Chapter 4 Types of Chemical Reactions and Solutions Stoichiometry

Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–2 QUESTION

Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–3 ANSWER 2)Polar Section 4.1 Water, the Common Solvent (p. 127) The solubility rule for molecular compounds is “like dissolves like”, that is, polar molecules dissolve in polar solvents and nonpolar molecules dissolve in nonpolar solvents.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–5 ANSWER 2)5.11 g Section 4.3 The Composition of Solutions (p. 133) Volume(L) times concentration(mol/L) gives moles. Moles are then converted to grams.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–7 ANSWER M  12 V, V 1)168 mL Section 4.3 The Composition of Solutions (p. 133) Use the dilution formula, 1 V = M  2 M is in mol/L and is in L.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–9 ANSWER – 3)3OH(aq) Section 4.6 Describing Reactions in Solution (p. 145) The net ionic equation is found by canceling the spectator ions from the total ionic equation.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–11 ANSWER 4 : 3)HClO Section 4.2 The Nature of Aqueous Solutions Strong and Weak Electrolytes (p. 129) Memorization of the list of strong acids will allow one to determine the difference between strong acids and weak acids.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–13 ANSWER. 2)HBr Section 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes (p. 129) Knowing the list of strong acids will allow one to determine which acids are strong and which are weak.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–15 ANSWER 3 3)NH Section 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes (p. 129) Knowing the list of strong bases will allow one to determine which bases are strong and which are weak.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–17 ANSWER. 1)hydration Section 4.1 Water, the Common Solvent (p. 127) Hydration is the process of water molecules surrounding and stabilizing ions so that they can be pulled into solution.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–19 ANSWER 2)False Section 4.3 The Composition of Solutions (p. 133) The amount of water decreases over time so the concentration (mol NaCl/volume of water) increases over time.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–21 QUESTION (continued)

Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–22 ANSWER )precipitation, redox, and acidbase reactions, respectively. Section 4.5 Precipitation Reactions (p. 140) PbI is insoluble, Ce changes to Ce and HOAc is an acid while NH is a base.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–24 ANSWER 5)All of these are soluble in water. Section 4.5 Precipitation Reactions (p. 140) According to the solubility rules for ionic compounds, compounds containing Group IA ions or nitrate ions will always be soluble. Compounds containing halides are generally soluble, aside from silver, leadand mercury(I) halides.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–26 ANSWER 2 s 3  4 + 3)Cu(OH) Section 4.4 Types of Chemical Reaction (p. 140) Ammonia produces hydroxide ion in water: NH + H 2 O NH+OH –

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–28 ANSWER 5) Na 2 SO 4 + 2H 2 O Section 4.8 Acid-Base Reactions (p. 149) The salt is made from the anion of the acid and the cation of the base.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–30 ANSWER )2.4 g Section 4.8 AcidBase Reactions (p. 149) Remember that the reaction is 2NaOH + HSO  NaSO + 2HO, so there are two moles of NaOH used per one mole of HSO 4.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–32 ANSWER 2 - – 2 O 2 2)NO Section 4.9 OxidationReduction Reactions (p. 154) Oxygen almost always has an oxidation state of 2 when part of a compound. The exception is when it is part of a peroxide. For example, hydrogen peroxide H. Then it has an oxidation state of –1.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–34 ANSWER - 2)the oxidizing agent. Section 4.9 OxidationReduction Reactions (p. 154) Metals lose electrons, so they are oxidized, making the other reactant an oxidizing agent.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–36 ANSWER. - 5)1, 3, and 4 are true Section 4.9 OxidationReduction Reactions (p. 154) (2) is false because certain reactions, such as double displacement reactions, are not redox reactions.

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Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–38 QUESTION (continued)

Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 4–39 ANSWER - 3) 2 Section 4.9 OxidationReduction Reactions (p. 154) If an element is found on the reactant’s side, this is almost always a redox reaction, since an element usually becomes part of a compound during a chemical reaction.