Molecular View Of Reactions In Aqueous | Test Bank Docx Ch.4 - Solution Bank | Chemistry Molecular Nature 8e by Neil D. Jespersen. DOCX document preview.
Chemistry: Molecular Nature of Matter, 8e (Jespersen)
Chapter 4 Molecular View of Reactions in Aqueous Solutions
1) A solute is
A) a solid substance that does not dissolve in water.
B) a solid substance that does not dissolve at a given temperature.
C) a substance containing a solid, liquid, or gas.
D) a substance that is dissolved in a solvent.
E) a liquid that does not dissolve in another liquid.
Diff: 1
Section: 4.1
2) Which of the following describes a saturated solution?
A) one that contains 1 mole of a substance in 100 mL of water
B) one that contains as much solute as it can hold at a given temperature
C) one that contains less solute than it can hold at 25°C
D) one in which the ratio of solute to solvent is small
E) one that is equivalent to a supersaturated solution
Diff: 2
Section: 4.1
3) When a solid forms in a solution, it is called
A) a dilute solution.
B) a solvent.
C) a gaseous mixture.
D) a soluble solid.
E) a precipitate.
Diff: 2
Section: 4.1
4) At room temperature, the solubility of table salt in water is 359 g/L of water. If a solution was prepared at a high temperature with 40 g of table salt in 100 mL of water and then cooled back to room temperature, what would be the best description of the resulting solution assuming that no precipitate was formed?
A) a saturated solution
B) an unsaturated solution
C) a supersaturated solution
D) an incomplete solution
E) a dominate solution
Diff: 2
Section: 4.1
5) At room temperature, the solubility of table salt in water is 359 g/L of water. If a solution was prepared at a high temperature with 20 g of table salt in 100 mL of water and then cooled back to room temperature, what would be the best description of the resulting solution assuming that no precipitate was formed?
A) a saturated solution
B) an unsaturated solution
C) a supersaturated solution
D) an incomplete solution
E) a dominate solution
Diff: 2
Section: 4.1
6) How many ions are produced when C6H12O6 dissolves in water?
A) 0
B) 2
C) 4
D) 6
E) 12
Diff: 1
Section: 4.2
7) Which is a nonelectrolyte?
A) barium nitrate, Ba(NO3)2
B) calcium chloride, CaCl2
C) sodium chloride, NaCl
D) methyl alcohol, CH3OH
E) potassium sulfate, K2SO4
Diff: 2
Section: 4.2
8) Which is a nonelectrolyte?
A) ammonium chloride, NH4Cl
B) ethylene glycol, HOCH2CH2OH
C) nickel(II) sulfate, NiSO4
D) sodium perchlorate, NaClO4
E) zinc nitrate, Zn(NO3)2
Diff: 2
Section: 4.2
9) Which is an electrolyte?
A) glucose, C6H12O6
B) calcium chloride, CaCl2
C) sucrose, C12H22O11
D) acetone, CH3COCH3
E) ethyl alcohol, C2H5OH
Diff: 2
Section: 4.2
10) Which is an electrolyte?
A) fructose, C6H12O6
B) acetone, CH3COCH3
C) ethylene glycol, HOCH2CH2OH
D) methyl alcohol, CH3OH
E) potassium sulfate, K2SO4
Diff: 2
Section: 4.2
11) Which of the aqueous solutions listed conducts electricity well?
A: sodium perchlorate, NaClO4
B: methyl alcohol, CH3OH
C: glucose, C6H12O6
D: calcium chloride, CaCl2
E: nickel(II) sulfate, NiSO4
A) A and E only
B) C, D, and E only
C) A and D only
D) A, D, and E only
E) B, D, and E only
Diff: 2
Section: 4.2
12) Which of the aqueous solutions listed conducts electricity well?
A: acetone, CH3COCH3
B: silver nitrate, AgNO3
C: ethylene glycol, HOCH2CH2OH
D: calcium chloride, CaCl2
E: ammonium bromide, NH4Br
A) A and E only
B) C, D, and E only
C) A and D only
D) A, D, and E only
E) B, D, and E only
Diff: 2
Section: 4.2
13) Which of the aqueous solutions listed does NOT conduct electricity well?
A: sucrose, C12H22O11
B: barium nitrate, Ba(NO3)2
C: ethylene glycol, HOCH2CH2OH
D: calcium bromide, CaBr2
E: ammonium chloride, NH4Cl
A) A and E, only
B) C, D, and E only
C) A and C only
D) A, D, and E only
E) B, D, and E only
Diff: 2
Section: 4.2
14) Which compound produces four ions per formula unit by dissociation when dissolved in water?
A) (NH4)2SO4
B) Hg2Cl2
C) Ca(NO3)2
D) Li3PO4
E) (NH4)4Fe(CN)6
Diff: 1
Section: 4.2
15) Which compound produces four ions per formula unit by dissociation when dissolved in water?
A) K2C2O4
B) Al(NO3)3
C) Hg2(NO3)2
D) NaBrO3
E) Na2S2O3
Diff: 1
Section: 4.2
16) Which compound produces three ions per formula unit by dissociation when dissolved in water?
A) Hg2SO4
B) NaClO2
C) LiClO4
D) KClO
E) (NH4)2SO4
Diff: 1
Section: 4.2
17) How many ions are produced in solution by dissociation of one formula unit of
NiCl2∙6H2O?
A) 2
B) 3
C) 4
D) 6
E) 9
Diff: 2
Section: 4.2
18) How many ions are produced in solution by dissociation of one formula unit of
Co(NO3)2∙6H2O?
A) 2
B) 3
C) 4
D) 6
E) 9
Diff: 2
Section: 4.2
19) Which substance does NOT produce ions when dissolved in water?
A) CH2O
B) KclO
C) Mn(NO3)2
D) CsCN
E) NaHS
Diff: 2
Section: 4.2
20) Which compound produces three ions per formula unit by dissociation when dissolved in water?
A) sodium nitrate
B) nickel(II) sulfate
C) calcium perchlorate
D) aluminum sulfate
E) ammonium bromate
Diff: 2
Section: 4.2
21) In the reaction, K2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2 KNO3(aq), which ions are the spectator ions?
A) Ba2+ and SO42
B) Ba2+ and K+
C) Ba2+ and NO3
D) K+ and SO42
E) K+ and NO3
Diff: 2
Section: 4.3
22) In the reaction, KHS(aq) + HCl(aq) → KCl(aq) + H2S(g), which ions are the spectator ions?
A) K+ and Cl
B) K+ and H+
C) H+ and HS
D) K+ and HS
E) HS and Cl
Diff: 2
Section: 4.3
23) The equation for the reaction, Pb(NO3)2(aq) + NaCl(aq) → PbCl2(s) + NaNO3(aq) can be written as an ionic equation. In the ionic equation, the spectator ions are
A) Na+ and Pb2+.
B) Na+ and Cl-.
C) Pb2+ and Cl.
D) Pb2+ and NO3-.
E) Na+ and NO3.
Diff: 2
Section: 4.3
24) The equation for the reaction, BaCl2(aq) + K2CrO4(aq) BaCrO4(s) + KCl(aq), can be written as an ionic equation. In the ionic equation, the spectator ions are
A) Ba2+ and K+.
B) K+ and CrO42- .
C) K+ and Cl-.
D) B2+ and CrO42-.
E) Cl- and CrO42-.
Diff: 2
Section: 4.3
25) In the reaction between aqueous silver nitrate and aqueous potassium chromate, what is the identity of the soluble substance that is formed?
A) silver chromate
B) silver nitrate
C) potassium chromate
D) potassium nitrate
E) No reaction takes place since all products are soluble.
Diff: 2
Section: 4.3
26) The equation for the reaction, AgNO3(aq) + K2CrO4(aq) Ag2CrO4(s) + KNO3(aq), can be written as an ionic equation. In the ionic equation, the spectator ions are
A) Ag+ and K+.
B) Ag+ and CrO42-.
C) K+ and CrO42-.
D) K+ and NO3-.
E) CrO42- and NO3.
Diff: 2
Section: 4.3
27) What is the formula of the solid that is formed when aqueous barium chloride is mixed with aqueous potassium chromate?
Hint: Make sure you look at the solubility of each compound and determine what the spectator ions are.
A) BaCrO4
B) KCl
C) K2Ba
D) K2CrO4
E) BaCl2
Diff: 3
Section: 4.3
28) Which statement below is true?
Hint: Think about the difference between strong and weak electrolytes when added to water.
A) All acids are strong electrolytes and ionize completely when dissolved in water.
B) All bases are weak electrolytes and ionize completely when dissolved in water.
C) All bases are strong electrolytes and ionize completely when dissolved in water.
D) All salts are strong electrolytes and dissociate completely if they dissolve in water.
E) All salts are weak electrolytes and ionize partially when dissolved in water.
Diff: 3
Section: 4.4
29) According to the Arrhenius theory of acids and bases, acids are substances that
A) exhibit a sour taste.
B) react with all metals to release hydrogen gas.
C) react with all metals to release carbon dioxide gas.
D) produce hydronium ions in water.
E) feel slippery on the skin.
Diff: 1
Section: 4.4
30) Which of the following is a property of bases that is used to classify a substance as an Arrhenius base?
A) They exhibit a sour taste.
B) They produce hydroxide ions in water.
C) They feel slippery to the touch.
D) They produce hydronium ions in water.
E) They exhibit a tart taste.
Diff: 1
Section: 4.4
31) Which species is a weak electrolyte?
A) HClO4
B) HCl
C) NaOH
D) NH3
E) LiOH
Diff: 1
Section: 4.4
32) Which species is a strong electrolyte?
A) HBrO
B) HClO2
C) HF
D) HI
E) H3PO3
Diff: 1
Section: 4.4
33) Which is NOT a strong base?
A) Ca(OH)2
B) Ba(OH)2
C) KOH
D) NaOH
E) NH3
Diff: 1
Section: 4.4
34) Which is NOT a strong acid?
A) HBr
B) HC2H3O2
C) HClO3
D) HClO4
E) HNO3
Diff: 1
Section: 4.4
35) Which is a strong acid?
A) HBrO
B) HClO2
C) HF
D) HI
E) H3PO3
Diff: 1
Section: 4.4
36) Which is NOT a property of strong acids?
A) Strong acids react with all metals to yield CO2 gas.
B) Strong acids exhibit a sour taste.
C) Strong acids turn litmus from blue to red.
D) Strong acids neutralize bases.
E) Strong acids react with carbonate salts to yield CO2 gas.
Diff: 2
Section: 4.4
37) Which one of the equations below represents what happens when HC2H3O2 is dissolved in water?
A) HC2H3O2 + H2O ⇄ H3O+(aq) + C2H3O2+(aq)
B) HC2H3O2 + H2O ⇄ H3O+(aq) + C2H3O2-(aq)
C) HC2H3O2 + H2O ⇄ C2H3O2+ (aq) + OH-(aq)
D) HC2H3O2 + H2O ⇄ H3O-(aq) + C2H3O2+(aq)
E) HC2H3O2 + H2O ⇄ 2 H+(aq) + OH-(aq) + C2H3O2-(aq)
Diff: 2
Section: 4.4
38) Which is NOT acidic?
A) grapefruit juice
B) household ammonia
C) carbonated water
D) vinegar
E) lemon juice
Diff: 1
Section: 4.4
39) Which species is a molecular base?
A) NaOH
B) NH3
C) C2H5OH
D) LiOH
E) NH4+
Diff: 2
Section: 4.4
40) Which one of the equations below represents what happens when NH3 is dissolved in water?
A) NH3 + H2O 
H3O+(aq) + NH3+(aq)
B) NH3 + H2O H3O+(aq) + NH2-(aq)
C) NH3 + H2O NH4+ (aq) + OH-(aq)
D) NH3 + H2O H3O-(aq) + NH2+(aq)
E) NH3 + H2O 2 H+(aq) + OH-(aq) + NH2-(aq)
Diff: 2
Section: 4.4
41) Which is the acid anhydride for HCl?
A) ClO
B) ClO2
C) Cl2O7
D) H2O
E) HCl does not have an anhydride.
Diff: 2
Section: 4.4
42) Which is the acid anhydride for H2CO3?
A) CO
B) CO2
C) C2O4
D) H2O
E) H2CO3 does not have an anhydride.
Diff: 2
Section: 4.4
43) Which is a basic anhydride?
A) SO2
B) CO2
C) O2
D) BaO
E) N2O5
Diff: 2
Section: 4.4
44) The chemical species present in all solutions which are acidic is
A) H2O(aq) .
B) OH(aq) .
C) H2O+(aq) .
D) H3O+(l) .
E) H3O+(aq) .
Diff: 1
Section: 4.4
45) The empirical formula of the acid anhydride of phosphoric acid, H3PO4, is
A) PO2.
B) PO3.
C) P2O3.
D) P2O5.
E) P2O.
Diff: 2
Section: 4.4
46) Which is the acid anhydride for HClO4?
Hint: Remember anhydride means "without water." Think about the chemical formula before water was added.
A) ClO
B) ClO2
C) ClO3
D) ClO4
E) Cl2O7
Diff: 3
Section: 4.4
47) Which substance will ionize when added to water?
Hint: Remember the difference between dissociation and ionization.
A) NaClO4(s)
B) HNO2(aq)
C) C6H12O6(s)
D) (NH4)2SO4(s)
E) Ba(OH)2(s)
Diff: 3
Section: 4.4
48) Which statement below states a fact?
Hint: Remember the difference between dissociation and ionization.
A) All acids are strong electrolytes and dissociate completely when dissolved in water.
B) Some acids are strong electrolytes and ionize completely when dissolved in water.
C) Some acids are strong electrolytes and dissociate completely when dissolved in
water.
D) Some acids are weak electrolytes and ionize completely when dissolved in water.
E) Some acids are weak electrolytes and dissociate partially when dissolved in water.
Diff: 3
Section: 4.4
49) Which is NOT a strong acid?
A) HBr
B) HCl
C) HClO3
D) HF
E) HI
Diff: 1
Section: 4.4
50) Which set below contains only weak electrolytes?
A) HNO3(aq), H2SO4(aq), HCN(aq)
B) KOH(aq), H3PO4(aq), NaClO4(aq)
C) NH3(aq), HC2H3O2(aq), HCN(aq)
D) NH4Cl(aq), HClO2(aq), HCN(aq)
E) NaOH(aq), H2SO4(aq), HC2H3O2(aq)
Diff: 2
Section: 4.4
51) Which solution is the most acidic?
A) 1.0 molar HCN
B) 1.0 molar HC2H3O2
C) 1.0 molar HNO2
D) 1.0 molar HF
E) 1.0 molar HClO3
Diff: 2
Section: 4.4
52) Which set below contains only weak acids?
A) HC2H3O2, HCN, HNO2
B) HC2H3O2, HCN, HNO3
C) HC2H3O2, HCl, HNO2
D) HClO, HCN, HBrO3
E) HNO2, HC2H3O2, HI
Diff: 2
Section: 4.4
53) A dynamic equilibrium is reached when acetic acid is dissolved in water. Which species is present in largest amount in the solution?
Hint: Consider whether acetic acid is a weak or strong electrolyte before determining which species has the highest concentration.
A) C2H3O2(aq)
B) H+(aq)
C) HC2H3O2(aq)
D) H3O+(aq)
E) OH(aq)
Diff: 3
Section: 4.4
54) A dynamic equilibrium is reached when hydrogen fluoride is dissolved in water. Which species is present in the highest concentration in this solution?
Hint: Consider whether hydrogen fluoride is a weak or strong electrolyte before determining which species has the highest concentration.
A) H3O+(aq)
B) HF(aq)
C) H+(aq)
D) F(aq)
E) OH(aq)
Diff: 3
Section: 4.4
55) A dynamic equilibrium is reached when hydrogen cyanide acid is dissolved in water. Which species is present in the highest concentration in this solution?
Hint: Consider whether hydrogen cyanide is a weak or strong electrolyte before determining the highest concentration.
A) C2H3O2(aq)
B) H3O+(aq)
C) OH(aq)
D) HCN(aq)
E) H+(aq)
Diff: 3
Section: 4.4
56) What is the formula of the oxoacid formed from the nitrate ion?
A) H2NO3
B) HNO2
C) HNO3
D) H2NO4
E) HNO
Diff: 2
Section: 4.5
57) What is the name of the oxoacid HBrO4?
A) Bromic acid
B) Hypobromous acid
C) Hydrobromic acid
D) Bromous acid
E) Perbromic acid
Diff: 1
Section: 4.5
58) What is the name of the oxoacid HClO?
A) Chloric acid
B) Hypochlorous acid
C) Hydrochloric acid
D) Chlorous acid
E) Perchloric acid
Diff: 1
Section: 4.5
59) What is the name of the oxoacid HIO2?
A) Iodic acid
B) Hypoiodous acid
C) Hydroiodic acid
D) Iodous acid
E) Periodic acid
Diff: 1
Section: 4.5
60) A student comes across a chemical in the laboratory that is labeled Butylamine. Based on this name, the substance is expected to be
A) an ionic salt.
B) a molecular base.
C) an oxoacid.
D) a binary acid.
E) a strong electrolyte.
Diff: 1
Section: 4.5
61) An example of an acid-base neutralization is the reaction of
A) H2(g) with O2(g) to form H2O(l).
B) H2(aq) with OH(aq) to form H2O(l).
C) H+(aq) with O2(g) to form H2O(l).
D) H+(aq) with OH(aq) to form H2O(l).
E) Na+(aq) with OH(aq) to form NaOH(aq).
Diff: 2
Section: 4.6
62) Which is the net ionic equation for the reaction that takes place when HClO3(aq) is added to KOH(aq)?
A) HClO3(aq) + KOH(aq) → KClO3(aq) + H2O(l)
B) H+(aq) + OH-(aq) → H2O(l)
C) HClO3(aq) + OH-(aq) → ClO3-(aq) + H2O(l)
D) H+(aq) + KOH(aq) → K+(aq) + H2O(l)
E) HClO3(aq) + K+(aq) → KClO3(aq) + H+(aq)
Diff: 2
Section: 4.6
63) Which is the net ionic equation for the reaction that takes place when HNO3(aq) is added to Mg(OH)2(s)?
A) HNO3(aq) + Mg(OH)2(s) → Mg(NO3)2(aq) + H2O(l)
B) H+(aq) + OH-(aq) → H2O(l)
C) HNO3(aq) + OH-(s) → NO3-(aq) + H2O(l)
D) 2H+(aq) + Mg(OH)2(s) → Mg2+(aq) + 2H2O(l)
E) HNO3(aq) + Mg2+(aq) → Mg(NO3)2(aq) + H+(aq)
Diff: 2
Section: 4.6
64) ZnCO3(s) is insoluble in water, but dissolves in excess 6.0 molar HCl(aq). Which equation best describes this reaction?
A) ZnCO3(s) Zn2+(aq) + CO32(aq)
B) ZnCO3(s) + H2O(l) → ZnO(aq) + H2CO3(aq)
C) ZnCO3(s) + 2 H+(aq) → Zn2+(aq) + H2O(l) + CO2(g)
D) ZnCO3(s) + 2 H2O(l) → Zn(OH)2(aq) + H2CO3(aq)
E) ZnCO3(s) + 2 H2O(l) → Zn(OH)2(aq) + H2O(l) +CO2(g)
Diff: 2
Section: 4.6
65) Which statement is NOT correct?
Hint: Remember what the prefixes mean for each type of acid and how those effect salt formation.
A) Acidic salts can be formed by partial neutralization of a monoprotic acid by a monoprotic
base.
B) Acidic salts can be formed by partial neutralization of a diprotic acid by a monoprotic base.
C) Acidic salts can be formed by partial neutralization of a diprotic acid by a diprotic base.
D) Acidic salts can be formed by partial neutralization of a triprotic acid by a diprotic base.
E) Acidic salts can be formed by partial neutralization of a polyprotic acid by a monoprotic base.
Diff: 3
Section: 4.6
66) Complete neutralization of phosphoric acid with barium hydroxide yields Ba3(PO4)2 as one of the products when it is separated and dried. This indicates the phosphoric acid is a
A) monoprotic acid.
B) diprotic acid.
C) triprotic acid.
D) tetraprotic acid.
E) hexaprotic acid.
Diff: 2
Section: 4.6
67) One of the phosphoric acids when fully neutralized by treatment with barium hydroxide yields, as one of its products, a substance with the formula Ba2P2O7. The parent acid for the anion in this compound is a
Hint: Write the reaction and identify the formula of each species to help.
A) monoprotic acid.
B) diprotic acid.
C) triprotic acid.
D) tetraprotic acid.
E) hexaprotic acid.
Diff: 3
Section: 4.6
68) Which reaction will yield NiCr2O7 as one of its products?
Hint: Write each reaction and identify the name of each species present.
A) nickel(II) hydroxide and dichromic acid
B) nickelic acid and chromium(II) hydroxide
C) nickel(II) hydroxide and chromic acid
D) nickel(II) hydroxide and chromate acid
E) nickel(II) hydroxide and bichromic acid
Diff: 3
Section: 4.6
69) What is the net ionic equation for the reaction that takes place when HClO4(aq) is added to NH3(aq)?
Hint: Make sure to cancel out your spectator ions.
A) HClO4(aq) + NH3(aq) → NH4ClO4(aq)
B) H+(aq) + OH-(aq) → H2O(l)
C) HClO4(aq) + OH-(aq) → ClO4-(aq) + H2O(l)
D) H+(aq) + NH3(aq) → NH4+(aq)
E) HClO4(aq) + NH4OH(aq) → H2O(l) + NH4ClO4(aq)
Diff: 3
Section: 4.6
70) What is the net ionic equation for the reaction that takes place when HC2H3O2(aq) is added to Ba(OH)2(aq)?
Hint: Make sure to cancel out your spectator ions.
A) HC2H3O2(aq) + Ba(OH)2(aq) Ba(C2H3O2)2(aq) + H2O(l)
B) H+(aq) + OH-(aq) → H2O(l)
C) HC2H3O2(aq) + OH-(aq) → C2H3O2-(aq) + H2O(l)
D) H+(aq) + Ba(OH)2(aq) → Ba2+(aq) + H2O(l)
E) HC2H3O2(aq) + Ba2+(aq) → Ba(C2H3O2)2(aq) + H+(aq)
Diff: 3
Section: 4.6
71) What is the net ionic equation for the reaction that takes place when HC2H3O2(aq) is added to NH3(aq)?
Hint: Make sure to cancel out your spectator ions.
A) HC2H3O2(aq) + NH3(aq) → NH4+(aq) + C2H3O2-(aq)
B) H+(aq) + OH-(aq) → H2O(l)
C) HC2H3O2(aq) + OH-(aq) → C2H3O2-(aq) + H2O(l)
D) H+(aq) + NH4OH(aq) → NH4+(aq) + H2O(l)
E) HC2H3O2(aq) + NH4OH(aq) → H2O(l) + NH4ClO4(aq)
Diff: 3
Section: 4.6
72) What is the net ionic equation for the reaction that takes place when HNO3(aq) is added to Fe2O3(s)?
Hint: Make sure to cancel out your spectator ions.
A) HNO3(aq) + Fe2O3(s) → Fe(NO3)3(aq) + H2O(l)
B) H+(aq) + OH-(aq) → H2O(l)
C) HNO3(aq) + OH-(s) → NO3-(aq) + H2O(l)
D) 6H+(aq) + Fe2O3(s) → 2Fe3+(aq) + 3H2O(l)
E) HNO3(aq) + Fe3+(aq) → Fe(NO3)3(aq) + H+(aq)
Diff: 3
Section: 4.6
73) What is the net ionic equation for the reaction that takes place when HCl(aq) is added to CaCO3(s)?
Hint: Make sure to cancel out your spectator ions.
A) HCl(aq) + CaCO3(s) → CaCl2(aq) + CO2(g) + H2O(l)
B) 2H+(aq) + CaCO3(s) → Ca2+(aq) + CO2(g) + H2O(l)
C) HCl(aq) + CO32-(aq) → Cl-(aq) + H2O(l) + CO2(g)
D) Cl-(aq) + CaCO3(s) → CaCl2(aq) + CO32-(aq)
E) HCl(aq) + CaCO3(s) → Ca2+(aq) + Cl2(g) + CO2(g) + H2O(l)
Diff: 3
Section: 4.6
74) What is the net ionic equation for the reaction that takes place when Ba(OH)2(aq) is added to NH4Cl(aq)?
Hint: Make sure to cancel out your spectator ions.
A) NH4+(aq) + OH-(aq) → NH3(aq) + H2O(l)
B) NH4+(aq) + Ba(OH)2(aq) → Ba2+(aq) + NH3(aq) + H2O(l)
C) NH4Cl(aq) + OH-(aq) → NH3(aq) + H2O(l) + Cl-(aq)
D) H+(aq) + Cl-(aq) → HCl(aq)
E) Ba(OH)2(aq) + NH4Cl(aq) → BaCl2(aq) + NH4OH(aq)
Diff: 3
Section: 4.6
75) Which one of the following is NOT an example of an acidic salt?
A) aluminum bicarbonate
B) barium dihydrogen phosphate
C) nickel(II) bichromate
D) potassium hydrogen chloride
E) sodium hydrogen sulfate
Diff: 2
Section: 4.6
76) Which is NOT an example of an acidic salt?
A) ammonium dihydrogen arsenate
B) barium bicarbonate
C) chromium(III) hydrogen sulfate
D) cobalt(II) hydrogen acetate
E) nickel(II) bichromate
Diff: 2
Section: 4.6
77) The reaction, BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2 HCl(aq), is an example of a
A) metathesis reaction.
B) neutralization reaction.
C) precipitation reaction.
D) redox reaction.
E) A and C
Diff: 2
Section: 4.6
78) Which compound is insoluble in water?
A) KNO3
B) Pb(NO3)2
C) Na2SO4
D) PbSO4
E) MgCl2
Diff: 1
Section: 4.6
79) Which compound is insoluble in water?
A) Na2CO3
B) NH4NO3
C) CaCO3
D) CaCl2
E) LiClO4
Diff: 1
Section: 4.6
80) Which compound is soluble in water?
A) PbCO3
B) AgBr
C) CaCO3
D) MgCl2
E) BaSO4
Diff: 1
Section: 4.6
81) Which compound is soluble in water?
A) NiCO3
B) PbSO4
C) BaCl2
D) AgCl
E) Fe(OH)3
Diff: 1
Section: 4.6
82) What is the net ionic equation for the reaction between HCl and NaHCO3?
Hint: Cancel out your spectator ions.
A) H2CO3(aq) → H2O + CO2(g)
B) HCl(aq) + HCO3-(aq) → H2O + CO2(g)
C) H+(aq) + HCO3-(aq) → H2O + CO2(g)
D) H2O + CO2(g) → H+(aq) + HCO3-(aq)
E) H+(aq) + NaHCO3(aq) → Na+(aq) + H2O + CO2(g)
Diff: 3
Section: 4.6
83) Which compound is soluble in water?
A) PbCl2
B) Ba(NO3)2
C) Ag2CO3
D) Fe(OH)3
E) Ag3PO4
Diff: 2
Section: 4.6
84) Which of the following is an example of a precipitation reaction?
Hint: Remember to consider the solubility rules and apply them to the products of each reaction.
A) the reaction between barium hydroxide and nitric acid
B) the reaction between calcium chloride and nitric acid
C) the reaction between barium hydroxide and sodium chloride
D) the reaction between barium chloride and sodium sulfate
E) the reaction between sodium carbonate and hydrochloric acid
Diff: 3
Section: 4.6
85) Which set contains compounds that are all soluble in water?
A) BaCO3, NaBrO3, Ca(OH)2, and PbCl2
B) NaCl, BaCl2, NH4NO3, and LiClO4
C) NiCO3, PbSO4, AgCl, and Mg(OH)2
D) NaCl, AgBr, Na2CO3, and Hg2(NO3)2
E) PbCl2, Pb(NO3)2, AgClO4, and HgCl2
Diff: 2
Section: 4.6
86) Which set of compounds are all insoluble in water?
A) BaCO3, NaBrO3, Ca(OH)2, and PbCl2
B) NaCl, BaCl2, NH4NO3, and LiClO4
C) NaCl, AgBr, Na2CO3, and Hg2(NO3)2
D) NiCO3, PbSO4, AgCl, and Mg(OH)2
E) PbCl2, Pb(NO3)2, AgClO4, and HgCl2
Diff: 2
Section: 4.6
87) Which set of compounds are all insoluble in water?
A) BaSO4, BaCl2, BaCO3, and Ba(OH)2
B) CrSO4, CrCl2, Cr(ClO4)2, and Cr(OH)2
C) Na2SO4, NaCl, Na2CO3, and NaOH
D) NiSO4, NiCl2, Ni(C2H3O2)2, and NiCO3
E) PbSO4, PbCl2, PbCO3, and Pb(OH)2
Diff: 2
Section: 4.6
88) Which reaction can be used to produce sulfur dioxide gas?
Hint: It may help to write out the formulas of each equation and determine products from there.
A) React aqueous barium hydroxide solution with aqueous sodium sulfite solution.
B) React aqueous nitric acid solution with aqueous sodium sulfate solution.
C) React aqueous nitric acid solution with concentrated sodium sulfide solution.
D) React aqueous sulfuric acid solution with solid sodium sulfite.
E) React solid barium sulfate with aqueous nitric acid solution.
Diff: 3
Section: 4.6
89) What is the net ionic equation for the reaction between HNO3 and Na2SO3?
Hint: Make sure to cancel out your spectator ions.
A) H2SO3(aq) → H2O + SO2(g)
B) HNO3(aq) + Na2SO3(aq) → H2O + SO2(g) + NO3-(aq)
C) 2H+(aq) + SO32-(aq) → H2O + SO2(g)
D) H2O + SO2(g) → H+(aq) + HSO3-(aq)
E) 2H+(aq) + Na2SO3(aq) → 2Na+(aq) + H2O + SO2(g)
Diff: 3
Section: 4.6
90) What is the molar concentration of a solution prepared by dissolving 0.100 mole of potassium nitrate in enough water to prepare 4.00 × 102 mL of the solution?
A) 2.50 × 10-4 M
B) 0.0400 M
C) 0.250 M
D) 4.00 M
E) 40.0 M
Diff: 1
Section: 4.7
91) Which solution is the least acidic?
A) 1.0 molar HCl
B) 1.0 molar H2SO4
C) 1.0 molar HClO4
D) 1.0 molar HNO3
E) 1.0 molar HCHO2
Diff: 2
Section: 4.7
92) Which solution is the least acidic?
A) 1.0 molar HCl
B) 1.0 molar HClO3
C) 1.0 molar HNO3
D) 1.0 molar HNO2
E) 1.0 molar HClO4
Diff: 2
Section: 4.7
93) Which solution is the least acidic?
A) 1.0 molar HF
B) 1.0 molar HCl
C) 1.0 molar HClO3
D) 1.0 molar HBr
E) 1.0 molar HI
Diff: 2
Section: 4.7
94) Which solution is the most acidic?
A) 1.0 molar HF
B) 1.0 molar HC2H3O2
C) 1.0 molar HCN
D) 1.0 molar HCl
E) 1.0 molar HNO2
Diff: 2
Section: 4.7
95) A 0.150 molar solution of sodium chloride in water is most accurately prepared in
A) a beaker.
B) an erlenmeyer flask.
C) a volumetric pipet.
D) a volumetric flask.
E) a florence (round bottom) flask.
Diff: 2
Section: 4.7
96) If 50.0 mL of 6.50 M H2SO4 is diluted to give a 1.30 M solution of H2SO4, what is the final volume of the diluted acid?
A) 1.30 × 102 mL
B) 135 mL
C) 25.0 mL
D) 3.00 L
E) 2.50 × 102 mL
Diff: 2
Section: 4.7
97) A solution is made by taking 54.62 grams of K2CrO4 in enough water to make 250.0 mL of solution. The molarity of the solution is therefore
A) 0.0002813 M.
B) 0.001125 M.
C) 0.2813 M.
D) 1.125 M.
E) 1.409 M.
Diff: 2
Section: 4.7
98) Sodium acetate, NaC2H3O2, has a formula weight of 82.034 g/mol. What is the molar concentration of a solution prepared by dissolving 4.10 grams of sodium acetate in enough water to prepare 2.50 × 102 mL of the solution?
A) 0.200 M
B) 1.03 M
C) 1.35 M
D) 5.00 M
E) 16.4 M
Diff: 2
Section: 4.7
99) Potassium nitrate, KNO3, has a formula weight of 101.10 g/mol. What is the molar concentration of a solution prepared by dissolving 7.58 grams of potassium nitrate in enough water to prepare 2.50 × 102 mL of the solution?
A) 0.0937 M
B) 0.300 M
C) 1.895 M
D) 3.065 M
E) 3.34 M
Diff: 2
Section: 4.7
100) What volume of 3.25 M (NH4)2SO4(aq) is needed in order to give 8.60 g of (NH4)2SO4?
A) 2.65 mL
B) 20.0 mL
C) 50.0 mL
D) 265 mL
E) 378 mL
Diff: 2
Section: 4.7
101) How many grams of NiSO47H2O would be required to prepare 5.00 × 102 mL of a solution that is 0.300 M in NiSO4(aq)?
Hint: Remember to use the correct units when dealing with Molarity.
A) 0.534 grams
B) 14.3 grams
C) 23.2 grams
D) 42.1 grams
E) 52.2 grams
Diff: 3
Section: 4.7
102) How many grams of Fe(NO3)3∙9H2O would be required to prepare 2.50 × 102 mL of a solution that is 0.100 M in Fe(NO3)3(aq)?
Hint: Remember to use the correct units when dealing with Molarity.
A) 6.05 grams
B) 10.1 grams
C) 14.3 grams
D) 20.2 grams
E) 52.2 grams
Diff: 3
Section: 4.7
103) How many grams of NH4NO3 would be required to prepare 0.500 L of a solution that is 
in NH4NO3(aq)?
A) 18.0 grams
B) 9.00 grams
C) 36.0 grams
D) 72.0 grams
E) 40.0 grams
Diff: 2
Section: 4.7
104) How many moles of MgCl2 would be required to prepare 0.750 L of a solution that is 0.350 M in MgCl2(aq)?
A) 2.86 moles
B) 0.467 moles
C) 2.14 moles
D) 263 moles
E) 0.263 moles
Diff: 1
Section: 4.7
105) How many mL of 2.0 M HCl solution would need to be diluted to produce 0.250 L of 0.8 M HCl?
A) 100 mL
B) 200 mL
C) 0.10 mL
D) 160 mL
E) 2.5 mL
Diff: 1
Section: 4.7
106) What volume of 0.250 M AgNO3(aq) is required to react with 35.0 mL of 0.210 M CaBr2(aq) in the reaction below?
2 AgNO3(aq) + CaBr2 (aq) → Ca(NO3)2(aq) + 2AgBr(s)
A) 25.0 mL
B) 12.5 mL
C) 37.5 mL
D) 58.8 mL
E) 103 mL
Diff: 2
Section: 4.8
107) 45.00 mL of an aqueous H2SO4 solution required 32.0 mL of 0.200 M KOH(aq) to neutralize it completely. The molarity of the H2SO4 solution is therefore
Hint: Write out the balanced neutralization reaction before beginning the problem.
A) 0.0711 M.
B) 0.142 M.
C) 0.200 M.
D) 0.281 M.
E) 0.284 M.
Diff: 3
Section: 4.8
108) A student wants to know how many mL of 0.300 M sulfuric acid is to be added to 50.0 mL of 0.250 M barium hydroxide solution to neutralize it completely.
Hint: Write out the balanced neutralization reaction before beginning the problem.
A) 20.8 mL
B) 30.0 mL
C) 41.7 mL
D) 60.0 mL
E) 110. mL
Diff: 3
Section: 4.8
109) In an experiment, 25.0 mL of 0.145 M H2SO4 react completely with 54.1 mL of a NaOH solution. What is the molar concentration (M) of the NaOH solution?
Hint: Write out the balanced neutralization reaction before beginning the problem.
A) 2.52 M
B) 0.134 M
C) 0.323 M
D) 1.67 M
E) 0.250 M
Diff: 3
Section: 4.8
110) What is the chloride ion concentration in a solution that is 0.255 M in aluminum chloride?
A) 0.0975 M
B) 3.05 M
C) 0.255 M
D) 1.55 M
E) 0.765 M
Diff: 2
Section: 4.8
111) What is the sodium ion concentration in a solution that is 0.175 M in sodium carbonate?
A) 0.0875 M
B) 0.350 M
C) 0.525 M
D) 0.175 M
E) 0.0583 M
Diff: 2
Section: 4.8
112) How many milliliters of 0.165 M aluminum chloride are required to react completely with 35.0 mL of 0.210 M silver nitrate? The net ionic equation is:
Ag+(aq) + Cl-(aq) → AgCl(s)
Hint: Consider that there are no coefficients necessary in the net ionic equation.
A) 105 mL
B) 35.0 mL
C) 14.8 mL
D) 6.55 mL
E) 44.5 mL
Diff: 3
Section: 4.8
113) How many mL of 0.200 M Na2SO4(aq) solution are required to completely react with 3.23 grams of BaCl2 (formula weight = 208.2 g/mol) to form products as shown below?
BaCl2(s) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)
A) 0.0155 mL
B) 0.0776 mL
C) 15.5 mL
D) 31.0 mL
E) 77.6 mL
Diff: 2
Section: 4.8
114) How many mL of 0.300 M NaOH(aq) solution are required to neutralize 1.858 g of KHC8H4O4 (formula weight = 204.22 g/mol) if the reaction is
NaOH(aq) + KHC8H4O4 → NaKC8H4O4(aq) + H2O(l)?
A) 30.3 mL
B) 4.55 mL
C) 45.5 mL
D) 75.9 mL
E) 550. mL
Diff: 2
Section: 4.8
115) How many mL of 6.00 M HCl(aq) solution are required to completely consume a 27.5 g sample of zinc metal (atomic weight = 65.39 g/mol) if the reaction is
Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)?
A) 126 mL
B) 140. mL
C) 280. mL
D) 1.26 × 103 mL
E) 2.52 × 103 mL
Diff: 2
Section: 4.8
116) A 25.0 mL sample of 0.200 M AgNO3(aq) was allowed to react with an excess of NaCl(aq). The AgCl precipitate from the reaction was carefully dried and weighed. How many grams of precipitate should be obtained?
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
A) 1.08 g
B) 0.432 g
C) 1.70 g
D) 3.13 g
E) 0.717 g
Diff: 2
Section: 4.8
117) A 100.0 mL sample of a 0.200 M aqueous solution of K2CrO4 was added to 100.0 mL of a 0.100 M aqueous solution of BaCl2. The mixture was stirred and the precipitate was collected, dried carefully, and weighed. How many grams of precipitate should be obtained? The reaction is
K2CrO4(aq) + BaCl2(aq) → BaCrO4(s) + 2 KCl(aq)
A) 2.05 g.
B) 2.53 g.
C) 5.07 g.
D) 6.16 g.
E) 7.60 g.
Diff: 2
Section: 4.8
118) NaHCO3 can be used to neutralize excess acid in situations such as, for instance, acid spills in the laboratory. The reaction is:
H+ (aq) + HCO3- (aq) → H2O (l) + CO2(g).
How many grams of NaHCO3 would be required to neutralize the acid in 75.5 mL of 1.00 M nitric acid?
A) 0.899 grams
B) 1.11 grams
C) 6.34 grams
D) 7.55 grams
E) 75.5 grams
Diff: 2
Section: 4.8
119) In a commercial laboratory, the acid in sulfuric acid waste can be readily neutralized using finely ground limestone chips. The reaction is:
H2SO4(aq) + CaCO3(s) → H2O(l) + CO2(g) + CaSO4(s)
A large bath holds 1.00 × 104 liters of solution, which is enough to fill 50 of the 2.00×102 liter drums. The acid content of the "neutralized" bath was determined to be 1.50 M in H2SO4. How many metric tons (1 metric ton = 1.000 × 103 kg) of CaCO3 would be the minimum amount to neutralize the acid in this bath?
A) 0.750 metric tons
B) 1.02 metric tons
C) 1.50 metric tons
D) 2.04 metric tons
E) 3.54 metric tons
Diff: 2
Section: 4.8
120) A 50.0 mL sample of a 0.200 M aqueous solution of Na3PO4 was added to 50.0 mL of a 
aqueous solution of BaCl2. The mixture was stirred and the precipitate was collected, dried carefully, and weighed. How many grams of precipitate should be obtained?
Hint: Write out the balanced equation and remember to use the correct units when dealing with molarity.
A) 1.00 g
B) 1.50 g
C) 3.01 g
D) 4.01 g
E) 9.03 g
Diff: 3
Section: 4.8
121) How many grams of lead(II) iodate, Pb(IO3)2 (formula weight = 557.0 g/mol), are precipitated when 3.20 × 102 mL of 0.285 M Pb(NO3)2(aq) are mixed with 386 mL of 0.512 M NaIO3(aq) solution?
Hint: Write out the balanced equation and remember to use the correct units when dealing with molarity.
A) 25.4 g
B) 39.8 g
C) 48.3 g
D) 50.8 g
E) 55.0 g
Diff: 3
Section: 4.8
122) A 3.50 g sample of solid Mg(OH)2 was treated with 50.0 mL of 0.500 M H2SO4(aq). After the reaction was over, some of the Mg(OH)2 remained undissolved. Calculate how many g of solid Mg(OH)2 remained.
Hint: Write out the balanced equation and remember to use the correct units when dealing with molarity.
A) 1.00 g
B) 1.46 g
C) 1.75 g
D) 2.04 g
E) 3.47 g
Diff: 3
Section: 4.8
123) A solid laboratory sample contains two substances, lead(II) carbonate and barium carbonate. A 5.000 g sample of this unknown was treated with aqueous nitric acid to dissolve it, then, after further treatment to adjust the acidity, it was treated with an excess of potassium chromate solution. The precipitate which formed, when dried carefully and weighed, has a mass of 6.276 grams. Calculate the percent, by weight, of lead(II) carbonate in this laboratory sample.
Hint: Remember to apply the solubility rules when determining the precipitate.
A) 34.60 %
B) 38.42 %
C) 45.91 %
D) 52.93 %
E) 67.38 %
Diff: 3
Section: 4.9
124) Morenosite is a hydrate of nickel sulfate with the formula NiSO4∙XH2O. A student was assigned to determine the value of X in the formula. This student took a 5.095 g sample of the hydrate, dissolved it in water and treated it with an excess of barium chloride solution. After carefully collecting the precipitate and drying it in an oven, he obtained a mass of 4.234 g for the precipitate. From this data, determine the value of X in the formula.
Hint: Remember to apply the solubility rules when determining the precipitate.
A) 4
B) 5
C) 6
D) 7
E) 8
Diff: 3
Section: 4.9
125) A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M KOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data.
Hint: Write out the neutralization reaction before proceeding with the problem.
A) 12.7 ml
B) 19.8 ml
C) 48.5 ml
D) 39.5 ml
E) 79.1 ml
Diff: 3
Section: 4.9
126) A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M NaOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the molarity of the sulfuric acid solution from this data.
Hint: Write out the neutralization reaction before proceeding with the problem.
A) 0.0842 M
B) 0.168 M
C) 0.244 M
D) 0.337 M
E) 0.597 M
Diff: 3
Section: 4.9
127) When 25.0 mL of sulfuric acid solution was completely neutralized in a titration with 0.050 M NaOH solution, it took 18.3 mL of the NaOH(aq) to complete the job. The unbalanced equation for the reaction is:
NaOH(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l)
What was the molarity of the sulfuric acid solution?
Hint: Don't forget to consider the coefficients of the balanced equation.
A) 0.0100 M
B) 0.0148 M
C) 0.0183 M
D) 0.0325 M
E) 0.0366 M
Diff: 3
Section: 4.9
128) Lactic acid (HC3H5O3) is a monoprotic acid that forms when milk becomes sour. A 40.00 mL sample of an aqueous lactic acid solution required 26.50 mL of 0.140 M NaOH(aq) to neutralize it by a titration. From this data, what is the molar concentration of lactic acid in the solution?
Hint: Write out the equation and be sure to use the correct units when dealing with molarity.
A) 0.0928 M
B) 0.148 M
C) 0.211 M
D) 0.757 M
E) 0.928 M
Diff: 3
Section: 4.9
129) Vinegar contains acetic acid (HC2H3O2), which is responsible for its acidity. In one analysis of a commercial vinegar brand, a 15.00 mL sample was titrated with 0.450 M NaOH(aq). It required 30.5 mL of sodium hydroxide to neutralize the acid in the vinegar sample. What is the molar concentration of acetic acid in the vinegar?
A) 0.102 M
B) 0.221 M
C) 0.305 M
D) 0.458 M
E) 0.915 M
Diff: 2
Section: 4.9
130) Ascorbic acid (Vitamin C, H2C6H6O6) is a diprotic acid. In a laboratory exercise, a vitamin C tablet was analyzed by titration using 0.125 M NaOH(aq). On the average, it required 29.5 mL of the base to neutralize the acid in the one tablet. How many mg of Vitamin C does one tablet contain?
Hint: Look at your units when calculating the final answer.
A) 100 mg
B) 162 mg
C) 273 mg
D) 325 mg
E) 649 mg
Diff: 3
Section: 4.9
131) A 2.710 g mixture contains CaCl2 — which does not react with HCl(aq) — and also CaO, which does react: CaO(s) + 2HCl(aq) → CaCl2 (aq) + H2O(l). It took 32.05 mL of 2.445 M HCl(aq) to react completely with all the CaO in the sample. The percent, by weight, of CaO in the sample is
Hint: Work backwards once you determine the amount of CaO present.
A) 35.15 %
B) 61.67 %
C) 77.62 %
D) 81.08 %
E) 84.17 %
Diff: 3
Section: 4.9
132) An ore containing lead carbonate, PbCO3, was analyzed. All of the lead in a 1.836 gram sample was converted to PbSO4(s) using a standard procedure involving treatment with HNO3(aq) followed by treatment with Na2SO4 solution. The lead sulfate which was recovered weighed 333 mg. What is the percent, by weight, of lead in the ore?
Hint: You should write out each reaction on paper and work backwards through the reactions.
A) 1.99 %
B) 12.4 %
C) 16.0 %
D) 18.1 %
E) 20.6 %
Diff: 3
Section: 4.9
133) A solid laboratory sample contains two substances, lead(II) carbonate and potassium carbonate. A 5.000 g sample of this unknown was treated with aqueous nitric acid to dissolve it, then, after further treatment to adjust the acidity, it was treated with an excess of potassium chromate solution. The precipitate which formed, when dried carefully and weighed, has a mass of 2.697 grams. Calculate the percent, by weight, of lead(II) carbonate in this laboratory sample.
Hint: You should write out each reaction on paper and work backwards through the reactions.
A) 44.60 %
B) 50.00 %
C) 65.91 %
D) 72.93 %
E) 77.38 %
Diff: 3
Section: 4.9
134) The formation of kidney stones is caused primarily by polyatomic anions such as
A) NO3- and CO32-.
B) PO43- and SO42-.
C) PO43- and C2O42-.
D) NO2- and HCO3-.
E) SO42- and SO32-.
Diff: 1
Section: Chemistry Outside the Classroom 4.1
135) Most kidney stones are made up of which substance?
A) sodium chloride
B) potassium sulfate
C) aluminum nitrate
D) sodium carbonate
E) calcium oxalate
Diff: 1
Section: Chemistry Outside the Classroom 4.1
136) The reaction most likely to lead to the formation of calcium bicarbonate in limestone regions is
A) the reaction between calcium chloride and sodium carbonate.
B) the reaction between sodium nitrate and carbonic acid.
C) the reaction between sodium hydroxide and acetic acid.
D) the reaction between calcium carbonate and carbonic acid.
E) the reaction between sodium carbonate and calcium carbonate.
Diff: 1
Section: Chemistry Outside the Classroom 4.2
137) The "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+, which are present in all ground water, can be removed by pretreating the water with
A) CaCl2.
B) KNO3.
C) Na2CO3∙10H2O.
D) PbSO4.
E) 0.0100 M HCl.
Diff: 1
Section: Chemistry Outside the Classroom 4.2
138) Which of the following sodium salts is a major component of soaps?
A) sodium chloride, NaCl
B) sodium nitrate, NaNO3
C) sodium acetate, NaC2H3O2
D) sodium stearate, NaC17H35O2
E) hydrated sodium carbonate, Na2CO3·10H2O
Diff: 2
Section: Chemistry Outside the Classroom 4.2
139) Boiler scale can be formed on the walls of hot water pipes from ground water due to
A) transformation of HCO3- ions to CO32- ions, which then form precipitates with the "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+.
B) transformation of HSO3- ions to SO32- ions, which then form precipitates with the "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+.
C) transformation of HSO4- ions to SO42- ions, which then form precipitates with the "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+.
D) transformation of H2PO4- ions to PO43- ions, which then form precipitates with the "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+.
E) reaction of the CO32- ions present in all ground water with the "hardness ions", Ca2+, Mg2+, Fe2+/Fe3+.
Diff: 2
Section: Chemistry Outside the Classroom 4.2
140) In a ________ solution, the ratio of solute to solvent is quite small.
Diff: 1
Section: 4.1
141) If a seed crystal is dropped into a supersaturated solution, a ________ is expected to form.
Diff: 1
Section: 4.1
142) How many ions per formula unit are produced by dissociation when (NH4)3AsO4 dissolves in water?
Diff: 2
Section: 4.2
143) How many ions per formula unit are produced by dissociation when Hg2SO4 dissolves in water?
Diff: 2
Section: 4.2
144) Write out the equation for the dissociation of MgCl2 when it dissolves in water. Include all states.
Diff: 1
Section: 4.2
145) Write out the equation for the dissociation of sodium carbonate when it dissolves in water. Include all states.
Diff: 2
Section: 4.2
146) Write out the equation for the dissociation of potassium dichromate when it dissolves in water. Include all states.
Diff: 2
Section: 4.2
147) How many ions are formed when sodium thiosulfate dissolves in water?
Diff: 2
Section: 4.2
148) How many ions are formed when potassium oxalate dissolves in water?
Diff: 2
Section: 4.2
149) Write the net ionic equation for the reaction which occurs when HClO4(aq) reacts with Ba(OH)2(aq).
Diff: 2
Section: 4.3
150) Write the net ionic equation for the reaction which occurs when potassium sulfate (K2SO4) reacts with barium nitrate (Ba(NO3)2) to form a precipitate. Include states in the equation.
Diff: 2
Section: 4.3
151) Write the net ionic equation for the reaction which occurs when silver nitrate (AgNO3) reacts with sodium chloride (NaCl) to form a precipitate. Include states in the equation.
Diff: 2
Section: 4.3
152) What are the spectator ions for the reaction which occurs when silver nitrate (AgNO3) reacts with sodium chloride (NaCl) to form a precipitate.
Diff: 2
Section: 4.3
153) All acids share the common property of reacting with water to produce ________.
Diff: 2
Section: 4.4
154) Ionization differs from dissociation in that in ionization no ________ exist prior to their formation.
Diff: 2
Section: 4.4
155) Write the equation for the ionization of perchloric acid with water.
Diff: 2
Section: 4.4
156) Acids that contain hydrogen, oxygen, and a nonmetallic element are called ________.
Diff: 2
Section: 4.4
157) According to the Arrhenius definitions of an acid, all acids produce ________ when added to water.
Diff: 2
Section: 4.4
158) When SO2(g) is dissolved in water, the name of the acid that is formed is ________
Diff: 2
Section: 4.4
159) Write the equation for the ionization of formic acid (HCHO2), a weak acid, with water.
Diff: 2
Section: 4.4
160) Write the equation for the ionization of hydrocyanic acid (HCN), a weak acid, with water.
Diff: 2
Section: 4.4
161) Write the equation for the ionization of ammonia (NH3), a weak molecular base, with water.
Diff: 2
Section: 4.4
162) Write the equation for the ionization of ethylamine (C2H5NH2), a weak molecular base, with water.
Diff: 2
Section: 4.4
163) When HI(g) is dissolved in water, the name of the acid that is formed is ________
Diff: 2
Section: 4.5
164) When HF(g) is dissolved in water, the name of the acid that is formed is ________
Diff: 2
Section: 4.5
165) When H2S (g) is dissolved in water, the name of the acid that is formed is ________.
Diff: 2
Section: 4.5
166) What is the name of the oxoacid HNO2?
Diff: 1
Section: 4.5
167) What is the name of the oxoacid HClO3?
Diff: 1
Section: 4.5
168) What is the formula for the oxoacid perchloric acid?
Diff: 1
Section: 4.5
169) What is the formula for the hydrocyanic acid?
Diff: 1
Section: 4.5
170) When HCl and NaOH are mixed in a 1-to-1 ratio, an ________ reaction occurs.
Diff: 1
Section: 4.6
171) What is the formula for sodium dihydrogen phosphate?
Diff: 2
Section: 4.6
172) The reaction between aqueous sulfuric acid and solid calcium carbonate produces which gas?
Diff: 2
Section: 4.6
173) Write the net ionic equation for the reaction of hydrochloric acid and potassium hydroxide. Include all states.
Diff: 2
Section: 4.6
174) Write the net ionic equation for the reaction of nitric acid and ammonia. Include all states.
Diff: 2
Section: 4.6
175) Write the net ionic equation for the reaction of perchloric acid and calcium carbonate. Include all states.
Hint: Remember to remove spectator ions.
Diff: 3
Section: 4.6
176) Write the net ionic equation for the reaction of acetic acid and sodium hydroxide. Include all states.
Hint: Remember to remove spectator ions.
Diff: 3
Section: 4.6
177) Write the net ionic equation for the reaction of formic acid (HCHO2) and ammonia (NH3). Include all states.
Diff: 2
Section: 4.6
178) Addition of a sodium sulfate solution to a solution containing three solutes—silver nitrate, ammonium nitrate, and barium nitrate—will cause the formation of what precipitate?
Diff: 2
Section: 4.6
179) Addition of a sodium hydroxide solution to a solution containing three solutes—lead nitrate, ammonium nitrate, and silver nitrate—will cause the formation of what precipitate?
Diff: 2
Section: 4.6
180) Students in a laboratory class were provided with 6.00 M hydrochloric acid solution from the stockroom. The instructions in the experiment called for 2.50 × 102 mL of 2.00 M hydrochloric acid per student. How many milliliters of the 6.00 M solution should be used to prepare enough hydrochloric acid solution for a lab class with 12 students, if one student is assigned the task of preparing the batch and needs to make 25.0% more than actually needed?
Hint: Remember the units of molarity when solving this problem.
Diff: 3
Section: 4.7
181) A student in laboratory was provided with 6.00 M of hydrochloric acid solution. The instructions call for 2.50 × 102 mL of 2.00 M hydrochloric acid solution. How many mL of the 6.00 M solution should be used to prepare 5.00×102 mL of the 2.00 M solution?
Diff: 2
Section: 4.7
182) How many grams of CaCl2 are needed to prepare a 1.10 L solution of 0.250 M CaCl2?
Diff: 2
Section: 4.7
183) How many mL of 2.50 M HNO3 are needed to prepare a 75.0 mL of 1.00 M HNO3?
Diff: 2
Section: 4.7
184) Each of the following solutions was treated with 0.10 M of H2SO4(aq). How many of the solutions will show a reaction?
0.10 M Ba(NO3)2(aq) 0.10 M Ca(NO3)2(aq)
0.10 M AgNO3(aq) 0.10 M Pb(NO3)2(aq)
0.10 M Zn(NO3)2(aq)
Hint: Consider spectator ions when determining if a reaction takes place.
Diff: 3
Section: 4.6
185) Each of the following solutions was treated with 1.00 M of H2SO4(aq). How many solutions will show a reaction?
0.10 M Na2SO3(aq) 0.10 M NH4NO3(aq)
0.10 M K2S(aq) 0.10 M Li3PO4(aq)
0.10 M Ni(ClO4)2(aq)
Hint: Consider spectator ions when determining if a reaction takes place.
Diff: 3
Section: 4.6
186) Each of the following solutions was treated with 0.500 M of Na2CO3(aq). How many solutions will show a reaction?
1.00 M H2SO4(aq) 1.00 M Ni(NO3)2(aq)
1.00 M BaCl2(aq) 1.00 M AgNO3(aq)
1.00 M K2SO4(aq)
Hint: Consider spectator ions when determining if a reaction takes place.
Diff: 3
Section: 4.6
187) How many grams of MgCl2 would be required to prepare 0.750 L of a solution that is 0.350 M in chloride ions?
A) 33.0 g
B) 58.7 g
C) 12.5 g
D) 66.1 g
E) 29.4 g
Diff: 1
Section: 4.8
188) A 250.0 mL sample of a solution containing potassium dichromate as the only solute was evaporated to dryness, then the residue was carefully dried in the oven at the recommended temperature. The oven-dried residue weighed 16.58 grams. What was the molarity of the potassium dichromate solution?
Hint: Remember the molarity formula is moles of solute/liters of solution.
Diff: 3
Section: 4.7
189) In the course of a titration of barium ion in a sample by sulfate ion in a titrant solution, 83.5 mL of 0.200 M Na2SO4(aq) was required to precipitate all the barium ions. How many grams will the dried precipitate weigh?
Hint: Remember the molarity formula is moles of solute/liters of solution.
Diff: 3
Section: 4.9
190) A solute is any substance that is dissolved in a solvent and the solute can be a solid, liquid, or gas.
Diff: 2
Section: 4.1
191) A solution that has less solute than is required for saturation is considered supersaturated.
Diff: 2
Section: 4.1
192) If a seed crystal is dropped into an unsaturated solution the formation of a precipitate is expected to form.
Diff: 1
Section: 4.1
193) When solid calcium nitrate dissolves in water, the process can be represented by the equation, Ca(NO3)2(s) → Ca2+(l) + 2 NO3(l).
Diff: 1
Section: 4.2
194) When solid nickel sulfate dissolves in water, the process can be represented by the equation, NiSO4(s) → Ni2+(aq) + S2(aq) + 2 O2(g).
Diff: 1
Section: 4.2
195) Spectator ions are ions that are used to make the precipitate in an ionic reaction.
Diff: 1
Section: 4.3
196) The symbol, H+(aq), is often used as a substitute for H2(aq).
Diff: 1
Section: 4.4
197) As a very important precaution, it is always advisable to taste an acid before using it in the laboratory.
Diff: 1
Section: 4.4
198) HNO2 is a strong acid.
Diff: 1
Section: 4.4
199) The compound, HBrO3, is named hydrogen bromate acid.
Diff: 2
Section: 4.5
200) The compound, Ca(OH)2, is named calcium dihydrogen oxide.
Diff: 2
Section: 4.5
201) All sulfates are insoluble except those of Group IA, Group IIA, and Al3+.
Diff: 2
Section: 4.6
202) Mixing an aqueous ammonium chloride solution with an aqueous barium nitrate solution will cause formation of a precipitate.
Diff: 2
Section: 4.6
203) Addition of a sodium sulfate solution to a solution containing three solutes—silver nitrate, ammonium nitrate, and barium nitrate—will cause formation of a precipitate.
Diff: 2
Section: 4.6
204) When a solution of sodium carbonate is mixed with a solution of nitric acid, a precipitate will form.
Diff: 2
Section: 4.6
205) When a solution of nitric acid is mixed with a solution of sodium sulfate, a gas is formed and escapes from the mixture.
Diff: 2
Section: 4.6
206) Nitric acid will dissolve a solid sample of calcium carbonate and no solid residue will remain.
Diff: 2
Section: 4.6
207) An aqueous solution contains one solute which is either sodium carbonate, sodium sulfate, or potassium nitrate. Addition of a barium chloride solution to a sample of the solution did not cause any visible chemical change. A student stated that it is possible to tell exactly which solute is present from this preliminary test. Is this true or false?
Diff: 2
Section: 4.6
208) A 0.540 M aqueous solution of sodium tetrafluoroborate (molar mass = 109.79 g mol-1) contains 14.82 grams of solute in 2.50 × 102 mL of solution.
Diff: 2
Section: 4.7
209) The mass of K2Cr2O7 (molar mass = 294.19 g mol-1) needed to make 235 mL of a 0.170 M solution, is 117 g.
Diff: 2
Section: 4.7
210) The molar concentration of aluminum ions in 0.10 M aluminum sulfate is 0.10 M.
Diff: 2
Section: 4.8
211) If the molar concentration of sodium ions is 0.44 M, then the concentration of sodium sulfate is 0.88 M.
Diff: 2
Section: 4.8
212) In quantitative analysis, the goal is always to determine what substances are present, without necessarily measuring the amounts of each substance.
Diff: 2
Section: 4.9
213) 50.0 mL of a solution of 0.200 M HNO3 will exactly neutralize 25.0 mL of a solution of 0.200 M Ca(OH)2.
Diff: 2
Section: 4.9
214) Kidney stones are formed via precipitation reactions.
Diff: 1
Section: Chemistry Outside the Classroom 4.1
215) Kidney stones are likely to contain calcium phosphate.
Diff: 2
Section: Chemistry Outside the Classroom 4.1
216) Limestone deposits are primarily composed of calcium carbonate.
Diff: 2
Section: Chemistry Outside the Classroom 4.2
217) Rain and natural waters dissolve CO2 from the atmosphere, causing the water to be slightly acidic because Na2CO3 is formed.
Diff: 2
Section: Chemistry Outside the Classroom 4.2
218) A solution is sitting undisturbed on a side shelf in the laboratory. A small crystal of solute from which the solution is made was gently dropped into the solution. Suddenly, a mass of crystals forms and settles to the bottom of the container. Which word best describes the solution?
Diff: 2
Section: 4.1
219) A student is trying to prepare a sample of solid lead sulfate for an experiment. He requests sodium sulfate and lead iodide from the store room. He is told this will not work to make a lead sulfate precipitate. Explain why.
Hint: Consider the solubility rules for this problem.
Diff: 3
Section: 4.3
220) CH3NH2 ionizes when dissolved in water. What is the acidic species formed when CH3NH2 ionizes in water?
Hint: Write the reaction out on paper to help visualize the products.
Diff: 3
Section: 4.4
221) List the seven common strong acids.
Diff: 2
Section: 4.4
222) Oxalic acid (H2C2O4) is a diprotic acid found in Rhubarb leaves. Write out the ionization reactions for oxalic acid when it reacts with water. Give the states involved.
HC2O4- (aq) + H2O (l) C2O42- (aq) + H3O+ (aq)
Diff: 2
Section: 4.4
223) What is the name of the oxoacid formed when CO2(g) is dissolved in water?
Diff: 2
Section: 4.5
224) What is the name of the salt formed from the neutralization of chloric acid (HClO3) with NaOH?
Diff: 2
Section: 4.6
225) Give the formula of the polyatomic ion formed from the complete neutralization of sulfurous acid (H2SO3).
Diff: 2
Section: 4.6
226) An aqueous solution contains one unknown solute which is either sodium carbonate, sodium sulfate, or potassium nitrate. Addition of a barium chloride solution to a sample of the solution did not cause any visible chemical change. What is the identity of the unknown solute?
Hint: Consider the net ionic reactions for each of the compounds with barium chloride.
Diff: 3
Section: 4.6
227) An aqueous solution contains one unknown solute which is either sodium hydroxide, ammonium sulfate, or silver nitrate. Addition of a potassium chloride solution to a sample of the solution causes a precipitate to form. What is the identity of the unknown solute?
Hint: Consider the net ionic reactions for each of the compounds with potassium chloride.
Diff: 3
Section: 4.6
228) A dry lab exercise was worded as follows. Three solutions, labeled A, B, and C, each contain one solute. One is barium chloride, one is sodium sulfate, and one is potassium nitrate. Devise a scheme in which you mix a few drops of one with a few drops of another, record the results you observe, and determine which solution is which.
Diff: 2
Section: 4.6
229) A 66.7 mL sample of 18.0 M sulfuric acid was diluted with enough water in a volumetric flask to make 5.00×102 mL of solution. A 25.0 mL aliquot of this solution was then further diluted to a volume of 1.50×102 mL. What is the molarity of the solution after the second dilution?
Hint: Take it one step at a time when calculating the dilutions. Don't mix up your values.
Diff: 3
Section: 4.7
230) How many mL of 0.446 M KMnO4(aq) are required to react with 50.0 mL of 0.200 M H2C2O4(aq) in the presence of H2SO4(aq)? The unbalanced equation for the reaction is:
KMnO4(aq) + H2C2O4(aq) + H2SO4(aq) → MnSO4(aq) + CO2(g) + H2O + K2SO4(aq)
Hint: Be sure to balance the equation.
Diff: 3
Section: 4.8
231) A friend who is working part time as a technician in a chemical manufacturing plant needs help with this problem. He has 6.00 M of aqueous sulfuric acid and 0.500 M of aqueous sulfuric acid. The water supply has been shut off, and he wants to make up 2.000 liters of 1.20 M aqueous sulfuric acid from just the two reagents above. How many mL of each should he take to make up the 2.000 liters?
Diff: 3
Section: 4.7
232) A finely powdered sample is a mixture containing NaCl and KCl. A 4.624 gram sample of the mixture was dissolved in 80.00 mL of water and treated with 0.264 M AgNO3(aq). It required 277.0 mL of the AgNO3(aq) solution to combine with all of the chloride ion present. The percent, by weight, of NaCl in the mixture is therefore ________ % .
Hint: Write the reaction out and balance it to help with your calculations.
Diff: 3
Section: 4.9
233) Hydrochloric acid solution can be neutralized by using lime (CaO). The unbalanced equation for the reaction is:
HCl(aq) + CaO(s) → CaCl2(aq) + H2O(l).
How many kg of CaO (formula mass = 56.077) are required for neutralization of 35.50 gallons of 2.40 M HCl(aq)?
Diff: 2
Section: 4.8
234) Vinegar contains acetic acid (HC2H3O2), which is responsible for its acidity. In one analysis of a commercial (off the shelf) vinegar brand, a 15.00 mL sample was titrated with 0.450 M NaOH(aq). It required 30.5 mL of this sodium hydroxide titrant to neutralize the acid in the vinegar sample. If 1.000 liter of this vinegar weighs 1.004 kg, what is the percent, by weight, of acetic acid in this vinegar brand?
Hint: Write the reaction out and balance it to help with your calculations.
Diff: 3
Section: 4.9
235) A student in a laboratory performed a titration to find out the exact molarity of her unknown KOH(aq) solution. She weighed out 2.465 g of KHC8H4O4, dissolved it in 100 mL of water and titrated it with the base. The equation for the reaction is:
OH-(aq) + HC8H4O4-(aq) → H2O + C8H4O42-(aq)
The titration showed that 42.5 mL of the base were required to neutralize the KHC8H4O4 sample. What is the molarity of the potassium hydroxide solution?
Diff: 2
Section: 4.9
236) A solid diprotic acid, H2A, has a molar mass which is being determined in this question. Following the procedure, a student weighed out 0.647 grams of the H2A sample, dissolved it in 50.0 mL of water and titrated it with 0.235 molar sodium hydroxide solution. It required 37.45 mL of the base to exactly neutralize the H2A sample. Based on this data, what is the molar mass of H2A to three significant digits?
Hint: Write the reaction out and balance it to help with your titration calculations.
Diff: 3
Section: 4.9
237) The average stomach holds around 1 liter of liquid and contains 0.01 M HCl (stomach acid). A typical antacid tablet contains 750 mg of calcium carbonate. If we assume someone has a full stomach, how many antacid tablets would a person need to neutralize all the acid in their stomach? Assume that no new acid is produced.
Hint: Write out the neutralization reaction before performing your calculations.
Diff: 3
Section: 4.8
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