1. Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of
Mg(OH)2 is
2.7 × 10-12
1.1 × 10-11
2.0 × 10-8
3.9 × 10-8
1.4 × 10-4 Question 2
1. Of the substances below, ________ will decrease the solubility of Pb(CN)2 in a saturated
solution.
Pb(MnO4)2
NaMnO4
HMnO4
H2O2
NaCl Question 3 1. Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid
(C7H5O2H) and of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 4.409 3.965 10.035 9.591 5.190 Question 4
1. In which of the following aqueous solutions would you expect AgI to have the highest
solubility?
pure water 0.050 M BaI2
0.050 M NaI 0.050 M KI 0.010 M AgNO3 Question 5
1. In which of the following aqueous solutions would you expect AgBr to have the lowest
solubility?
0.040 M SrBr2
pure water 0.040 M NaBr 0.040 M KBr 0.010 M AgNO3 Question 6
1. The pH of a solution prepared by dissolving 0.350 mol of solid methylamine
hydrochloride (CH3NH3Cl) in 1.00L of 1.10mol methylamine (CH3NH2) is ________.
The Kb for methylamine is
1.66 2.86 10.28 (Assume the final volume is 1.00 L.) 11.14 10.61 Question 7
1. Which one of the following pairs cannot be mixed together to form a buffer solution?
C5H5N, C5H5NHCl
HC2H3O2, NaOH (C2H3O2- = acetate)
KOH, HI NH2CH3, HCl
NaClO, HNO3 Question 8
1. A solution containing which one of the following pairs of substances will be a buffer
solution?
KI, HI AgBr, HBr CuCl, HCl CsI, HI None of these Question 9
1. Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.300mol of
in water sufficient to yield 1.00 L of solution.
The Kb of ammonia is 5.204 4.300 9.700 8.781 8.796 Question 10 1. The solubility of manganese (II) hydroxide (Mn(OH)2) is
Mn(OH)2? What is the Ksp of 1.1 × 10-14
4.3 × 10-14
2.1 × 10-14
4.8 × 10-10
2.2 × 10-5 Question 11
1. Of the following solutions, which has the greatest buffering capacity?
1.15 M HF and 0.624 M NaF 0.574 M HF and 0.312 M NaF 0.287 M HF and 0.156 M NaF 0.189 M HF and 0.103 M NaF They are all buffer solutions and would all have the same capacity. Question 12 A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH
solution. The titration curve above was obtained. Which of the following indicators
would be best for this titration?
methyl red bromthymol blue thymol blue phenolpthalein bromocresol purple Question 13
1. The primary buffer system that controls the pH of the blood is the ________ buffer
system.
carbon dioxide, carbonate carbonate, bicarbonate carbonic acid, carbon dioxide carbonate, carbonic acid carbonic acid, bicarbonate Question 14 A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution.
The titration curve above was obtained. The concentration of the monoprotic acid is about
________ mol/L.
25.0 0.0600 0.240 0.120 0.100 Question 15
1. The Henderson-Hasselbalch equation is ________. Question 16
1. In which of the following aqueous solutions would you expect AgF to have the highest
solubility?
0.00750 M LiF 0.030 M AgNO3
0.023 M NaF 0.015 M KF AgF will have the same solubility in all solutions. Question 17
1. Of the following solutions, which has the greatest buffering capacity?
0.543 M NH3 and 0.555 M NH4Cl
0.087 M NH3 and 0.088 M NH4Cl
0.234 M NH3 and 0.100 M NH4Cl
0.100 M NH3 and 0.455 M NH4Cl They are all buffer solutions and would all have the same capacity. Question 18
1. How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M
hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 × 10-8.
7.60 50.0 41.6 60.1 7.35 Question 19
1. What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer
system in the blood?
kidneys, liver lungs, kidneys spleen, liver lungs, skin brain stem, heart Question 20
1. Which one of the following will cause hemoglobin to release oxygen?
increase in pH decrease in pH decrease in temperature decrease in CO2 concentration
increase in O2 concentration

 

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