH3 and HC2H3O2
Dec 133:02 AM
9 Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present?
A 1.60 M
B 0.800 M
C 0.640 M
D 0.600 M
E 0.400 M
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10 The solubility of PbS in water is 3 x 1014 M. What is the solubility product constant, Ksp, for PbS?
A 2 x 107
B 9 x 107
C 3 x 1014
D 3 x 1028
E 9 x 1028
Dec 133:02 AM
11 Temperature is often given with Ksp values because
A the solubilty of solids aways increases with increasing temperature.
B the solubility of solids varies with temperature changes.
C solubility changes with temperature but Ksp values do not.
D Ksp varies with temperature even though concentrations do not.
E the number of ions varies with the kind of salt that is dissolving.
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12 The Ksp expression for silver phosphate is
A Ksp = [3Ag+][PO43]
B Ksp = [3Ag+]3[PO43]
C Ksp = [Ag+]3[PO43]
D Ksp = [Ag+][PO43]3
E Ksp = [Ag+][PO43]
Dec 133:02 AM
13 What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 x 1012.)
A 8 x 1012 M
B 2 x 1012 M
C (4 x 1012 M)1/2
D (4 x 1012 M)1/3
E (2 x 1012 M)1/3
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14 Which of the following compounds is the most soluble (in moles/liter?)
A BaSO4
B CoS
C PbSO4
D AgBr
E BaCO3
BaSO4 1.5 x 109CoS 5.0 x 1022PbSO4 1.3 x 108AgBr 5.0 x 1013BaCO3 1.6 x 109
Ksp
Dec 133:02 AM
15 Lead Iodide has a Ksp value of 1.08 x 107 at 20oC. Calculate the molar solubilty.
A 5.00 x 108
B 3.00 x 106
C 1.00 x 104
D 6.00 x 103
E 3.00 x 103
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16 Will a precipitate form when 75.0 mL of 0.050 M ZnCrO4 is mixed with 75.0 mL of 0.10 M Ca(NO3)2?Ksp for CaCrO4 is 7.1 x 104.
A Yes, a precipitate will form, Q>Ksp
B Yes, a precipitate will form, Q<Ksp
C Yes, a precipitate will form, Q=Ksp
D No, a precipitate will not form, Q>Ksp
E No, a precipitate will not form, Q<Ksp
Apr 276:19 PM
Answers:1. B2. D3. B4. C5. D6. C7. E8. A9. B10. E11. B12.C13.E14. C15. E16. A