Name__________________
Questions
1.
Date____________
7.
Based on the above information, what is the pH of a HCO3–(aq) solution closest to if the reaction container
starts out with 0.01 M HCO3– .
1) 5
2) 6
3) 7
4) 8
5) 9
2. If 50 mL of 0.025 M NaOH is mixed with 50 mL of 0.05 M HCl, what is the resulting pH of the mixture
closest to?
1) 1
2) 2
3) 3
4) 4
5) 5
3. What is the pH of a 0.1 M solution of ammonium
chloride closest to if Ka is 5.56 × 10–10 ?
1) 3
2) 4
3) 5
4) 6
5) 7
4.
Given the above K w values, Which is true about
hydronium and hydroxide ion concentrations when water
is heated?
1)
2)
3)
4)
5)
[H3O+ ] and [OH–] both remain the same
[H3O+ ] and [OH–] both decrease
[H3O+ ] increases and [OH –] decreases
[H3O+ ] decreases and [OH –] increases
[H3O+ ] and [OH–] both increase
5.
Based on the table above, which acid–base indicator has
a transition point between pH 7 and pH 9 ?
1) alizarin blue
3) cresol red
5) none of these
2) congo red
4) ethyl red
8. Which two compounds would serve well as a buffer?
1)
2)
3)
4)
5)
HC 2H3O2 and C2H3O2–
HBr and NaOH
HCl and ClO –
HCHO 2 and HF
OH – and H2O
9. CH 3COOH + H2O « CH 3COO– +H3O+
In the reaction above, a small amount of acid is added to
a buffer solution at equilibrium. When equilibrium is
reestablished,
1)
2)
3)
4)
5)
[CH3COO–] and pH are both higher
[CH3COOH] and pH are both lower
[CH3COO–] is lower and pH is about the same
[CH3COOH] is lower and pH is about the same
[CH3COO–] and pH are both about the same
10. A solution of CH3COOH is neutralized by KOH in the
titration curve above.
A few drops of the indicator chlorophenol red are added
to a colorless solution of pH 4.0.Based on the above
reading, what is the color and explanation for the
resulting solution?
1)
2)
3)
4)
5)
Red as [HCph ] < [Cph –]
Red as [HCph ] > [Cph –]
Yellow as [HCph] < [Cph –]
Yellow as [HCph] = [Cph –]
Yellow as [HCph] > [Cph –]
6. Which will produce a buffer solution when added to 1.0 M NH 3?
1) HNO3
3) NaOH
5) K3PO 4
2) KNH2
4) NH 4Cl
The solution is buffered
1) at point I
3) at point III
5) after point IV
2) at point II
4) at point IV
11. How much 2.50 M H2SO 4 is needed to titrate 25.0 mL
of 1.50 M Ca(OH) 2?
1) 5.00 mL
3) 15.0 mL
5) 30.0 mL
2) 7.50 mL
4) 25.0 mL
Questions
12. The solubility product constant, K sp for silver bromide,
AgBr, is 5.3 × 10 –13 at room temperature. When equal
volumes of 2.0 × 10–3 M AgNO3 and 2.0 × 10 –3 M
NaBr are mixed at room temperature, the mixing
produces
1)
2)
3)
4)
5)
no visible precipitate
a visible precipitate of AgBr
a visible precipitate of NaNO 3
a visible precipitate of AgNO 3
a visbile precipitate of NaBr
13. HI(aq) + F – (aq) « I–(aq) + HF(aq)
The reaction above has a large K eq. What can be
concluded from this statement?
1)
2)
3)
4)
HI(aq) is a weaker acid that HF(aq).
The conjugate base of HF(aq) is HI(aq).
F–(aq) is a stronger base than I–(aq).
The equilibrium constant will increase with
increased temperature.
5) Equimolar concentrations of HI(aq) and HF(aq)
have a pH of 7.0.
16. In the reaction:
NH 3(aq) + H2PO 4–(aq) « NH4+(aq) + HPO42–(aq) the dihydrogen phosphate ion, H 2PO 4–, acts as
1) an acid
3) a catalyst
5) a reducing agent
2) a base
4) an oxidizing agent
17. Base your answer to the following question on the
elements below.
(A) Chlorine
(B) Silicon
(C) Lead
(D) Lithium (E) Silver
An oxide of this element reacts with water to form
strong acid
1) A
2) B
3) C
4) D
5) E
Base your answers to questions 18 through 21 on the
titration diagram below.
14. Based on the above table, list the acids in order of increasing acid strength.
18. The pH of the solution is equal to the pKa of the acid.
1)
2)
3)
4)
5)
CH 3COOH, NH 4+ , HIO 3
HIO 3, CH 3COOH, NH 4+
HIO 3, HIO 3, CH 3COOH
NH 4+ , HIO 3, CH 3COOH
NH 4+ , CH 3COOH, HIO3
15. HF(aq) + NH 3(aq) « NH 4+ (aq) + F –(aq)
Which statement is true about the equilibrium reaction
above?
1) The reactants are favored because NH4+ and HF
are acids of equal strength.
2) The products are favored because NH 4+ is a
stronger acid than HF.
3) The reactants are favored because HF is a stronger
acid than NH 4+ .
4) The reactants are favored because NH4+ is a
stronger acid than HF.
5) The products are favored because HF is a stronger
acid than NH 4+ .
1) I
3) III
5) II and IV
2) II
4) IV
19. This is when there is excess base.
1) I
3) III
5) II and IV
2) II
4) IV
20. At this point the solution is buffered.
1) I
3) III
5) II and IV
2) II
4) IV
21. This point is the equivalence point.
1) I
3) III
5) I and III
2) II
4) IV
Questions
22.
25. A 0.985 g sample of impure solid NaOH is neutralized
by 43.2 mL of 0.275 M HCl solution. What is the
percent, by mass, NaOH in the sample?
1) 1.21% 2) 2.42% 3) 27.9% 4) 48.2% 5) 12.1%
26.
Which indicator would be best suited for this titration?
1)
2)
3)
4)
5)
Methyl violet
Alizarin yellow
Thymolphthalein
Bromocresol green
All the indicators are equally suited for this
titration.
23.
Ksp = 1.10 ×10–36 for Fe(OH)3 Ksp = 3.70 ×10–15 for
Al(OH)3
A 100. mL is 0.10 M with respect to Fe(NO 3) 3 and 0.10
M with respect to Al(NO 3) 3. If 0.10 M KOH is added
to the solution in drops until a precipitation occurs,
which of the following will occur?
1) Ferric hydroxide will be the only precipitate.
2) Aluminum hydroxide will be the only precipitate.
3) Aluminum and ferric hydroxide will both be
precipitated.
4) Potassium nitrate and ferric hydroxide will be
precipitated.
5) Potassium nitrate and aluminum hydroxide will be
precipitated.
27. A student mixes 200. mL of 0.50 M strontium nitrate (
aq) with 300. mL of 0.25 M potassium nitrate (aq).
What is the final concentration of Sr2+ ions in solution?
1) 0.40 M
3) 0.25 M
5) 0.13 M
Which titration is represented by the above graph?
1)
2)
3)
4)
5)
Adding a weak acid to a strong base
Adding a weak base to a strong acid
Adding a weak base to a strong acid
Adding a strong acid to a strong base
Adding a strong acid to a neutral solution
24. Which titration curve represents the titration of HCl
with NaOH?
1)
2)
3)
4)
2) 0.05 M
4) 0.20 M