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Chapter 5
Introduction to Reactions in Aqueous Solutions
 
 
 
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 Mobile ions are conductors of electricity
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 Animation: Electrolytes and Non-Electrolytes (*) In NaCl crystals the ions which are held in place by interactions between ions in the crystal lattice and cannot move in an electrical field. When NaCl is dissolved in water the water associates with the ions and separates them, allowing them to move freely in the solution. These mobile ions are good conductors of electricity. An aqueous solution of a nonelectrolyte such as sugar which contains no ions does not conduct electricity.
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 Conductivity of a strong and a weak electrolyte
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 Demonstration: Strong and Weak Electrolytes (***) This experiment shows that pure water does not conduct electricity. When gaseous HCl is dissolved in H2O, the acid dissociates to give H3O+ ions and Cl- ions, which conduct electricity. Acetic acid, a weak acid,is only partially ionized in aqueous solution, so there are fewer ions in solution to conduct electricity. This causes the light to glow less than it did in the HCl solution.
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 The dissociation of HCl, HNO3 and acetic acid in aqueous solution is illustrated using a single molecule of each.
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 Animation: Introduction to Aqueous Acids (*) HCl and HNO3 are strong acids. The complete dissociation of a single molecule of HCl and HNO3 is demonstrated. The partial ionization of a single molecule of acetic acid is also demonstrated in this animation.
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 The dissociation of NaOH and the reaction of NH3 with H2O are illustrated using a single formula unit of each substance.
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 Animation: Introduction to Aqueous Bases (*) Strong and weak bases are illustrated using NaOH and NH3, respectively. The complete dissociation of a strong base is illustrated using a single formula unit of NaOH as an example. One molecule of NH3 and one molecule of H2O are used to show that NH3 is a weak base and that most of the NH3 in aqueous solution is not ionized.
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 The exothermic reaction between Fe2O3 and aluminum is demonstrated.
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 Demonstration: Thermite (***) In the thermite reaction, Al reduces Fe2O3 to Fe in an extremely exothermic reaction in which Al is oxidized to Al2O3. The reaction produces enough heat to melt the iron. Because of the extreme heat produced in the thermite reaction, it is used industrially to weld iron.
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 Copper oxide reacts with carbon to form copper and carbon dioxide
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 Demonstration: Reduction of CuO (**) When black carbon and black copper oxide are heated together the Cu2+ ions are reduced to metallic Cu and a gas is evolved. When the gas is collected in Ca(OH)2 a white precipitate of CaCO3 is formed. The reaction which occurs involves the reduction of Cu2+ ions by carbon which is oxidized to CO2.
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 Demonstration of the reaction between sodium and chlorine to form sodium chloride
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 Demonstration: Formation of Sodium Chloride (***) Molten sodium burns when it is put into a container of chlorine gas. In the reaction a sodium ion loses an electron to form a sodium cation and a chlorine atom simultaneously gains an electron to form a chloride anion. The product of the reaction is the ionic compound sodium chloride, which is the white solid observed.
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 Oxidation of Zn by O2
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 Animation: Redox Reactions - Part 1 (*) Oxidation is a loss of electrons and reduction is a gain of electrons. The oxidation of metallic Zn by O2 to form ZnO(s) is illustrated at the molecular level. The transfer of electrons from Zn to O2 is shown. atoms can be observed to change as they are oxidized or reduced, respectively to their ionic forms.
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 Oxidation of Zn by H+ and by Cu2+
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 Animation: Redox Reactions - Part 2 (*) The oxidation of zinc by H+ ions which are reduced to form H2 gas is demonstrated at the molecular level. The reduction of Cu2+ by Zn, which is oxidized, is also illustrated. In both reactions, Zn is the reducing agent and the substances reduced by Zn are oxidizing agents. The differences in the sizes of Zn and Zn2+ and Cu2+ and Cu are illustrated
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 The reduction of Ag+ by Cu is demonstrated.
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 Demonstration: Formation of Silver Crystals (**) When a copper wire is placed in a solution of AgNO3, the Cu reduces Ag+ to metallic Ag. At the same time, Cu is oxidized to Cu2+. As the reaction progresses Ag crystals can be seen to form on the Cu wire and the solution becomes blue as a result of the formation of Cu2+ ions.
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 Redox reaction between Sn2+ and Zn
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 Demonstration: Redox Chemistry of Sn and Zn (*) When acidified SnCl2 is added to a beaker containing a piece of Zn, some of the Sn2+ reacts with H+ in the solution to produce H2 gas. Immediate changes can also be observed on the surface of the Zn as it quickly becomes coated with Sn crystals. After the reaction has progressed for a time needles of Sn can be observed on the surface of the Zn.
5.2
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 05.02
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 Beaker of liquid with power source attached to electrodes in the liquid - showing ions in solution
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5.3.1UN
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 Hydronium ion
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5.4.1UN
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 Formation of AgBr from KBr and AgNO3
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5.6.1UN
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 Space filling model of ammonium ion (for Visualization VIS 5-01)
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5.6.2UN
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 05.06.02
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 This marble statue has been eroded by acid rain. Marble is a material having CaCO3 as its primary component. Acids react with and dissolve the marble through the reaction described in Equation (5.10).
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5.9
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 Oxidation states of Nitrogen
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5.11.3UN
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 05.11.03
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 space filling models for chapter 5, exercise 29
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5.11.8UN
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 05.11.08
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 graph with conductance and volume of NaOH with equivalence point
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Table 5.1
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 Table 5.1
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Table 5.2
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 Table 5.2
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Table 5.3
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 Table 5.3
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