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CHM 142 Exam 4 Review questions and answers 100% complete solution 2024/2025
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CHM 142 Exam 4 Review questions and answers 100% complete solution 2024/2025
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CHM 142 Exam 4 ReviewWhich of the following titrations will result in a noticeably basic solution at the
equivalence point?
KOH(aq) + HI(aq)
HCl(aq) + NaOH(aq)
CH3COOH(aq) + NaOH(aq)
NH3(aq) + HClO4(aq)
NaHCO3(aq) + HCl(aq)
CH3COOH(aq) + NaOH(aq)
Which of the following indicators is suitable for the titration of 0.10 M CH3COOH (Ka =
1.8 x 10-5) with 0.15 M NaOH?
methyl orange (Ka = 2.0 x 10-4)
phenolphthalein (Ka = 4.0 x 10-10)
bromocresol green (Ka = 2.0 x 10-5)
bromothymol blue (Ka = 1.0 x 10-7)
methyl red (Ka = 7.9 x 10-6)
phenolphthalein (Ka = 4.0 x 10-10)e
Calculate the concentration of fluoride ions in a saturated solution of chromium fluoride
(CrF3). Ksp(CrF3) = 6.6 x 10-11
3.9 x 10-3 M
What is the molar solubility of PbBr2 in a 0.15 M solution of KBr? Ksp(PbBr2) = 6.6 x
10-6.
2.9 x 10-4 M
Which of the following salts will not be significantly more soluble in acidic solution than
in pure water?
AgBr
BaCO3
PbF2
ZnS
Ba3(PO4)2
AgBr
In which of the following aqueous solutions would you expect AgBr to have the lowest
solubility?
0.030 M KBr
pure water
0.010 M MgBr2
0.020 M FeBr3
0.020 M AgNO3
0.020 M FeBr3
In which solutions the molar solubility of NiCO3 will be greater than in pure water?
A: 0.010 M Ni(NO3)2
B: 0.010 M NH3
, C: 0.010 M HCl
D: 0.010 M Na2CO3
only B and C
Will a precipitate of Ba(IO3)2 form when 50.0 mL of 4.2 x 10-3 M Ba(NO3)2 solution is
added to 50.0 mL of 2.2 x 10-3 M NaIO3? For Ba(IO3)2, Ksp = 4.0 x 10-9.
No, Qsp < Ksp
Consider a 2.5 x 10-2 M aqueous solution of Pb(NO3)2. What is the minimal
concentration of I- ions required to begin the precipitation of PbI2? Ksp(PbI2) = 9.8 x 10-
9.
6.3 x 10-4 M
Consider a solution in which concentrations of Ca2+, Sr2+ and Ba2+ ions are all 1.00 x
10-4 M. If enough solid Na2SO4 is added to this solution so that the concentration of
SO42- ions is 1.0 x 10-3 M which sulfates(s) will precipitate?
The solubility product constants are:
CaSO4: Ksp = 4.9 x 10-5
SrSO4: Ksp = 3.4 x 10-7
BaSO4: Ksp = 1.1 x 10-10
Only BaSO4 will precipitate.
Find the pKsp for a salt of the AB3 type given that its molar solubility is 7.71 µM.
19.02
Find the molar solubility (in mM) of salt of the A3B2 type given the solubility product
constant: Ksp = 4.74 x 10-13.
1.34
For which of the three phase transitions: deposition, fusion and sublimation is ∆S
negative?
only deposition
Find the molar entropy of vaporization (in J/(K·mol)) for a certain substance given that to
vaporize 0.228 mol of that substance at -43.4 ºC ∆H = 3.94 kJ.
75.2
Find ∆S (in J/K) for a reversible isothermal expansion of 0.618 mol of an ideal gas when
it expands from 2.69 L to 7.03 L at 39.7 ºC.
4.94
For which of the following reactions is ∆Sº negative?
2NO2(g) → 2NO(g) + O2(g)
CH3OH(l) → CH3OH(g)
2H2O2(l) → 2H2O(l) + O2(g)
Br2(l) + H2(g) → 2HBr(g)
Ba2+(aq) + SO42-(aq) → BaSO4(s)
Ba2+(aq) + SO42-(aq) → BaSO4(s)
Arrange the following reactions according to increasing ∆Sº.
1: 2C(s) + O2(g) → 2CO(g)
2: H2O(g) → H2O(l)
3: 2NaHCO3(s) → Na2CO3(s) + H2O(g) + CO2(g)
∆Sº(2) < ∆Sº(1) < ∆Sº(3)
Which of the following species has the highest standard molar entropy (Sº) at 25 ºC?
CaCl2(s)
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